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Gas phase methanol synthesis for carbon-11 radiopharmaceuticals Van Lier, Erik 2007

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GAS PHASE METHANOL SYNTHESIS FOR CARBON-11 RADIOPHARMACEUTICALS by Erik van Lier B.Eng., McGill University, May 2001 A THESIS SUBMITTED IN PARTIAL FULFILLMENT OF THE REQUIREMENTS FOR THE DEGREE OF MASTER OF APPLIED SCIENCE in THE FACULTY OF GRADUATE STUDIES (Chemical and Biological Engineering) THE UNIVERSITY OF BRITISH COLUMBIA August 2007 © Erik van Lier, 2007 Abstract Carbon-11 radiopharmaceuticals are gaining an increasing importance in positron emission tomography due to their importance in diagnostic medicine. The most wide spread method of production of these radiopharmaceuticals is by methylation of an appropriate precursor with the highly reactive [nC]methyl iodide. Conventional synthesis of this intermediate involves liquid phase synthesis of [nC]methanol, which is the step that limits the specific activity of the final product. A catalytic gas phase methanol synthesis process was eval uated, that promises to avoid the loss of specific activity. In this procedure, [nC]carbon dioxide produced in the target is first trapped and purified, then converted to [nC]carbon monoxide using molybdenum and finally reduced to [nC] methanol using a copper zinc oxide catalyst in the presence of hydrogen. In this study a device to trap and purify [nC]carbon dioxide was developed and opti mized. [nC] Carbon dioxide produced in target was quantitatively trapped at -20° C on a carbon molecular sieve column and quantitatively released in less than 3.5 minutes. A reactor to convert 50 ppm carbon dioxide to carbon monoxide, based on the reaction with molybdenum, was developed. A commercially available process simulator was used to assist the optimization of operating conditions and molybdenum pretreatment methods. Under optimal conditions, carbon dioxide was converted to carbon monoxide with over 70% yield. A reactor to catalytically convert 50 ppm carbon monoxide to methanol was developed. A copper zinc oxide catalyst was prepared by a co-precipitation method. The catalyst was ii activated by reduction with hydrogen and passivated with compressed air prior to methanol synthesis. The effect of temperature, pressure and flowrate on the conversion of carbon monoxide to methanol were studied and results were used to create a kinetic model. This model was used to determine optimal operating conditions for this reactor and predicts 60% conversion of [nC]carbon monoxide to [nC]methanol. These findings suggest that gas phase [nC] methanol synthesis is a viable alternative to the conventional liquid phase method, meriting further studies with carbon-11. iii Contents Abstract «' Nomenclature x Acknowledgements xv 1 Introduction 1 1.1 Background1.1.1 Positron emission tomography 2 1.1.2 Application of PET 7 1.1.3 Carbon-11 radiopharmaceuticals 8 1.2 Objective of the study 9 2 Literature review 11 2.1 Radiochemistry of carbon-11 12.1.1 Production of C-11 2 2.1.2 Recovery and purification of nC02 and nCH4 14 2.1.3 Reduction of nC02 and oxidation of UCH4 17 2.1.4 Synthesis of uCH3OH 20 2.1.5 Synthesis of carbon-11 radiopharmaceuticals 22 2.2 Molybdenum compounds for the reduction of C02 to CO 23 2.2.1 History 2iv 2.2.2 Reduction of molybdenum oxides . 24 2.2.3 Oxidation of molybdenum 26 2.2.4 Interaction of C02 and CO with Mo2C 27 2.3 Methanol synthesis 30 2.3.1 History2.3.2 Catalyst preparation 31 2.3.3 Catalyst poisoning / deactivation 32 2.3.4 Thermodynamics and kinetics3 Experimental: Trapping and purification of11C02 34 3.1 Introduction 33.2 Materials and methods 35 3.3 Experimental set-up . ; '. 36 3.4 Experimental procedure 33.4.1 Production of11C02 . 7 3.4.2 Trapping and release of11C02 39 3.5 Results and discussion 40 3.5.1 Effect of carbon molecular sieve mass on 11C02 trapping efficiency 41 3.5.2 Effect of trap temperature on C02 trapping efficiency 42 3.5.3 Overall trapping efficiency 43 4 Experimental: Reduction of C02 to CO 44 4.1 Introduction 44.2 Preliminary experiments: reaction of nC02 and Mo 44 4.2.1 Materials and methods 44.2.2 Experimental set-up 5 4.2.3 Experimental procedure 46 4.2.4 Results and discussionv 4.3 Equilibrium computer simulations of systems containing molybdenum . . 48 4.3.1 Reduction of Mo03 with H2 49 4.3.2 Oxidation of Mo with 02 50 4.4 Cold experiments: reaction of C02 and Mo 54 4.4.1 Introduction 54.4.2 Materials and methods 55 4.4.3 Experimental set-up 6 4.4.4 Experimental procedure 57 4.4.5 Results and discussion 9 5 Experimental: Methanol synthesis 65 5.1 Introduction 65.2 Materials and methods 66 5.2.1 Cu/ZnO catalyst preparation 67 5.3 Experimental procedure 68 5.3.1 Preliminary experiments: Cu/ZnO catalyst for CH3OH synthesis . . 68 5.3.2 Effect of flowrate and temperature on CH3OH synthesis 69 5.4 Results and discussion: 71 5.4.1 Preliminary experiments: Cu/ZnO catalyst 71 5.4.2 Effect of flowrate and temperature on CH3OH synthesis 73 5.4.3 Kinetic Model 76 6 Conclusion and Recommendations 80 6.1 Conclusions 86.2 Recommendations for future work 81 Bibliography 3 vi Appendices 91 Appendix I: Flowmeter calibration curves 9Appendix II: Calibration curves 93 Appendix III: Surface molybdenum 6 Appendix IV: Temperature profile 98 Appendix V: Process simulator 100 Appendix VI: Carbon dioxide estimate 105 vii List of Tables 3.1 C-l 1 target yields, 14 MeV 40 3.2 nC02 trapping/releasing Sequence 1 3.3 nC02 trapping efficiencies 43.4 Comparison of overall trapping efficiency 43 4.1 UC02 Reduction sequence 47 4.2 Summary of uCO yields, 17.5-70 cm3/min, 2 bar 47 5.1 Effect of flowrate on conversion of CO to methanol (50bar, 180°C) .... 74 5.2 Effect of temperature on conversion of CO to methanol at 55bar, 126 cm3/min(STP) 75.3 Kinetic parameters for Leonov's model 76 6.1 Mo surface moles rough estimate 96.2 Mo total moles 97 6.3 C02 concentration estimates 105 viii List of Figures 1.1 Conceptual visualization of a cyclotron 3 1.2 Interior view of the PET TR-19 cyclotron 4 1.3 Annihilation of a positron . . 5 1.4 Commercial PET scanner 6 1.5 18FDG-PET scan of a breast cancer patient 7 2.1 Separation of air, CO, CH4 and C02 using gas chromatography 17 2.2 Separation of H2, air, CH4 and C02 using gas chromatography 18 2.3 Decay corrected nCO yields as a function of temperature 28 2.4 CO formation rate from temperature programmed reaction of C02 with Mo2C 29 3.1 11C02 Trapping experimental flow diagram 37 3.2 11 C02 activity vs. time, for different trap temperatures 42 4.1 nC02 Reduction experimental flow diagram 45 4.2 Equilibrium compositions of Mo-MoO-Mo02-Mo03-H2-02-H20 from 300 to 1500 K 54.3 Equilibrium mole fraction of Mo02 for different H2:Mo03 ratios from 300 to 1500K 1 4.4 Equilibrium of composition of Mo-Mo02-Mo2C-C02-CO 52 4.5 Equilibrium molar fraction of C02 from eqs. 4.5 53 4.6 Equilibrium molar fraction of CO from eqs. 4.6ix 4.7 Conversion of C02 to CO vs. temperature for different C02 concentration, based on Aspen equilibrium data 54 4.8 Experimental flow-diagram for the reduction of C02 57 4.9 Effect of temperature on reaction of C02 and Mo, at 4 cm3/min and 2 bar . 60 4.10 Effect of flowrate on reaction of C02 and Mo at 825°C and 2 bar 61 4.11 Total carbon oxides as a function of temperature 62 4.12 Total carbon oxides as a function of flowrate5.1 Experimental flow diagram for methanol synthesis 68 5.2 Aspen generated equilibrium conversion of 50 ppm CO to methanol, in hydrogen 69 5.3 Methanol produced for continuous feed of H2/CO 72 5.4 Semi-batch methanol produced, 180°C, 50 bar for different flowrates ... 73 5.5 Semi-batch methanol produced, 120 cm3/min, 50 bar for different temper atures 75 5.6 Conversion of carbon monoxide to methanol vs. temperature 77 5.7 Conversion of carbon monoxide to methanol vs. flowrate 78 6.1 Mass flow control valve calibration curve 92 6.2 Correlated ball flowmeter calibration curve6.3 Gas chromatogram of CO containing sample 94 6.4 C02, CO and CH3OH calibration curves 5 6.5 Reactor temperature profile, at 740°C 99 6.6 Equilibrium relationships at atmospheric pressure Mo-C-Mo2C-H2-CH4 . . 101 6.7 Aspen generated equilibrium relationships at atmospheric pressure Mo-C-Mo2C-H2-CH4 102 x Nomenclature a Alpha particle: 2 protons and 2 neutrons <p Diameter £T' Trapping Efficiency, ratio of the amount of C-l 1 trapped to the amount of C-ll entering the trap £T Recovery Efficiency, ratio of the amount of C-ll released from the trap to the amount of C-l 1 released from the target A Mass number: number of protons + number of neutrons i.d. Inner Diameter I Length iV Activity remaining after initial activity NO has decay for time t ATj Initial amount of activity o.d. Outer Diameter Pe Particle emitted Pi Incident Particle p Proton xi t Synthesis time, minutes tl/2 Half life: 20.4 minutes for nC tT Trap time: time elapsed betwen begin of target unloading until C-ll is recovered from the trap TPR Temperature Programmed Reduction X Target Nucleus X' Residual Nucleus y Yield, defined as the amount of final product (mCi) divided by the amount of starting mateiral (mCi) y' Decay corrected yield, defined as the yield assuming no decay of product occured Z Atomic number: number of protons mCi MilliCuries, unit of radioactivity define to be the decay rate of 1.00 g radium, which corresponds to 37 billion disintegrations per secon CCH30H Concentration methanol, ppm CCO Concentration carbon monoxide, ppm CC02 Concentration carbon dioxide, ppm Ea Activation energy EOB End of Bombardment F Flowrate, gas flowrate defined in standard cubic centimeters per minute FID Flame Ionization Detector xii I Proton beam intensity, in microamperes IBS Ion Beam Stop id Inner Diameter k Reaction rate constant Keq Equilibrium constant ko Reaction rate pre-exponential factor LiAlH4 Lithium aluminum hydride n Number of experiments repeated at same conditions od Outter Diameter PET Positron Emission Tomography Pi Component i partial pressure R Ideal gas law constant r Methanol formation reaction rate STDEV Standard Deviation STP Standard Temperature and Pressure T Temperature TEC Thermo Electric Cooler THF Tetrahydrofuran TPR Temperature Programmed Reduction UHP Ultra High Purity xiii Vi Input Voltage, defined as the input voltage signal supplied to the mass flow con troller, in volts xiv Acknowledgments I would like to thank my supervisors at UBC, Dr's. Dusko Posarac, C.J. Lim and E. Kwok, as well as my mentors at Ebco Technologies Inc., Dr's. R. Johnson and K. Erdman, for their guidance and support. I also would like to thank my colleagues at Ebco Technolo gies and Advanced Cyclotron Systems Inc. and fellow students and machine shop from the Department of Chemical and Biological Engineering for their assistance with technical issues and their continued support. Finally, I would like to acknowledge the Science Coun cil of British Columbia, National Science and Engineering Research Council of Canada and Ebco Technologies for making this project possible. Finally, I would like to thank my family for their support. xv Chapter 1 Introduction 1.1 Background Short half-life radiopharmaceuticals are used in nuclear medicine together with positron emission tomography (PET) cameras to visualize organ function, particularly of the brain and the heart. PET clinics routinely use radiopharmaceuticals as a diagnostic tool for various disease conditions including cancer. Since the early 1970's, the number of ra diopharmaceuticals labeled with the positron-emitting radionuclide carbon-11, has rapidly increased. The most widely used carbon-11 labeling method involves methylation of an appropriate precursor, using [11C]methyl iodide as an intermediate [1]. For many medical applications it is essential that the radiopharmaceutical possesses a high specific activity [2], i.e. a high concentration of radioactivity per unit mass. The pro cess for production should permit sequential automated production runs, while minimizing operator exposure to radiation. Producing high specific activity [nC]methyl iodide with sufficient yield has been one of the major challenges in developing a process for the routine production of carbon-11 radiopharmaceuticals [3, 4]. 1 1.1.1 Positron emission tomography The in vivo study of biochemical processes, i.e. molecular imaging, became a reality in the second half of the 20th century [5, 6]. Discoveries made in nuclear physics in the 1930's gave rise to the conceptual idea of measuring biochemistry in vivo [7, 8]. Although ra dioisotopes could be produced, there were several technological barriers preventing the transfer of this technology to a clinical setting. Scintillation crystals were discovered around 1950 [9] and computers for data acquisition and processing were only available at a later date. The first positron camera was constructed in the 1960s [10]. Ten years later, groups in Europe, Japan and North America produced PET radiopharmaceuticals and developed PET scanners [10]. The major steps involved in PET imaging are production of the radioisotope with a par ticle accelerator, synthesis of the appropriate radiopharmaceutical and in vivo visualization of the biological uptake with 3-dimensional PET scanners. Particle accelerators The first step in PET is the production of the appropriate radionuclide by bombarding a target material with accelerated protons or deuterons. This can be accomplished using a linear accelerator or a cyclotron; most PET facilities use a cyclotron due to lower overall cost and physical size. In a linear accelerator, particles travel down a long, straight track and collide with the target. In a cyclotron, particles travel in a circular orbit until they reach the required energy and collide with a target. A conceptual visualization of a cyclotron is illustrated in Figure 1.1. It consists of a pair of hollow, semicircular metal electrodes (dee's), positioned between the poles of a large magnet. The dee's are separated from one another by a narrow gap and enclosed in a high vacuum chamber. An external source of ions (typically H~) supplies charged particles to the center of the cyclotron. As they enter the cyclotron, the radio-frequency (RF) accelerator alternates the 2 PRODUCTION TARGET Courtesy of Ebco Technologies Inc. [11] Figure 1.1: Conceptual visualization of a cyclotron electric field between the dee's within the cyclotron. The incoming ions are exposed to this electric field as well as a strong magnetic field generated by the main magnet, accelerating the negative ions in a circular path. As the number of orbits increases, so does their speed and energy. When the desired energy is reached, the electrons are stripped off the nega tively charged ions by a carbon extraction foil, and the resulting positive ion beam is thus extracted from its orbit. The resulting proton (or deuteron) beam collides with the target material to produce the desired radioisotope. Figure 1.2 illustrates a modern cyclotron, with the main vacuum chamber open. Radioisotope production A general form to describe a nuclear reaction between the target material and the acceler ated proton or deuteron is shown in eq. 1.1 [12], where X is the target material, P; is the incident particle, X' the generated radioisotope, and Pe the emitted particle. 3 RF Dees Courtesy of Ebco Technologies Inc. [11] Figure 1.2: Interior view of the PET TR-19 cyclotron £x+p; -> t:x' + pe (i.i) }4N + p -> I'C + a (1.2) The production of carbon-11 (eq. 1.2) involves the bombardment of nitrogen gas with an incident beam of protons, which creates a very unstable oxygen-15 intermediate [13] containing 8 protons and 7 neutrons. This intermediate instantaneously stabilizes by emit ting an alpha particle (2 protons, 2 neutrons), to yield the radionuclide carbon-11, which has 6 protons and 5 neutrons. Common radionuclides produced with a medical cyclotron are nC (ti/2 = 20.4 min), 13N (ti/2 = 10 min), 150 (t1/2 = 2 min) and 18F (t1/2 = 110 min). These radionuclides decay by pure positron emission, as illustrated by the decay of carbon-11 in eq. 1.3. The half life is a characteristic constant for a given radioisotopes and corresponds to the time 4 required for half of a radioactive sample to decay [14]. nC^l°B + P+ (1.3) In addition to their short half lives, the principal positron emitters nC, 13N, 150 and 18F are useful for clinical PET since their stable isotopes are the building blocks for most organic molecules (18F is used in place of H or OH). The radionuclides are chemically processed to prepare a radiopharmaceutical that will target the desired metabolic process or tissue in the body. PET Cameras Positrons ((3+) travel at most a few millimeters before they are annihilated with nearby electrons to give two gamma rays of 511 keV emitted in opposite directions (Figure 1.3). Before • + electron positron Best mass of each is 0 51 MeV Figure 1.3: Annihilation of a positron The PET camera uses rings of detectors that register the 511 keV rays from a single annihilation. The detectors are arranged in a circle around the patient, or in a hexagonal array where the detectors are grouped into cassettes. The content of each cassette varies 5 0.51 MeV Gamma photon 0.51 MeV Gamma photon according to the manufacturer, but usually these consist of 256 scintillating crystals being viewed by 16 photomultiplier tubes (four blocks composed of 64 crystals and four photo-multiplier tubes) with as many as three rings of 16 buckets in a circle (12,288 crystals with 768 photomultiplier tubes) [15]. An alternative design to the bucket, is one that uses rings of detectors with 11 crystals in a staggered array being exposed to 6 photomultiplier tubes [15]. As can be seen in Figure 1.4, once the patient is placed inside the scanner, he/she slowly moves through the rings of detectors to provide a whole or partial body scan. Figure 1.4: Commercial PET scanner When two detectors at opposite sides of the camera simultaneously detect a gamma ray, the data processor assumes that on the virtual line connecting the two detectors a positron was annihilated. Once sufficient data is collected, a 3-dimensional image of the radiation distribution can be generated. For example, Figure 1.5 shows the 18FDG uptake in a patient with breast cancer, revealing that numerous active metastatic cancer sites are present. 6 Courtesy Dr. F. Benard Figure 1.5: 18FDG-PET scan of a breast cancer patient 1.1.2 Application of PET PET is currently used clinically in cardiology, neurology, and oncology. The most common radiopharmaceutical used in PET is [18F]fluoro-deoxy-glucose (FDG) [16], which allows the measurement of glucose consumption in vivo and detects organs and tissues with high metabolic activity. Applications of PET in cardiology also include measurement of blood flow with 13NH3 and/or [nC]acetate, in addition to the studies on the glucose consumptions of the heart with 18FDG [17]. Applications in neuroscience include glucose metabolism with 18FDG, protein synthesis rate with [nC]tyrosine and blood flow with H2lsO [18]. In oncology, 18FDG-PET is a major tool for diagnostic and treatment follow-up. In addition to FDG, [J^methionine, [nC]thymine, [J^cytostatics are used for imaging of more specific cancers. Positron emitter labeling with carbon-11, nitrogen-13 and oxygen-15, can be used to investigate the catalytic processes and to quantify reaction phenomenon, yielding insight in 7 elementary reaction mechanisms useful as input to mathematical simulations [19]. 1.1.3 Carbon-11 radiopharmaceuticals Carbon-11 radiopharmaceuticals are finding an increasing number of applications in car diology, neurology, and oncology [18]. Many applications, such as brain imaging, require high specific activity radiopharmaceuticals. For example, [nC]raclopride, which is used to visualize dopamine receptors in the brain, requires a high specific activity since only a small number of dopamine receptors are available. Low specific activity, i.e. the presence of many [12C]raclopride molecules, may result in receptor saturation and poor image qual ity. Many [nC]radiopharmaceuticals are synthesized by the methylation of an appropriate precursor with [x^methyl iodide, which in turn is generally prepared from [UC]methanol. Production of carbon-11 radiopharmaceuticals Carbon-11 is produced in a cyclotron by the bombardment of a gas target filled with ni trogen, using a proton beam (typically 10-19 MeV), via the 14N(p,a)nC nuclear reaction. In the presence of 02, the carbon-11 is produced as nC02, while in the presence of H2, nCH4 is produced. A sequence of chemical reactions is carried out to convert these pre cursors to a carbon-11 radiopharmaceutical, typically via the [nC]CH3OH and [nC]CH3I intermediates. The conventional synthesis of [nC]methyl iodide most widely used over the past 30 years [20] involves two main reactions: the reduction of nC02 to nCH3OH, followed by iodination to yield nCH3I (eq. 1.4) [20]. LiAlHA HI nC02 -> nCH3OH _> nCH3I (1.4) In the liquid phase synthesis, nC02 is bubbled through a solution of lithium aluminum 8 hydride (LiAlH4) for the production of uCH3OH , which is then treated with HI to yield nCH3I. The LiAlH4 is a strong reducing agent and is readily contaminated with C02 from the atmosphere during preparation of the reagent. Consequently, relatively low specific activity [nC]methyl iodide is generally produced. The quantity of LiAlH4 utilized in the reaction has a great influence on the yield and specific activity of nCH3OH [13]. Large quantities of LiAlH4 in the reactor give rise to high yields with low specific activity. On the other hand, small amounts of LiAlH4 lead to low yields but with higher specific activity. Thus, the main drawback of this method is that a sufficient yield cannot be obtained while simultaneously achieving a high specific activity. Alternative methods, include the gas phase production of [nC] methyl iodide by react ing UCH4 with I2[21, 22]. This synthesis route avoids the use of LiAlH4 and consists of recirculating nCH4 with iodine vapor through a hot reactor. 1.2 Objective of the study The conventional method to produce many carbon-11 radiopharmaceuticals involves the LiAlH4 reduction of UC02 and is not suitable for production of high specific activity ra diopharmaceuticals. The main objective of this study was to determine the feasibility of an alternative gas phase process involving catalytic methanol synthesis, which providing a process for the production of large quantities of high specific activity carbon-11 radiophar maceuticals. The proposed gas phase reaction route consists of the reduction of C02 to CO followed by catalytic reduction of CO to CH3OH. The steps leading to methanol synthesis will be developed and optimized. Detailed objectives of the present study include: 1. To design / implement / optimize performance of C02 trapping device 2. To design / implement / optimize performance of reduction of C02to CO 9 3. To design / implement / optimize performance of reduction of CO to CH3OH 4. To develop an empirical rate equation for methanol synthesis to predict performance using carbon-11 10 Chapter 2 Literature review This chapter is divided in three sections. The first section deals with the radiochemistry of carbon-11. The second section provides in depth information of the reactions of carbon oxides and molybdenum compounds. The third section includes history and background information on industrial methanol synthesis. 2.1 Radiochemistry of carbon-11 Since the early 1970's, when medical cyclotrons where introduced, an increasing number of compounds are labeled with the positron emitting radionuclide carbon-11 [23]. The most widely used method to produce carbon-11 radiopharmaceuticals involves the methy-lation of an appropriate precursor with [nC]methyl iodide [2]. Based on this method, a large number of receptor-ligands have been investigated [24]. These radiopharmaceuticals require a high specific activity and it is thus important that each step in their production minimizes contamination with carrier carbon-12. The conventional method for the preparation of I1 methyl iodide is the reduction of [11C]carbon dioxide to [nC]methanol by lithium aluminum hydride, followed by conver sion to [nC]methyl iodide with hydroiodic acid [25]. An alternative method used by many PET centers involves a recently developed gas phase method, which consists of reacting 11 [nC]methane with iodine vapor to give [uC]methyl iodide [21, 22, 26]. Throughout this work the terms yield and decay corrected yield are frequently used. The yield is defined as the ratio of the amount of radioactive product to the amount of radioactive starting material, as shown in eq. 2.1. Although synthesis time does not show up directly in this equation, it is incorporated in the yield since a certain amount of C-11 is lost due to decay during the synthesis. However, in order to quantify the efficiency of the various steps in the process, it is desirable to calculate the decay corrected yield, also referred to as the radiochemical yield. It is calculated by multiplying the yield by a decay correction factor, which depends on the time elapsed and the half life of the radionuclide in question, as shown in eq.2.2. The decay corrected yield refers to the yield assuming no radioactive decay occurred, and is also referred to as the chemical yield. Amount Product (mCi) ^ ^ Amount of Reagent (mCi) y' = yexp0-693''/'^ (2.2) For example, consider a process which has a 30% yield (UC02 to 11CH3OH) with synthesis time of 20.4 minutes. Since the half life of carbon-11 is 20.4 minutes, the decay corrected yield is 60%. Thus the actual chemical conversion of [nC]carbon dioxide to [nC]methanol is 60%, but since half of the carbon-11 decayed, the actual yield is only 30%. 2.1.1 Production of C-ll Although several nuclear reactions can be used to produce carbon-11, the most convenient is the 14N(p,a)nC reaction using natural occurring nitrogen gas. Carbon-11 can be pro duced in the gas target as nC02 or nCH4; in the case of nC02 0.1-2% oxygen is added to the nitrogen, while for nCH4 production 5-10% hydrogen is added to the nitrogen gas. The natural abundance of C02 in the air is 330 ppm, whereas that of methane is 1.6 ppm. 12 This means that much precaution must be taken to exclude air from synthesis modules and reagents during synthesis with nC02. However, specific activities of nC02 and nCH4 produced in target are reported to be similar. For in target production of nCH4, a specific activity of 5 Ci/u-mol was reported [27, 28]. For in target production of nC02, specific activities up to 16.5 Ci/iamol were reported [29]. An independent study demonstrated that only a negligible amount of carrier 12C02 originates from the target [24]. [nC]Methane production yields are typically less than 65% of [nC]carbon dioxide yields [28]. These factors are among the reasons that many PET centers routinely produce 11C02 as opposed to nCH4. Target for C-ll production Pure aluminum, aluminum alloys and stainless steel are suitable materials for target con struction. Havar®, titanium or stainless steel are suitable materials for the target window foils. Metal gaskets are preferable to rubber O-rings [13]. In order to reduce potential car rier carbon and increase specific activity, ultra-pure materials with very low carbon content should be used. Thus, ultra pure aluminum would be suitable as target body and ultra pure titanium foil for the target window. For good recovery of C-l 1 from the target, it is recom mended that newly constructed targets be carefully washed with phosphoric acid followed by water, and dried under vacuum. The target gas should be of high purity and in particular as free as possible from carbon-containing impurities. An additional precaution against [L2C]carbon dioxide contamination would be to introduce a carbon dioxide trap in between the nitrogen gas cylinder and the target and also to use stainless steel tubing to minimize entry of carrier 12C02 by diffusion [13]. nCQ2 Produced(EOB) yUC°2 " I- (1-exp (-0.693-t/t1/2)) (23) 13 An important characteristic for a target is the nC02 yield at the end of bombardment (EOB). As can be seen in eq. 2.3, the nC02 yield depends on the amount of nC02 pro duced in the target, the half life of C-l 1, the beam intensity (I) and the duration of irradi ation (t). For an energy beam of 14 MeV, C-ll experimental target yields vary between 93 and 135 u-Ci/uA [30, 31, 32]. The theoretical target yield, calculated from 14N(p,n)nC excitation function, was determined to be 169 (a.Ci/(J.A at 14 MeV [31]. As can be seen from this data, the reported experimental yields are at least 25% less than the theoretical yield. 2.1.2 Recovery and purification of NC02 and nCH4 The target gas is either a mixture of N2/ H2 or of N2/ 02. The short half life of C-11 makes it necessary to concentrate it rapidly from a large volume of target gas in order to prepare the C-ll radiopharmaceutical [33]. In addition, the carbon-11 produced in the target as nC02 or nCH4 must be separated from the target gas, in order to remove the 02 or the H2, which can affect downstream processing of the C-ll radiopharmaceutical [34]. Two common methods exist for recovery of C-l 1, which are the use of a cryogenic trap and/or the use of an adsorbent trap (such as molecular sieve) [13]. The performance or overall trapping efficiency (£T) depends on the amount of C-l 1 released from the target, the amount of C-l 1 released from the trap and the time required for this process. The trapping efficiency (£T0 is defined as the ratio of the amount of C-l 1 trapped to the amount of C-l 1 entering the trap, as shown in eq. 2.4 and indicates how well the trap retains the nC02. The overall trapping efficiency is defined as the ratio of the amount of C-ll recovered from the trap to the amount of C-l 1 released from the target, as shown in eq. 2.5. The overall trapping efficiency can also be related to the trapping efficiency and the time required for trapping 14 and releasing the C-l 1, as shown in eq. 2.6. t f = C-ll trapped (mCi) 'T C-ll entering trap (mCi) C-ll released from trap (mCi) C-ll released from target (mCi) £T = exp-°-693'tT/tl/2 (2.6) Cryogenic nC02 trap: The trap typically consist of a small stainless steel tube, (40 cm x d> 0.02 mm). The tube is initially immersed in liquid nitrogen or liquid argon. The target gas is then flushed through the cold trap with an inert carrier gas such a helium, thus trapping the [uC]carbon dioxide. The [nC]carbon dioxide is recovered simply by passing a slow stream of inert carrier gas while heating the trap to room temperature. This requires removing the trap from the liquid nitrogen bath. Cryogenic nC02 traps typically have a trapping efficiency of 90% using a stainless steel tube immersed in liquid nitrogen or argon with overall trapping/releasing time of approximately 5 minutes [13]. This corresponds to an overall trapping efficiency of 76%. This method has been further improved, by the use of a stainless steel frit trap instead of a tube. The trap consist of a 2.25 cm long stainless steel check valve cartridge (for | tubing) which is packed with eight 20 urn stainless steel frits. The trapping efficiency was improved to 96% and overall trapping/releasing time was reduced to 3.9 minutes [35]. This corresponds to an overall trapping efficiency of 84%. Molecular sieve UC02 trap: The basic principle behind the molecular sieve trap is chromatography. Chromatography is a method of separation that relies on differences in partitioning behavior between a flowing 15 mobile phase and a stationary phase to separate the components in a mixture. Molecular sieves have been used as packing for chromatographic recovery of nCG*2 [13]. The trap typically consists of a column packed with zeolites molecular sieves. The target gas is un loaded through the trap, then flushed with inert gas, and heated to above 200°C for thermal desorption of the nC02. For a column of the following dimensions, I = 6cm, i.d. = 9mm, packed with activated 60-80 mesh molecular sieve 4A, the trapping efficiency is above 98% [13]. With an overall trapping/releasing time of approximately 5 min, the trap releases 90% of the carbon dioxide when heated to 230°C. This corresponds to an overall trapping effi ciency of 74%. The tenacious affinities of zeolites for both CO2 and water require careful activation be fore use and rather high thermal desorption temperatures. These inherent characteristics of zeolites lead to the development of an improved molecular sieve trap, with the use of carbon molecular sieves. In contrast to zeolites based materials, carbon sieves are quite hy drophobic in nature and have little affinity for water and small polar molecules. However, they avidly and selectively retain CO2 then release it freely upon the application of modest heat. This is clearly illustrated when comparing the chromatograms of a carbon molecular sieve column at room temperature and at 140°C, as shown in Figure 2.1. A similar trapping procedure has been used, with a 65 cm long trap, 2 mm i.d., packed with 1 g of 80-100 mesh carbon molecular sieve. Trapping efficiency was essentially 100%, and 98% of the nC02 was released from the trap heated to 100°C, with an overall trap/release time of 5 minutes [34]. This corresponds to an overall trapping efficiency of 83%. Control experi ments showed that most of the carbon sieves tested did not significantly contribute 12C02 carrier to the final product [34]. 16 0 2 4 15 Min. 0 2 4 Min. A) 1. 02, 2. N2, 3. CO, 4. CH4 B) 1. Air, 2. CO, 3. CH4, 4. C02 20°C, 45 cm3/min He 140°C, 45 cm3/min N2 Chromatogram, using carbon molecular sieve column, obtained from Alltech Inc. [36] Figure 2.1: Separation of air, CO, CH4 and C02 using gas chromatography Cryogenic/chromatographic nCH4 trap In order to increase the retention time of nCH4 in a chromatographic column and obtain separation from target gas, a combination of cryogenic trapping and chromatography are used. The trap consists of a tube packed with Poropak N (80-100 mesh). The trap is initially submerged in liquid nitrogen, after which the target is unloaded under controlled flow. As can be seen in Figure 2.2, heating to room temperature is sufficient to release the [nC]methane. Trapping methane on Poropak N at -196°C is less efficient than trapping car bon dioxide on molecular sieves [22], with overall trapping releasing time approximately 6.0 minutes. Assuming that the trapping efficiency is 90%, this would correspond to an overall trapping efficiency of 73%. 2.1.3 Reduction of nC02 and oxidation of nCH4 Reduction of UC02 to nCO [nC]Carbon monoxide was one of the first tracers used for blood flow measurement in hu mans [37]. Since it is less reactive than other [nC]labeling agents, it has found little appli-17 T = 35°C, 30 cm3/min He, 1. H2, 2. Air, 3. CH4, 4. C02 Chromatogram, using poropak Q column, obtained from Alltech Inc. [36] Figure 2.2: Separation of H2, air, CH4 and C02 using gas chromatography cation as an intermediate in radiopharmaceutical syntheses. However, recently palladium catalyzed cross-coupling reactions for the direct preparation of ketones have been reported [38, 39]. [nC]Carbon monoxide can be produced in situ or by reduction of [11C]carbon dioxide on the surface of various transition metal elements. An established method for [nC]carbon monoxide preparation is the reaction of [nC]carbon dioxide with zinc metal, as illustrated in eq. 2.7. Highest yields are obtained at 400°C which 4 is very near the melting point of zinc (420°C), thus rigorous temperature control is required to avoid melting the zinc. The zinc granules must be thoroughly cleaned before use and require frequent replenishment. Yields are under 50% since a significant amount of ra dioactivity remains in the reactor [37]. A more recent method for [11C]carbon monoxide preparation is the reaction of [11C]carbon dioxide with molybdenum metal (eq. 2.8). The reactor consisted of a 25 mm inner diameter quartz tube and 150 mm long, packed with 2000 m of 0.05 mm diameter molybdenum wire (99.97% Mo). A helium stream of 25 cm3/min (STP) was used to transfer the [nC]carbon dioxide through the molybdenum reactor, which was kept at a preset temperature. Decay corrected yields of up to 81% were reported with reactor temperature of 800° C [40], with 18 a gas transfer and reaction time of approximately 3 minutes, resulting in a yield of 73%. nC02 + Zn(s) - nCO + ZnO(s) (2.7) 400°C 211C02 + Mo(s) _> 2nCO + Mo02(s) (2.8) 800° C Reduction of nC02 to nCH4 The reduction of UC02 to nCH4 has been carried out for several applications, includ ing preparation of [nC]methyl iodide, [nC]methyl triflate and [nC]cyanide [2]. Although [uC]methane can be produced in target, many PET centers choose to first produce [nC]carbon dioxide and then react it with hydrogen using a nickel catalyst to produce [nC] methane, as illustrated in eq. 2.9. Ni nC02 + 4H2 _, nCH4 + 2H20 (2.9) 450° C In gas chromatography, flame ionization detectors (FID) are not very sensitive to trace amounts of carbon oxides, but are much more sensitive to methane. Accordingly, nickel based catalyst are frequently used to convert trace amounts of carbon oxides to methane in order to improve the FID sensitivity. In a unique setup, [uC]carbon dioxide is reduced to [nC]methane for production of [nC]methyl triflate. The reactor consists of a nickel/alumina/silica (64% Ni) powder mixed with glass wool packed into a 4 mm inner diameter borosilicate glass tube. The purified 19 [nC]carbon dioxide is swept from the trap with 10% hydrogen in nitrogen. The reactor oven is held at 450°C and the gas flowrate is approximately 50 cm3/min (STP). Yields of [nC]carbon dioxide to [nC]methane routinely exceed 95% [41] in approximately 2 minutes, corresponding to a decay corrected yield of over 99%. 2.1.4 Synthesis of nCH3OH The established method to prepare [nC]methanol involves the reduction of UC02 to nCH3OH using LiAlH4(aq). This method produces low specific activity nCH3OH due to contamina tion of LiAlH4 with 12C02. To improve the specific activities of nCH3OH, alternate liquid phase and gas phase methanol synthesis routes have been investigated. Liquid phase nCH3OH synthesis The conventional process for the reduction of [nC]carbon dioxide to [uC]methanol uses a solution of LiAlH4 in tetrahydrofuran (THF), as shown in eq. 2.10. The nC02 recov ery from the trap is done with a gas stream of helium or nitrogen at flow rate of 10-100 cm3/min (STP). The gas is dried over a dehydrating agent (MgC104 • H20 or P205) and then the gas is bubbled through a solution of LiAlH4 in THF The solvent is then evaporated under a stream of nitrogen at approximately 100°C, leaving behind a dry radioactive com plex from which [nC]methanol is generated by the addition of water. The [nC]methanol can be distilled for downstream use or alternatively hydroiodic acid can be added for in-vial preparation of [nC]methyl iodide. An increase in the amount of LiAlH4 leads to an increase in the yield, but a decrease in the specific activity. While a decrease in the amount of LiAlH4 leads to an increase in the specific activity but a decrease in the yield. The prepa ration of methanol typically takes 3-4 minutes with decay corrected yield in the order of 75%, and corresponding yield of approximately 66% [1]. Reported specific activities for [nC]methyl iodide produced via this procedure range from 0.1-1.7 Ci/u.mol [1, 13]. In attempts to reduce the amount of LiAlH4, a variation of the conventional method has 20 been developed, using LiAlH4 adsorbed on alumina. The alumina cartridge is pretreated at 200°C under helium flow, for 1 hour, to desorb water and possible traces of carbon dioxide and then cooled to room temperature. It is then impregnated with 50 ul of 1 M LiAlH4 diluted with 200 u.1 diethyl ether. The [uC]carbon dioxide is trapped on the cartridge, after which it is heated up to 160°C under a 50 cm3/min flow of helium to remove the solvent. The dry complex is then hydrolyzed by injecting 0.01 M phosphoric acid to form [11C]methanol. Decay corrected yields of 95% are reported with [nC]methanol preparation time of approximately 5 minutes, which corresponds to a yield of 80%. The specific activity of the downstream produced [nC]methyl iodide has been reported to be 2-2.5 Ci/u-mol [42, 13]. l)LiAlH4lTHF nC02 _> nCH3OH 2)H20 H20 nC02(g) CH30~(aq) —> CH3OH Gas phase nCH3OH synthesis Only a few publications report the catalytic conversion of [uC]carbon dioxide to [nC]methanol according to eq. 2.12. Cu/ZnO/Al203 nC02 + 3H2 _> nCH3OH + H20 (2.12) 150-250°C (2.10) (2.11) 21 J.T. Patt studied the synthesis of [nC]methanol from [nC]carbon oxides using Pd/Al2C>3 and Cu/Zn07Al203 catalysts [43]. Using either catalyst, and a mixture of uCO and/or nC02, Ar, H2 as feed gas, produced negligible amounts of methanol at 200-240° C and at 2-3 bar. The highest methanol yield obtained was 7%, with synthesis time of 25 min, at 240°C and at 2 bar, by adding N20 to the feed stream [43]. A patent describes a pre-conditioning method of a catalyst prior to use for [nC]methanol synthesis [44]. A copper-zinc oxide catalyst, supported on alumina and/or silica, is first re duced and then preconditioned with a stream of CO:C02:H2 (1:1:8). Prior to [11C]methanol synthesis, the catalyst is heated to 200°C and then gas containing [nC]carbon dioxide and hydrogen is passed through the reactor at a pressure of 50 bar. The [nC]methanol may remain adsorbed on the catalyst, and can be removed by addition of a catalyst poison, such as hydrogen sulphide or by increasing the temperature of the reactor to 280-320°C. The yield of [nC]methanol is 57% and the specific activity ranging from 4-20 Ci/umol [44]. An alternative method uses 11CH4 as starting material instead of 11C02 . A mixture of nCH4, Cl2 and H2 is passed over Cr203 on pumice stone at 700°C in order to oxidize the nCH4 to nCH3OH with yields up to 45% [45]. Synthesis time is 2 minutes decay corrected yield of 48%. The specific activity of the subsequently prepared nCH3I was 1 Ci/u-mol [45]. 2.1.5 Synthesis of carbon-11 radiopharmaceuticals Most procedures to synthesize carbon-11 radiopharmaceuticals involve the methylation of an appropriate precursor. The reactivity of nCH3OH is insufficient for most applications and accordingly the nCH30H needs to be converted to a more reactive intermediate, such as nCH3I. The preparation of [nC]methyl iodide is done by reacting [nC]methanol with a source of iodine, a step that does not affect the specific activity of the product. Traditionally, [nC]methyl iodide has been prepared by reaction of [nC]methanol with hydrogen iodide under reflux [13]. The yield is above 90% [45, 42]. A more recent vari-22 ation of this reaction route involves the use of aqueous HI impregnated on alumina, for which the yield was above 97% at optimal conditions [42]. Alternative iodination agents, diphosphorous tetra-iodide and triphenylphosphine diiodide, have been investigated for the production of [nC]methyl iodide[46, 47]. The yields are similar as for the HI procedure, however by avoiding the use of volatile HI, the solid reagents allow a cleaner operation. An alternative procedure, based on the iodination of [nC] methane with iodine, has been pioneered by Larsen et al. [22, 21]. The reaction is carried out in a reactor in which [nC]methane, helium and iodine vapors are mixed and heated. The formed [nC]methyl iodide is continuously removed from the reactor while the unreacted [nC]methane is re circulated through the reactor. The synthesis time is 10.5 minutes and reported yields are 58% with specific activity of 15 Ci/ixmol. 2.2 Molybdenum compounds for the reduction of CO2 to CO Molybdenum commonly occurs in nature as the mineral molybdenite, M0S2, in quartz rock. For this study molybdenum will be used to reduce carbon dioxide to carbon monoxide, by oxidizing the molybdenum. In this section, the history and chemistry of molybdenum, molybdenum oxides and molybdenum carbides are presented. 2.2.1 History Molybdenum was discovered in 1778, but for the next hundred years, molybdenite was merely a laboratory curiosity. The first major use came during World War I when it was dis covered that addition of molybdenum produced steels with excellent toughness and strength at high temperatures, suitable for use as tank armor and in aircraft engines [48]. Molybdenum is mainly used as an alloying element in steel, cast iron, and super-alloys to increase hardenability, strength, toughness, and corrosion resistance. However, 23 it has found many other applications in lighting, electronics, vacuum coating and nuclear medicine. It is also extensively used as a catalyst or as a component thereof [48]. 2.2.2 Reduction of molybdenum oxides Reduction of molybdenum oxides with hydrogen Molybdenum metal powder is produced industrially by reducing high-purity molybdenum compounds, such as molybdenum trioxide, ammonium hexamolybdate or ammonium di-molybdate, with hydrogen [48]. Molybdenum metal powder can be produced industrially by reducing M0O3 powder with hydrogen between 500-1150° C [49]. Molybdenum tri oxide, a gray-green powder is reduced by hydrogen at 500-600°C to M0O2, which is fur ther reduced at 900-1050°C to molybdenum metal. Since the first reduction to Mo02 is exothermic, this step is performed at 600°C to prevent caking due to the melting of M0O3 ( 800° C). The red-brown Mo02 [50] is reduced to metallic molybdenum powder at 1050°C. The powder has a particle size of 2-10 u.m, a specific surface area of 0.1-1 m2/g, and an oxygen content of 100-500 mg/kg (partly adsorbed and partly as oxide) [48]. Thermal decomposition and reduction of molybdenum trioxide under different reduc ing conditions has been extensively studied [51, 52, 53]. Molybdenum trioxide powder was reduced in pure hydrogen with gradual temperature increase from 300 to 800°C at approximately 6 °C/min and isothermally at 600°C. Under these conditions, the reduc tion of molybdenum trioxide to molybdenum dioxide took place at 387-615°C while the reduction to molybdenum metal took place slowly at 623-740°C[51]. Lee et al. [54] performed temperature programed reduction (TPR) of high purity molybdenum trioxide, from 300 to 750 °C, in pure hydrogen, with a heating rate of 1 °C/min. The gas products obtained during TPR were monitored by gas chromatography, equipped with thermal conductivity detector for the detection of water. Reduction of M0O3 to Mo02 occurred between 430-620°C, while complete reduction to molybdenum occurred above 700°C. 24 Iwasawa et al. [55] found that molybdenum dioxide on alumina was reduced with hydrogen to molybdenum at 600°C. In contrast to the one-step reduction mechanism of molybdenum trioxide to molybdenum dioxide, Burch [56] suggested that M04O11 is an in termediate product of the reaction. However, Ressler et al. [53] found that Mo4On was also formed by reaction of different molybdenum oxides. Temperature programmed reduction of M0O3 with 5-100% H2 was studied for temperatures ranging from 300-800°C. Between 350 and 425°C, the reduction of M0O3 to Mo02 is a one-step process without formation of crystalline intermediates. At temperatures above 450°C, Mo4On can be obtained and its formation was explained as the product of a parallel reaction between molybdenum diox ide and molybdenum trioxide. There is a general agreement between various researchers that at reduction temperatures above 500°C and hydrogen concentrations of at least 10%, metallic molybdenum is produced as the final product according to a two step reduction, as illustrated in eqs. 4.2 and 4.3 [53]. Reduction of molybdenum oxides with carbon monoxide Reduction of molybdenum trioxide with carbon monoxide at 400° C gave carbon dioxide, the reddish-brown molybdenum dioxide and unreacted molybdenum trioxide [57]. The reduction was presumed to proceed according to the eq. 2.13. At higher temperature (565°C), molybdenum trioxide in a stream of carbon monoxide gave carbon dioxide and a dark-gray almost black material, which was assumed to be molybdenum carbide and free carbon. The overall reaction is illustrated in eq. 2.15, which proceeds through intermediate eqs. 2.13 and 2.14. Further experiments were carried out with carbon dioxide (19%) and carbon monoxide (81 %) and molybdenum dioxide at roughly 800°C, which yielded grayish molybdenum carbide, presumably according to the reversible eq. 2.14. The addition of carbon dioxide was to prevent build-up of carbon on the surface, which was confirmed by 25 the color and the carbon content of the molybdenum carbide [57]. 400°C CO + MoO; '3 C02 + Mo02 (2.13) 565°C 6CO + 2Mo02 5C02 + Mo2C (2.14) 565°C 8CO + 2MoO; '3 7C02 + Mo2C (2.15) Hexagonal Mo2C is the only molybdenum-carbide phase of commercial interest and is the only phase that is stable below 1100°C [58]. It is produced as a powder in the micron range, with colors varying from white-gray to black [48, 59, 60]. It is stable in hydrogen, but it oxidizes in air above 500°C [48]. 2.2.3 Oxidation of molybdenum Oxidation of molybdenum with oxygen gas Molybdenum retains its luster almost indefinitely in air, particularly when it has been drawn to fine wire. On prolonged heating in air below 600°C, the metal becomes covered with its trioxide; at 600°C the oxide sublimes and rapid oxidation occurs. Molybdenum burns in oxygen at 500-600°C [48]. Oxidation of molybdenum with carbon dioxide Vandenberghe reported that carbon dioxide reacts with molybdenum to form carbon monox ide and molybdenum trioxide above 700°C [61]. Spencer et al. [57] later pointed out that 26 these authors made no analysis of the solid product, but assumed that the molybdenum was oxidized to molybdenum trioxide. The progression of the oxidation was monitored by observations of the appearance of the solid phase. The colors suggested that the oxidation was carried only to the dioxide, according to eq. 2.16 [57, 61]. 700° C Mo + 2C02 — M0O2 + 2CO (2.16) Hilpert et al. [62] indicated that at 1000°C, carbon monoxide passed over finely divided molybdenum leads to dimolybdenum carbide. At 800°C they obtained a carbide of high carbon content by reacting carbon monoxide with molybdenum trioxide. Smith et al. [63] previously observed no reaction when molybdenum was heated to a over 1000°C in an atmosphere of carbon monoxide. Lian et al. [64] demonstrated that at room temperature and at 80°C, H2, N2, CH4 and CO showed no reactivity with molybdenum atoms, while 02 and C02 both reacted with molybdenum. Thin molybdenum wire is reported to react with nC02 between 700 and 1000°C for the formation of nCO, and it was concluded to proceed according to eq. 2.8. Chemical conversions of up to to 80% were reported, over a narrow temperature range, 840-860°C, as illustrated in figure 2.3. At 825°C nC02 decay corrected yield was 35% and decreased with decreasing temperature, while at 875°C, nC02 decay corrected yield was 45% and decreased with increasing temperature. 2.2.4 Interaction of C02 and CO with Mo2C M02C is used in special cemented carbide grades containing TiC and nickel metal. Most Mo2C is used in steel alloys, where it forms during melting. Although M0O3 or M0O2 can be carburized with carbon at 1500°C, a carbide with the correct carbon content and a 27 90 -Temperature (*C) Radiochemical yield, i.e. decay corrected to EOB, from Zeilser et al. [40] Figure 2.3: Decay corrected nCO yields as a function of temperature low oxygen content is difficult to obtain. Pure Mo2C is best made by heating molybdenum metal powder with carbon in hydrogen at 1500°C [65]. Molybdenum carbide is also used extensively as a catalyst, such as for aromatization of ethane, ethylene, propane and in the oxidative dehydrogenation of these compounds using carbon dioxide as an oxidant. The catalyst is prepared by heating molybdenum trioxide in a stream of methane and hydrogen, from 500 to 800°C [54]. During preparation, surface contamination by carbon generally occurs. The latter can be removed by treatment with hydrogen under controlled environment. Once the excess carbon was completely removed, it was observed that the BET surface area of the catalyst and CO chemisorption were high est. For a catalyst treated with hydrogen, the surface area was found to be 60 m2/g, with a CO uptake at room temperature of 220 u.mol/g [54]. Lee et al. [54] showed that the molybdenum metal has a much lower surface area than the Mo2C catalyst. The Mo2C had a BET surface area of 60-100 m2/g while TPR of M0O3 with hydrogen yielded molybdenum with BET surface area of 3 m2/g. Prior 28 500 600. 700.. 800 900 1000 Temperature [KJ From Solymosi et al. [66] Figure 2.4: CO formation rate from temperature programmed reaction of C02 with Mo2C to removal from the reactor, the dimolybdenum carbide was passivated with 1% oxygen at room temperature [54]. Molybdenum can be passivated by oxidation, especially by electrolytic oxidation, becoming chemically unreactive [48]. Iwasawa et al. [55] observed deposition of small amounts of carbon on molybdenum fixed on alumina, after it had been reduced with hydrogen at 500°C for 5 h. Solymosi et al. [66] studied the reaction between carbon dioxide and supported Mo2C. Temperature programmed reaction of carbon dioxide with supported Mo2C forms carbon monoxide, as illustrated in figure 2.4. Carbon monoxide was first detected at 300°C, and a more extensive decomposition of carbon dioxide to carbon monoxide occurred above 600°C [66]. Using 13C02 as supply gas, it was demonstrated that over 90% of the CO was formed from the supply gas and not from the carbide [66]. It was demonstrated that the CO comes mainly from decomposition of C02, according to eq. 2.17, and that the contri bution of the reaction of carbon in Mo2C with the O atom formed in the C02 dissociation, according to eq. 2.18, is limited [66]. 29 C02 ^ C0(g) + 0(a) (2.17) C(8) + 0(a) ^ C0(g) (2.18) The reaction between 25% C02 and Mo2C was carried out for several hours at 800°C and complete oxidation to M0O3 did not occur [66]. 2.3 Methanol synthesis 2.3.1 History The history of industrial methanol synthesis covers over three quarters of a century, with the first barrel of synthetic methanol produced at BASF, Germany, in 1923. The first industrial methanol synthesis process is known as the high pressure process, which operated at 250-300 bar and 320-450°C, and was the dominant technology for 45 years. The feed syngas was based on coal/lignite, which generally contained a significant amount of poisons, such as chlorine and sulfur. Accordingly, a relatively poison-resistant catalyst was developed, based on zinc oxide / chromium oxide. However, further developments found that copper increased the selectivity to methanol, and that zinc was an efficient dispersant of copper [67]. The copper based catalyst is quite easily deactivated by poisons found in coal/lignite, though this problem was overcome by utilizing synthetic gas originating from natural gas and removal of catalyst poisons prior to methanol synthesis. Accordingly, a low pressure process was developed in the late 1960's, which operates at much milder conditions, i.e. 35-55 bar and 200-300°C. The low pressure process is still the dominant process being used today [68]. 30 2.3.2 Catalyst preparation Many different types of catalysts have been studied, including co-precipitated copper-zinc oxide, co-precipitated copper-zinc oxide alumina, Raney copper, intermetallic compounds and precious metals such as palladium [69]. The current catalysts used in industrial low pressure methanol synthesis are based on copper / zinc oxide / alumina with possible addi tives such as magnesium oxide [67]. The ratios of components vary from one manufacturer to another, but typically the copper oxide ranges between 25-80%, zinc oxide between 10-50% and the alumina between 5-10% [68]. Commercially available low pressure methanol catalysts have a methanol selectivity above 99% [68]. The low pressure catalysts are obtained as metal hydroxycarbonates or nitrates by co-precipitation of a multi-metal nitrate solution with a solution of sodium carbonate [70, 71]. Preparation parameters" such as pH, temperature, composition, duration, play an important role in the quality of the produced catalyst. A typical sequence for co-precipitation is the following: 1. Prepare solution of zinc, copper and aluminum nitrates to desired ratio 2. Co-precipitate metal ions using a solution of sodium carbonate 3. Filter metal carbonates and wash with water 4. Dry metal carbonates at 120°C 5. Calcinate the metal carbonates in air at 300-500° C 6. Pelletize metal oxides 7. Activate the resulting catalyst by reduction in 2% hydrogen at 250°C Prior to reduction, the commercial catalysts have a BET surface area of 60-100 m2/g, which is reduced to 20-30 m2/g after reduction [68]. 31 Activation of freshly prepared industrial catalyst is generally carried out by reduction in a 1-5% H2/N2 at 1 bar for several hours by ramping up the temperature to 240°C(~30 °C/h) and holding at this temperature for several hours. The reduction of CuO/ZnO and CuO/ZnO/Al203 catalysts, with 2% hydrogen in nitrogen at 250°C and 1 bar has been demonstrated to reduce the CuO to Cu metal, via the intermediate Cu20 [70]. At these conditions, the copper oxide is fully reduced to copper metal, without any residual copper oxide remaining [67]. 2.3.3 Catalyst poisoning / deactivation Halogen compounds are known to poison the copper surface, so methanol feed gas needs to be halogen free [69]. Other impurities in the catalyst itself, such as silicon compounds, nickel carbonyls or iron carbonyls, can cause damage to the catalyst [68]. The catalyst can also be deactivated when the reactor is operated in the absence of oxidizing agent such as carbon dioxide [70]. Experiments using a mixture consisting of only H2/CO rapidly and irreversibly deactivated the catalyst [71]. Methanol yields have been enhanced by the presence of carbon dioxide, water, and/or oxygen [72]. Experiments performed by pulsing oxygen to a CO/H2 feed indicated that up to a 15 fold increase of methanol yields could be obtained [72]. Active sites for methanol synthesis can be deactivated when the catalyst is operated for extended periods of time at elevated temperatures above 245°C [72, 69]. 2.3.4 Thermodynamics and kinetics Methanol synthesis, typically involves five components: hydrogen, carbon dioxide, carbon monoxide, water and the product methanol. The role of carbon dioxide in the reaction mechanism has been an ongoing debate [73]. Until the early 1980's, mechanistic considerations were based mainly on the reaction between carbon monoxide and hydrogen, illustrated in eq. 2.19 [68]. The higher yields achieved by the addition of carbon dioxide was attributed to the displacement of the re-32 verse water gas shift equilibrium 2.20. In addition, carbon dioxide was believed to affect the oxidation state of the active sites in the catalyst [70]. Alternatively, it was proposed that methanol was formed uniquely due to the reaction of hydrogen and carbon dioxide, illustrated in eq. 2.21 [74]. Recent experiments with isotope labelled reactants showed that both reactions 2.19 and 2.21 are possible [68]. CO + 2H2 ^ CH3OH (2.19) C02 + H2 ^ H20 + CO (2.20) C02 + 3H2 ^ CH3OH + H20 (2.21) Reaction enthalpies can be determined from the standard enthalpies of the reactants and products, and are -91 kJ/mol for eq. 2.19, -49 kJ/mol for eq. 2.21. Both reactions for methanol synthesis are exothermic and consequently methanol synthesis is favored by low temperature and high pressure. Additionally, the reaction of carbon dioxide with hydrogen, know as the reverse water-gas shift reaction, shown in eq. 2.20, must be taken into account. The enthalpy for the reverse water-gas shift reaction, is 41 kJ/mol. Consequently, this endothermic reaction is favored by high temperatures and low pressure. 33 Chapter 3 Experimental: Trapping and purification of nCC>2 The key intermediate in the radiosynthesis of many carbon-11 radiopharmaceuticals is [nC]methanol. This study focuses on the feasibility of a gas phase methanol synthesis, the optimization of the main steps involved and it's applicability to the radiosynthesis of [nC]methanol. The three principal steps evaluated in this study include: 1. Trapping and purification of [nC]carbon dioxide 2. Conversion of carbon dioxide to carbon monoxide using molybdenum 3. Methanol synthesis from carbon monoxide and hydrogen over a copper zinc oxide catalyst 3.1 Introduction The UC02 is produced in a cyclotron and subsequently concentrated in a carbon molecular sieve trap. The effect of temperature and mass of carbon molecular sieves on the trap performance was examined by computing the trapping efficiency, illustrated in eq. 2.4. The 34 overall trapping efficiency, illustrated in eq. 2.6, is based on the irradiation conditions for production of carbon-11 (proton current, proton energy, irradiation time) and on trapping data (amount nC02 not trapped, amount of nC02 released from trap and time required). 3.2 Materials and methods Irradiations were performed with the Ebco Technologies TRI 9 cyclotron of the CHUS PET facilities, Sherbrooke, QC. Capintec dose calibrators where used for quantitative measure ment of carbon-11. The target used is an Ebco Technologies gas target, consisting of a water-cooled aluminum cylindrical body, which contains the target gas. Two Havar win dows, which separate the high pressure gas target from the high vacuum cyclotron, are cooled with helium. A trap was designed such that it could be cooled to -20° C and rapidly heated to 110°C. The prototype trap was built at Ebco Technologies. Thermo-electric coolers (TEC's) were selected for their ability to be remotely controlled by computer and their relatively rapid cooling time. They have the advantage over conventional cryogenic traps that no liquid ni trogen is required and thus no moving parts are necessary. The TEC's require a DC voltage input, therefore the trap cooling can be remotely controlled by computer. This increases the level of automation in the final synthesis module and enables repeated productions with out having to access the unit. To provide fast heating, a 325 W cartridge heater were used, combined with the TEC's operated in reverse mode, which provided an additional 100 W heating power. The final trap design implemented consisted of a copper block, through which a U shape was machined and onto which two 35 mm long 6.35 mm outer diameter copper tubes were brazed. The U shape trap was then packed with carbon molecular sieve (Carbosphere 60-80 mesh) and both ends were plugged with quartz wool. Additionally, a 6.35 mm diameter hole was bored through the copper block, in which the 325 W cartridge heater was placed. 35 A K-type thermocouple was mounted on the copper trap to monitor temperature and allow temperature control. The copper block was screwed onto an aluminum heat sink block, with 2 thermo-electric coolers (TEC's) placed in between. A hole was drilled through the aluminum block and connected to a supply of cooling water, to remove the heat gener ated by the TEC's during the cooling step. After trap assembly, the carbospheres where conditioned by heating to 250°C and under flow of helium for 2 hours. Nitrogen/oxygen (UHP 99.5% N2, 0.5% 02) for the production of carbon-11 and helium (Helium UHP) were available on site at the CHUS facilities. The temperature was controlled by a manual thermostat, obtained from Omega. The flow rate of the helium sweep gas was controlled by a mass flow controller, obtained from MKS. The mass flow controller was calibrated using the soap bubble method, for which calibration curves are illustrated on page 91. Solenoid valves, 2-way normally closed, were obtained from Precision Dynamics. A check valve, with cracking pressure of 0.3 bar, was obtained from Swagelok. A control panel, to enable remote control of valves, reactor temperature and mass flow controller was built by Ebco Technologies. 3.3 Experimental set-up Figure 3.1 illustrates the experimental setup used to determine the trapping efficiencies. The [nC]carbon dioxide trap, the solenoid valve for helium gas supply, the mass flow control valve for helium flow control, the check valve and Ascarite column were located in a lead shielded hot cell. The cyclotron was located in a concrete shielded vault. The target was installed on the cyclotron target selector, which is locally shielded. 3.4 Experimental procedure The trapping efficiencies of a copper tubular trap, with 4 different amounts of carbon molec ular sieves, were measured with the experimental configuration illustrated in figure 3.1, for 36 99.5% N. 0.5% O 2 Alphas Protons 15.4 MeV *| Target He N2, a,,1 SV2 0) O SV3 MFC Dose Calibrator Fume Hood Figure 3.1: nC02 Trapping experimental flow diagram temperatures varying from -20° C to 100°C. The experimental procedure can be separated in to two distinct majors steps; production of nC02 and 11C02 trapping, purification and release. [nC]Carbon dioxide was produced by proton irradiation of the nitrogen/oxygen filled gas target. The gas target and all valves to control the filling/unloading were already in place at the CHUS PET facilities. Thus the target loading and unloading were done using the current setup implemented at CHUS for [nC]acetate production, with the unload line re-plumbed to connect it to the experimental setup located in the hot cell. The 22 cm3 (STP) target was filled to 17 bar. Once the cyclotron was in operation at a few U.A, the target was positioned so that at least 80% of the beam bombarded the tar get. The current was then increased to approximately 10 u-A, while monitoring the target pressure, ensuring that it did not exceed 25 bar. A saturated yield of C-ll is produced in roughly 40 min of bombardment. However, for these tests, only small amounts of ra dioactivity were desired, mainly to keep exposure to radiation below allowable levels set by Health Canada. Consequently 10 min of bombardment was sufficient. The cyclotron energy was not modified, and remained at the preset value of 15.4 MeV. Due to energy drop across the Havar foils, the beam energy that actually irradiates the target gas was about 3.4.1 Production of UC02 37 14 MeV. Several control runs were performed in order to determine the yield of the target. The target was irradiated as above, and its contents were directly emptied in an Ascarite trap lo cated in the Capintec dose calibrator. This allows measurement of total amount of [n]C02 produced in target as a function of irradiation conditions, namely beam intensity and irradi ation duration. Ten control runs were performed and the target yield was determined using eq. 2.3. For subsequent experiments, the amount of nC02 produced in target was com puted based on the target yield, proton beam intensity and an irradiation duration, using eq. 2.3. The steps involved in the production of nC02 are the following: 1. Turn on cyclotron (Ion source, main magnet, vacuum, utilities, target window cool ing, target cooling, RF) 2. Open the main valve on the nitrogen/oxygen gas cylinder 3. Set the pressure regulator to read 17 bar 4. Open the target valve 5. Close the target valve once pressure sensor read-back is roughly 17 bar 6. Set the N2/ 02 pressure regulator to 8 bar(for target rinse) 7. Remove ion beam stop (IBS) (now beam will be on target) 8. Adjust cyclotron main magnet 9. Adjust position of target 10. Increase proton beam to 10 u.A 11. Irradiate for 10 min 38 3.4.2 Trapping and release of NC02 Prior to production of the nC02, the trap water cooling valve was opened and the TEC's were turned on. A stable trap temperature of -20°C was reached in less than 10 min. The target gas was unloaded through the pre-cooled trap and rinsed with 8 bar N2/02 mixture. The trap was then rinsed with UHP He at flow-rates up to 70 cm3 (STP). The trap was closed and heated to 110°C. The nC02 was released with a stream of He and then trapped in a sodium hydroxide column. The sodium hydroxide column was placed in a dose calibrator, to allow continuous measurement of nC02. This enabled quantification of the amount of nC02 not trapped by the trap, and also the amount released from the trap. These quantities were decay corrected to end of the bombardment (EOB) (eq. 2.2), to enable determination of the overall trapping efficiency (eq. 2.5). In order to ensure that no activity remains on the trap, it was disassembled and placed in the dose calibrator. The steps involved in the nC02 trapping and releasing are the following: 1. Turn on cooling water and TEC 2. Open valve on helium gas cylinder and set regulator to 2 bar 3. Set mass flow-control valve to desired set point 4. Place a fresh sodium hydroxide column in dose calibrator 5. Open valve to unload target 6. Make sure target pressure is below 8 bar 7. Open valves on carbon molecular sieve trap 8. Measure amount of nC02 breakthrough throughout unloading step 9. Close valve to unload target 10. Open valve to fill target with N2/02 to rinse target and close after 10 s 39 11. Open valve to unload target 12. When the target pressure is ~ atmospheric, close all valves 13. Open Helium supply valve to rinse trap for 30 s 14. Heat trap (until release temperature is reached) 15. Flush helium through cold trap 16. Note radioactivity reading every 15 s 3.5 Results and discussion The target yield was determined to be 83 ±4 mCi/u.A, for an extracted beam energy of 15.4 MeV and energy on target of approximately 14 MeV. As can be seen in table 3.1, this value is lower than other reported experimental and theoretical yields. The target was subsequently redesigned to give a yield of about 150 mCi/uA. Table 3.1: C-ll target yields, 14 MeV Target Yield (mCi/^A) Ebco improved target 150 Ebco target 83 ±4 Vandewalle et al.[32] 135 ±7 Casella etal. [30] 92 Theoretical yield[31] 169 The time required for each step of the trapping sequence was determined in a system atic fashion. The unload time was set to 30 s since at that time the pressure in the target had dropped to nearly atmospheric. The time required for the rinse target step was set to 15 s, corresponding to the time required to manually perform the sequence of valve actuation. The time for the second target unload was determined by monitoring the radioactivity col lected in an Ascarite column, with the nC02 trap bypassed. A maximum value was seen after 45 s. Additional runs were done with 2 target rinses, however no significant amount 40 Table 3.2: UC02 trapping/releasing Sequence Step Description Time elapsed (min:s) 1 Unload target (EOB) 0:00 2 Rinse target 0:30 3 Unload target 0:45 4 He Rinse trap 1:30 5 Heat trap 2:00 6 Release nC02 2:30 Table 3.3: nC02 trapping efficiencies Trap Carbosphere (g) Trapping efficiency (± STDEV) 1 1.0 25% ± 2% (n=4) 2 1.3 45% ± 2% (n=4) 3 1.9 92% ± l%(n=4) 4 2.8 99% ± l%'(n=4) of additional C-11 was recovered. The He rinse of the trap was set to 30 s, to allow suf ficient time to remove the target gas from the trap [34]. The time for heating the trap to 110°C was 30 s. Table 3.2 illustrates the final sequence used, with the time (from EOB) at which each step was executed. 3.5.1 Effect of carbon molecular sieve mass on nC02 trapping effi ciency The amount of carbon molecular sieves necessary for optimal trapping was determined by comparing the trapping efficiencies for different amounts of carbon molecular sieves. The pre-cooled trap temperature was typically -20° C and the amount of 60-100 mesh carbon molecular sieves, was varied from 1.2 g to 2.8 g . Table 3.3 illustrates the trapping efficiencies for four different amounts of carbon molecular sieve. As the amount of carbon molecular sieves increases, the trapping efficiency increases. However, with increasing amount of carbon molecular sieves, the time required for nC02 recovery will likely increase and the volume in which the nC02 is delivered to downstream process may be larger. Thus the amount of carbon molecular sieves used for subsequent 41 300 — T = 100 °C ^-T = 20°G -«-T.= -20 °C . ^ ' t ' —i . , . , . 1 , , 4 0:00 0:30 1:00 1:30 2:00 2:30 3:00 3:30 4:00 Elapsed time, from E'OB (min) Figure 3.2: 11 C02 activity vs. time, for different trap temperatures. experiments was set to 2.0 g, i.e. the lowest amount required to obtain above 95% trapping efficiencies. The optimal amount will vary with target volume, target pressure, length and size of tubing from the target to the trap and trapping temperature. 3.5.2 Effect of trap temperature on CO2 trapping efficiency The temperature required for optimal trapping was determined by comparing the trapping characteristics at different trapping temperatures. The trap temperature was kept constant for each run, and the sequence shown in table 3.2 was used, with steps 5 and 6 omitted. Thus, the He rinse step was continued until 10 minutes EOB. Figure 3.2 illustrates the effect of temperature on the retention of 11C02 in the trap. At 100°C, the trap did not retain any significant amount of nC02. At room temperature, there was a slight delay before the activity was seen in the ascarite column. At -20°C, the activity remains on the trap even after 10 minutes EOB. The initial amount of nC02 at EOB was approximately 250 mCi in each case. 42 Table 3.4: Comparison of overall trapping efficiency Trap Overall trapping efficiency Cryogenic [13, 35] 76-84% Molecular sieve 13x[l3] 74% Carbon molecular sieve[34] 83% Carbon molecular sieve (this work) 88% ±2% 3.5.3 Overall trapping efficiency For a trapping efficiency of 99% obtained using 2.8 g carbon molecular sieve at -20°C, the time required to deliver the nC02 was 3.5 minutes. This corresponds to an overall trapping efficiency of 88%, which is competitive with reported results (see table 3.4). This would be sufficient for incorporating into a system for routine production of carbon-11 radiopharmaceuticals. 43 Chapter 4 Experimental: Reduction of CO2 to CO 4.1 Introduction The following step in the overall process for 11CH3OH preparation is the reduction of nC02 to nCO. Yields up to 80% were reported at 850°C for the reduction of nC02 to nCO using molybdenum [1], as described in section 2.1.3. No special treatment to the molybdenum was done prior to reaction, and the reaction proceeds by direct oxidation of molybdenum to molybdenum dioxide as shown in eq. 2.8 [75]. 4.2 Preliminary experiments: reaction of nC02 and Mo Preliminary experiments for the reduction of carbon dioxide were performed at the CHUS PET facilities, Sherbrooke, QC, using nC02. 4.2.1 Materials and methods The nC02 was produced and purified using procedure described in Chapter 3 on page 34. The carbon dioxide/carbon monoxide reactor consisted of a 9.5 mm outer diameter cylin drical quartz tube with 6 mm inner diameter, packed uniformly with 2.3 g of molybdenum 44 wire, 0.05 mm diameter and 500 m (Goodfellow Corp). The quartz tube was horizontally mounted in a 400 W ceramic tubular heater (Omega). The temperature was measured with a K-type thermocouple (Omega) and controlled with a manual thermostat (Omega). A mass flow controller, obtained from MKS, was used to control the flow rate of the helium sweep gas. It was calibrated by varying the input voltage from 0-5 V, and the output flow of helium was measured using the soap-bubble technique. The flowrates were corrected to STP using the ideal gas law. The resulting calibration curve is illustrated on page 92. Solenoid valves, 2-way normally closed, were obtained from Precision Dynamics. A control panel, to enable remote control operation of valves, reactor temperature and mass flow controller, was built by Ebco. 4.2.2 Experimental set-up The flow diagram for the experiments using nC02 is illustrated in figure 4.1. The same set-up was used as described in section 3.3 for production and release of nC02. The molybdenum reactor was added to the outlet of the nC02 trap, followed by an Ascarite (Aldrich) trap and a silica (Aldrich) trap, which was cooled with liquid nitrogen. At the outlet of the reactor, a solenoid valve was placed to avoid exposure to atmosphere. The setup was located in a lead shielded hot cell, with all valves / flowmeter controlled remotely. 99.5% N. 0.5% Q, SV1) Alpha as Protons 15.4 MeV Target N^.O^'.CO, He SV2 I cv1 j-X—t&H1 !SV3 MFC 11co2 Trap He. "C0„"C0, SV5 fx3—1——-2 ^ He SV4 He, N„0. Mo > Reactor 8 CD C/3 He.1,CO Dose Calibrator ; Fume Hood Figure 4.1: nC02 Reduction experimental flow diagram 45 4.2.3 Experimental procedure The production of nC02 was carried out as in the nC02 trapping experiments, described in section 3.4.1. The irradiation condition were noted to enable quantification of the total amount of nC02 produced in target. The nC02 trap was conditioned by flowing helium at 250°C for 2 h. Initial experiments were carried out with molybdenum as-supplied. Sub sequently, experiments where carried out after pre-reducing the molybdenum with 10 % hydrogen in helium at 850°C. The silica gel trap was initially conditioned by heating to 650°C while purging with helium. The molybdenum oven was preheated to 800, 850, 900 and 950°C, under flow of helium. The nC02 was released from the nC02 trap at 17.5, 35 and 70 cm3/min (STP) helium, through the molybdenum reactor, the Ascarite column and the silica column submerged in liquid nitrogen. The cold silica column was placed in the dose calibrator to measure the amount of uCO. When the activity on the silica col umn reached a maximum, the amount of nC02 on the Ascarite was likewise measured by placing the column in the dose calibrator. This enabled quantification of the amount of un-reacted nC02 that had been released from the reactor. To minimize exposure to radiation, long thongs were used to place the Ascarite trap in the dose calibrator. The decay corrected conversion of nC02 to 11 CO was computed based on the amount of activity produced in target and the amount of nCO measured. Table 4.1 illustrates the sequence that was used, with the time from EOB at which each step was executed. 4.2.4 Results and discussion Initial experiments resulted in nC02 conversion to uCO of about 5%. At the end of the experiments, it was observed that the molybdenum surface was no longer a shiny metallic color but a dull grayish color. Since the industrial compound Mo03 is described as a gray-green powder [48], it was suspected that the molybdenum was oxidized. Molybdenum metal powder is produced industrially by reducing compounds such as M0O3 powder with 46 Table 4.1: UC02 Reduction sequence Step Description Time elapsed (min:s) 1 Unload target (EOB) 0:00 2 Rinse target 0:30 3 Unload target 0:45 4 He rinse trap 1:30 5 Heat trap 2:00 6 Release UC02 2:30 7 11 CO measurement 6:30 8 11C02 measurement 7:30 Table 4.2: Summary of nCO yields, 17.5-70 cm3/min, 2 bar T(°C) Yield (decay corrected) S.D. 800 6% 2% 850 8% 2% 900 9% 4% 950 8% 2% hydrogen between 500-1150°C [49]. In order to reduce the molybdenum trioxide back to the metallic state, 10% hydrogen in argon was flowed through the reactor at 850°C, for 30 min. Thereafter, experiments were resumed. Decay corrected yields were calculated based on eq. 2.2. The amount of [nC]carbon dioxide produced in the target at the end of bombardment was computed using eq. 2.3, based on the target yield (see table 3.1), beam current and irradiation duration. A summary of the decay corrected yields obtained during hot experiments are given in table 4.2. For each temperature tested, at helium flow rates of 17.5, 35 and 70 cm3/min (STP), the average conversion of nC02 to nCO was at most 9%. Based on these results, there is no apparent correlation between flow and/or temperature with conversion. Conversion in the order of 80% was expected based on published data [40]. After completing the hot experiments, the molybdenum was again a dull grayish color indicating that oxidation may have occured. It is suspected that the helium flush of the nC02 trap was insufficient, and that some of the oxygen from the target gas remained in the nC02 trap. When attempting to reduce the UC02 with the molybdenum reactor, the 47 residual oxygen may have oxidized the molybdenum. Molybdenum retains its luster almost indefinitely in air, particularly when it has been drawn to fine wire. However, when heated in air, oxidation occurs and renders the surface chemically unreactive [48]. Consequently, for future use it is recommended to ensure that all oxygen is removed from the nC02 trap. This can be practically implemented by flowing additional helium through the nC02 trap at room temperature or during the heating step, prior to nC02 desorption. Another interesting observation is that on average, only 53% of the C-l 1 was accounted for during runs performed immediately after reduction of the molybdenum. Using a hand held Geiger counter, most of the unaccounted for carbon-11 was found to be on the molyb denum reactor. For subsequent runs (i.e. not immediately after reduction), an average of 96% of the expected carbon-11 was recovered from the reactor. It appears that freshly re duced molybdenum either reacts with carbon oxides or that carbon oxides remain adsorbed on the surface. Clearly the state of the molybdenum plays an important role in the reduction of carbon dioxide to carbon monoxide. To gain a better understanding of surface pretreatment and the effect of flow and temperature on C02 reduction by molybdenum, further experiments were carried out with cold 12C02 at UBC. In parallel to these experiments, a study of equilibrium using Aspen was carried out for various systems containing molybdenum, molybdenum oxides, molybdenum carbides, oxygen, hydrogen, carbon, carbon oxides and water. 4.3 Equilibrium computer simulations of systems contain ing molybdenum Equilibrium of molybdenum oxidation with oxygen and molybdenum trioxide reduction with hydrogen reduction were examined, as was the equilibrium of molybdenum oxidation with carbon dioxide using a process simulator. Two process simulators were available in the Department of Chemical & Biological Engineering; Aspen [76] and Hysys [77]. Aspen was 48 selected due to it's broad component database which includes solids such as molybdenum. In order to obtain equilibrium data, a Gibbs reactor was setup using Aspen. All relevant components available from the database were included for each simulation. Using the sensitivity study feature of Aspen, equilibrium data was generated for a wide range of temperatures. Further details about setting up the Aspen simulations are described in the appendix, on page 100. A good overall agreement between Aspen produced simulation data with published equilibrium data for the system containing Mo, CH4, C, H2 and Mo2C is demonstrated. 4.3.1 Reduction of M0O3 with H2 Aspen generated equilibrium data for the system containing H2, 02, H20, M0O3, Mo02, MoO and Mo is presented in figure 4.2, based on an initial H2: M0O3 ratio of 15:1, and at atmospheric pressure. Mo03 is reduced to Mo02 at room temperature. At 800 K, Mo02 begins to form Mo, until it is completely reduced at -1000 K. Based on simulation re sults, it appears that the reduction of Mo03 to Mo proceeds through two reactions, via the intermediate molybdenum dioxide, as shown in eqs. 4.2 and 4.3. In practice, a large excess of H2 will be present, since a continuous stream of hydrogen would flow over a fixed amount of molybdenum. Figure 4.3 illustrates the effect of increas ing the amount of Ff2 from stoichiometric feed amounts (for complete reduction according to eq. 4.1) up to an excess with H2: M0O3 molar ratio of 240:1. The effect of increas ing the excess of hydrogen is to shift the equilibrium to metallic molybdenum at a lower temperature. 3H2 + M0O3 — Mo + 3H20 H2 + M0O3 — Mo02 + H20 2H2 + Mo02 — Mo + 2H20 (4.1) (4.2) (4.3) 49 900 Temperature (K) -MO — -MOO -H2 1500 02 Initial ratio of H2: M0O3 of 15:1, at atmospheric pressure Figure 4.2: Equilibrium compositions of M0-M0O-M0O2-M0O3-H2-O2-H2O from 300 to 1500 K 4.3.2 Oxidation of Mo with 02 Equilibrium of oxygen and molybdenum Using the same component database and Gibbs reactor as for M0O3 reduction, equilibrium data for Mo oxidation was obtained. The data generated from Aspen indicates that Mo would be completely oxidized to M0O3, as illustrated in eq. 4.4, at temperatures above 273 K, for stoichiometric and larger amounts of 02. 302 + 2Mo -* 2Mo03 (4.4) Equilibrium of carbon dioxide and molybdenum Similar to above, simulations were carried out using Aspen to obtain equilibrium curves to better understand the effect of temperature on interaction between Mo and C02. To cover all possible reactions, the components added to the simulation were the following: He, Ar, 50 300 500 ?00 900 1,100 1,300 1.500. Temperature (K) H,: MoO, Ratio | 240:1 60:1. 15:1 7.5:1 -iiT] Figure 4.3: Equilibrium mole fraction of Mo02 for different H2:Mo03 ratios from 300 to 1500K CO, C02, C, Mo, MoO, Mo02, M0O3, MoC and Mo2C. The gas feed stream was set to contain 50 ppm C02 in argon, with an excess molybdenum, at atmospheric pressure. The resulting data is illustrated in figure 4.4. The compounds present at equilibrium are Mo, CO, C02, Mo2C, Mo02. Three distinct stages can be observed. Between 500 K and 800 K, equimolar amount of Mo02 and Mo2C are formed, most probably according to eq. 4.5, and no carbon is present in the form of carbon oxides. As the temperature increases above 800 K, the amount of Mo2C relative to Mo02 decreases, until no Mo2C is present at 910 K. At this point the amount of CO is the highest, corresponding to 73% conversion of C02. Above 910 K, it appears that the reaction proceeds according to eq. 4.6. C02 + 3Mo Mo2C + Mo02 (4.5) 2C02 + Mo _> 2CO + Mo02 (4.6) To verify these reactions independently, Aspen simulations were carried out for the 51 1.0 500 BOO 700 BOO 900 1000 1100 1200 1300 1400 1500 T(K) j C02 CO MO -MOQ2 - M02C | Figure 4.4: Equilibrium of composition of Mo-Mo02-Mo2C-C02-CO same components as above, but using an equilibrium reactor, for which the chemical re action can be specified. The feed gas stream was set to contain 50 ppm C02 in argon, with an excess molybdenum in the solid feed stream, both at atmospheric pressure. For an equilibrium reactor based on eq. 4.5 only, the resulting equilibrium curve is illustrated in figure 4.5. For temperatures below 800 K, no carbon dioxide is present, the only com pounds present are dimolybdenum carbide and molybdenum dioxide, which confirms that the lower temperature plateau in figure 4.4 proceeds according to eq. 4.5. For an equilib rium reactor based on eq. 4.6, the resulting equilibrium curve is illustrated in figure 4.6. At 500 K, carbon monoxide is present with a molar fraction just below 0.90. As temperature increases, the molar fraction of carbon monoxide gradually decreases to 0.66 at 1500 K. The high temperature plateau in figure 4.4 follows the same exponential decrease, which confirm that the high temperature stage proceeds according to eq. 4.6. Further simulations were carried out to explore the effect of varying the C02 concen tration on the equilibrium amounts of CO present, as represented in figure 4.7. The equi librium data is represented in terms of conversion of C02 to CO, which was calculated by 52 Figure 4.5: Equilibrium molar fraction of CO2 from eqs. 4.5 1.00 0.90 0.80 0.70 0 0 c 0:60 0 ati 0:50 LL U 0 40 O S 0.30 0.20 0.10 500 700 900 1100 1300 1500 Temperature (K) Figure 4.6: Equilibrium molar fraction of CO from eqs. 4.6 53 80% Q70% 5 60% §50% ^40% c30% o 0 20% j$ 10% 0% r / ™ j ,< / : I ; / i / ! ; I i / I 1 / J 500 700 900 1100 T(K) 1300 1500 1 ppm C02 1% C02 10% CQ2 50 ppm Figure 4.7: Conversion of C02 to CO vs. temperature for different C02 concentration, based on Aspen equilibrium data dividing the equilibrium amount of CO by the initial amount of C02. The shape of the curve follows a similar pattern for each C02 concentration. The three stages described above are present in all cases. The temperature at which C02 conversion reaches a maxi mum increases with increasing carbon dioxide concentration. For 1 ppm carbon dioxide, the maximum C02conversion to CO occurs at 850 K, while for 10% carbon dioxide the maximum conversion occurs at 1250 K. Cold experiments were performed with 50 ppm carbon dioxide. Accordingly, the ex perimental temperature range was selected to cover the three stages described above, i.e. from 600 to 1150 K. 4.4 Cold experiments: reaction of CO2 and Mo 4.4.1 Introduction CHUS "hot" testing facilities provide a relatively simple method to quantify conversion of trace amounts of nC02. However, due to limited availability of the CHUS facilities and the financial burden associated with their use, "cold" testing with non-radioactive C02 was 54 done to better understand the factors affecting the reduction of C02 with molybdenum. Temperature programed reduction of carbon dioxide with molybdenum and the effect of flow rate on the reduction of carbon dioxide with molybdenum were studied. 4.4.2 Materials and methods During typical productions of carbon-11 compounds, the concentration of C02 ranges from 1-2000 ppm in the feed gas, as demonstrated in the appendices on page 105. A 50 ppm C02 feed gas was selected, consisting of certified 51.4 ppm C02 in helium, which was contained in a 100 bar standard laboratory size gas cylinder. The gas flow rate was controlled by a mass flow controller (MKS instruments) for flow rates below 70 cm3/min (STP) and by an adjustable needle valve correlated flowmeter (Cole-Parmer) for higher flowrates. Calibration of both flow control devices was done using the soap-bubble method, and calibration curves are included in the appendices, on page 91. Manual 2-way valves (Swagelok) were placed at the inlet and at the outlet of the reactor. The reactor consisted of a 400 W ceramic tubular heater (Omega Heating) in which a glass tube was placed, which contained 2.3 g molybdenum wire previously described, covering a length of 10 cm. A K-type thermocouple was placed in the middle of the ceramic heater, and a second K-type thermocouple was place inside the reactor, on the molybdenum wire. Temperature was controlled with a manual operated thermostat (Omega). The temperature profile along the reactor was obtained by measuring the temperature at 2 cm intervals from the entrance of the reactor. Temperature profile of the reactor showed a variation of over 160°C over the molybdenum covered length of the reactor for a setpoint of 740°C, as illustrated in the appendices, on page 98. The addition of quartz wool plugs on either end of the ceramic heater improved the temperature profile along the reactor, reducing the temperature variation of the molybdenum covered length to less than 60°C. The product gas stream was connected to a 6-port sampling valve (VICI). The 6-port 55 valve was also connected to a waste stream, to a 2 cm 3(STP) sample loop, to a hydrogen supply and to the the inlet of the gas chromatograph. A Varian 3600 gas chromatograph was used, equipped with a a flame ionization detector (FID). The column used on the gas chromatograph was a 3 m long, 3.2 mm outer diameter column, packed with 60-80 mesh carbon molecular sieve. FID detectors are not very sensi tive to carbon monoxide, and are not useful for detection of carbon dioxide. A well known method of analyzing trace amounts of carbon oxides using FID is to first convert the oxides to methane using a nickel catalyst. Near quantitative conversion of carbon monoxide and carbon dioxide to methane can be accomplished by flowing the sample gas containing the carbon oxides over a nickel catalyst with excess hydrogen, at 370-450°C. Accordingly, a methanizer was built. A 15 cm long aluminum heater block was built at Ebco to accom modate a 6.3 mm diameter 175 W cartridge heater (Omega), a 3.2 mm diameter tube and a 1.6 mm diameter K-type thermocouple (Omega). A 3.2 mm diameter stainless steel tube was packed with 0.34 g of a mixture of 15% commercially available nickel on alumina powder (< 60 u.m) and 85% activated alumina, 100-120 mesh size. The excess nickel pow der was shaken off prior to packing the tube, after which quartz wool plugs were placed at both ends of the tube. The nickel packed tube was placed in the aluminum heating block. Swagelok fittings were placed on either end of the tube. The methanizer was placed in the gas chromatograph, in between the separation column and the flame ionization detector. The temperature was controlled with a manual thermostat (Omega). Calibration curves for carbon monoxide and carbon dioxide are given in the appendices, on page 93. 4.4.3 Experimental set-up The flow diagram for the experimental setup used for the reduction of C02 to CO is illus trated in figure 4.8. 56 He/C02/CO He/ CO 2 MFC SV1 Reactor Mo He/CO,/CO —{X SV2 GC MV1 NV1 Figure 4.8: Experimental flow-diagram for the reduction of C02 4.4.4 Experimental procedure Preliminary experiments, described in section 4.2, gave less than 10% conversion of [nC]carbon dioxide to [nC]carbon monoxide, most probably due to the presence of oxygen which ox idized the molybdenum to molybdenum trioxide. Aspen equilibrium data suggests that the temperature at which molybdenum oxides are reduced to molybdenum metal depends on the molar ratio of hydrogen to molybdenum. For a ratio of H2 :Mo of 240, complete reduction to molybdenum occurs at 400° C. For a ratio of Ff2:Mo of 7.5, complete reduction to molybdenum occurs at 900°C. In the reactor used, 2.3 g of molybdenum wire was placed in a length of 10 cm within the 6.3 mm inner diameter quartz reactor. Assuming only the exposed surface atoms are available for reaction, this corresponds to a molar ratio for H2:Mo of 130. At this molar ratio, Aspen generated data indicates that 425°C would be sufficient for reduction to molybdenum. There is a general agreement that the reduction of molybdenum trioxide with hydrogen to molybdenum metal is a two step process, forming molybdenum dioxide as intermediate, though the exact temperature at which reduction is reported varies. The reduction of molyb denum trioxide to molybdenum dioxide is reported to occur between 350-600°C while the reduction of molybdenum dioxide to molybdenum is reported to occur between 500-1150°C. Lee et al. [54] prepared molybdenum by TPR of 0.5 g Mo03 powder with pure hydrogen at 50 cm3/min, from 300°C to 700°C, increasing temperature 60 °C/h. 57 Carbon monoxide is more strongly adsorbed on freshly reduced molybdenum carbide than unreduced molybdenum carbide [54]. Iwasawa et al. [55] observed deposition of small amounts of carbon on molybdenum fixed on alumina, after it had been reduced with hydrogen at 500°C for 5 h. Although no data was provided for adsorption of carbon monoxide and carbon dioxide on freshly reduced molybdenum, there is a chance that ad sorption is higher on freshly reduced molybdenum as well. Lee et al. [54] suggested to passivate dimolybdenum carbide with 1 % oxygen at room temperature prior to removal of carbide from the reactor for surface analysis. Following Lee's [54] procedure, temperature programmed reduction was performed on the molybdenum wire, from 300 to 700°C with a temperature increase of 60°C/h, with an additional 12 hours of isothermal reduction at 700°C. UHP hydrogen, which contained 50 ppm of CO and 50 ppm CO2 was used as reduction media. Following cooling, the molybdenum wire was passivated with UHP compressed air, at room temperature, for one hour. Experiments were carried out using the experimental set-up illustrated in figure 4.8. The experiments were separated in two parts, temperature programed reaction and flowrate programed reaction. For the temperature programed reaction experiments, the gas stream was fed through the reactor at a fixed pressure of 2 bar and a fixed flowrate of 4 cm3/min (STP). The temperature of the molybdenum wire was varied from 331 and 883°C, in increments of approximately 60°C. At each temperature, 2 cm3 samples of the gas product were analyzed using GC for quantification of carbon dioxide and carbon monoxide. For the flowrate programmed experiments, the molybdenum wire was kept at a fixed temperature of 825°C and the feed gas was kept at constant pressure of 2 bar. The flowrate of the feed stream containing 50 ppm C02 in helium was varied from 5 to 1642 cm3/min (STP). At each flowrate, a 2 cm3 sample of the gas product was analyzed using GC for quantification of carbon dioxide and carbon monoxide. 58 4.4.5 Results and discussion During the reduction of molybdenum, water vapor was visible at the outlet of the reactor, indicating that molybdenum oxides were present initially. At the end of the isothermal re duction at 700°C, water vapor was no longer visible. There was some concern that molyb denum carbide may have been formed, due to the presence of 50 ppm carbon monoxide and carbon dioxide in the hydrogen gas. GC analysis of the product stream showed a sin gle peak, methane, indicating that carbon oxides reacted with hydrogen to form methane. Additional Aspen equilibrium simulations indicated that the only components in the prod uct stream at equilibrium at 700°C are molybdenum, methane, water and hydrogen. The molybdenum wire had a shiny metallic finish, characteristic of molybdenum metal. It was concluded that molybdenum oxides were present and that they were reduced to molybde num. The effect of temperature on the ratio of CO to total carbon oxides in the product stream from a feed stream containing 50 ppm C02 reacting with molybdenum from 331 and 883°C is illustrated in figure 4.9. Three distinct stages can be observed: 1. from 331 to 600°C, a plateau with average CO/(C02+CO) of 20%, 2. from 600 to 700°C, an abrupt increase from 20% to over 70% CO/(C02+CO) 3. from 700 to 883°C, a plateau with average CO/(C02+CO) of 71 %. A similar abrupt increase in carbon monoxide generation was observed by Zeisler et al. [40] at 825°C (see figure 2.3), for reaction of nC02 with molybdenum, and by Solymosi et al. [66] at 600°C (see figure 2.4), for reaction of carbon dioxide with molybdenum carbide. Aspen generated equilibrium data shows an abrupt increase in the conversion of C02 to CO, as illustrated in figure 4.7. The most notable difference between Aspen generated equilibrium data and experimental data is the fact that Aspen data suggests the absence of carbon oxides in the lower temperature plateau. However, experimental data from this study 59 80% -| 70% -60% -6 50% -o + o 40% -o o 30% -o 20% -10% 0% * X X x x X X X X K X. 500 600 700 800 900 1000 1100 1200 1300 T(K) Figure 4.9: Effect of temperature on reaction of C02 and Mo, at 4 cm3/min and 2 bar and others indicate that carbon monoxide is present at the lower temperature plateau. Aspen equilibrium data suggests that in the lower temperature plateau all the carbon dioxide reacts with molybdenum to form dimolybdenum carbide and molybdenum dioxide, as illustrated in figure 4.5. However, experimental results show that both carbon dioxide and carbon monoxide are present between 331 to 600°C. Overall, Aspen appears to be a good tool to determine the general profile for equilibrium conversions of carbon dioxide to carbon monoxide as a function of temperature for the conditions of this study, in particular for the second and third temperature stages described above. The effect of flowrate on the ratio of CO to total carbon oxides in the product stream from a feed stream containing 50 ppm CO 2 reacting with molybdenum at 825°C is illus trated in figure 4.10. Between 5 and 70 cm3/min (STP), there is no significant change in the ratio of carbon monoxide to total carbon oxides, averaging 76%. At 70 cm3/min (STP), the ratio of carbon monoxide to total carbon oxides decreases exponentially from 74% to less then 2% at approximately 1250 cm3/min (STP). The total amount of carbon oxides in the product stream exceeded the 51.4 ppm carbon 60 250 500 750 1,000 1,250 1,500 1,750 Flowrate (seem) Figure 4.10: Effect of flowrate on reaction of C02 and Mo at 825°C and 2 bar dioxide contained in the feed stream. For this reason, both figure 4.9 and 4.10 were plotted as a ratio of carbon monoxide to total carbon oxides. Figures 4.11 and 4.12 show the total amount of carbon oxides in the product stream, as a function of temperature and flowrate respectively. In figure 4.11, the data follows a similar trend as the curve in figure 4.9. There is an initial increase in total carbon oxides in the product stream from 50 ppm to around 120 ppm, from 340 to 400°C. Between 400 and 600°C, the amount of carbon oxides gradually decreases from 120 ppm to 90 ppm. Between 600 and 800°C, there is a much larger increase from 90 to 450 ppm carbon oxides. From 800 to 880°C, the amount remained constant at 450 ppm. In figure 4.12, the total amount of carbon oxides decreases exponentially from 75 ppm down to around 50 ppm. Considering that the flow experiment were done after the temper ature experiments, this decrease from 75 to 50 ppm appears to be the tail end of the larger peak seen in figure 4.11, beginning at 600°C. There are two possible explanations for the source of this additional carbon. The first possibility is that molybdenum carbide may have formed at the lower temperature during 61 100 90 80 10 250 500 750 1,000 1,250 1,500 1,750 Flowrate (seem) Figure 4.12: Total carbon oxides as a function of flowrate. 62 start-up of the apparatus and reacted with carbon dioxide and/of molybdenum dioxide to form carbon monoxide. The second possibility is that carbon dioxide and/or carbon monox ide remained adsorbed on the molybdenum surface prior to experiments and were released during experiments. Aspen generated equilibrium data suggests that Mo2C and Mo02 are formed by react ing molybdenum with carbon dioxide, from room temperature to 500° C. However, pub lished data on formation of molybdenum carbide from carbon monoxide with molybdenum dioxide, according to the reversible eq. 2.14 on page 26, proceeds at temperatures above 565°C [57]. The formation of molybdenum carbide by reaction of CH4 in hydrogen with molybdenum trioxide was reported to occur above 500°C. Thus, regardless of how molyb denum carbide is formed, it appears that the temperature must be over 500°C and that the carbon source must react with a molybdenum oxide. In Figure 4.11, there is always more than 51.4 ppm total carbon in the product stream, indicating that carbon dioxide probably did not react with molybdenum to form molybdenum carbide. Thus, the possibility that molybdenum carbide was the source of additional carbon seems highly improbable. Considering the second possibility, numerous studies have found CO and carbon ad sorption on molybdenum compounds is significant, in particular after reduction with hy drogen [54, 55]. During preparation of the molybdenum, after TPR reduction, some carbon dioxide and carbon monoxide may have remained adsorbed on the freshly reduced molyb denum while cooling to room temperature. During start-up of the experiments, helium containing 51.4 ppm carbon dioxide was flowing through the reactor. Since up to 120 ppm carbon dioxide was measured in the product stream, it is highly probable that some carbon dioxide was previously adsorbed on the molybdenum surface. The adsorption of carbon monoxide and carbon dioxide on the molybdenum surface during start-up and pretreatment seems to be the most likely source of additional carbon measured during experiments. The components molybdenum, molybdenum oxides, molybdenum carbides and carbon oxides constitute a complex system. The equilibrium data generated by Aspen provided 63 a good prediction of the achievable yield of carbon monoxide. For the high temperature plateau, the reduction of C02 to CO proceeds according to eq. 4.6, oxidizing molybdenum to molybdenum dioxide. 64 Chapter 5 Experimental: Methanol synthesis 5.1 Introduction In order to estimate the requirements for the production of [nC]methanol via a gas phase catalytic process, a series of experiments have been conducted with non-radioactive carbon monoxide. Although commercial methanol production involves a catalytic gas phase pro cess, no practical procedure is currently available for the production of [nC]methanol. The industrial production of methanol uses catalysts such as Cu/ZnO/Al203 that are prepared by co-precipitation and activated with 1-3% hydrogen at 250-290°C prior to use. The feed gas is normally syngas, which contains CO, C02, CH4 and H2, with the carbon dioxide acting as an oxidizing agent. This study aimed at determining the suitability of the catalytic gas phase procedure for the production of [nC]methanol. Activation and precondition of a copper zinc oxide catalyst were evaluated. The effect of pressure, temperature and flowrate of the feed gas on the methanol yield were studied and a kinetic model was generated. The model was used to establish optimal condition and estimate the potential yields of [11C]methanol production via a catalytic gas phase method. 65 5.2 Materials and methods In order to be consistent with conditions encountered during carbon-11 labelling proce dures, a 50 ppm CO feed gas was selected (see page 105). It consisted of certified 50 ppm CO in hydrogen, which was supplied in a 100 bar standard laboratory size gas cylinder. UHP helium gas, contained in a 100 bar standard laboratory cylinder, was used as inert sweep gas. The gas flow rate was controlled by a mass flow controller (MKS instruments) for flow rates below 70 cm3/min and by an adjustable needle valve correlated flowmeter (Cole-Parmer) for higher flowrates. Calibration of both flow control devices was done using the soap-bubble method, for which calibration curves are included in the appendices, on page 91. A manual 3-port valve (Swagelok) was placed at the inlet of the reactor, to select either helium or the feed gas. The reactor consisted of a 400 W ceramic tubular heater (Omega Heating) in which a 6.3 mm inner diameter stainless steel tube was placed, which contained the copper based catalyst, covering a length of 6 cm. A K-type thermocouple was placed in the middle of the ceramic heater, and a second K-type thermocouple was placed inside the reactor, in contact with the catalyst. The reactor temperature was controlled with a manual operated thermostat (Omega). Quartz tubes, 6.3 mm outer diameter with 1 mm inner diameter, where placed on both ends of the reactor to reduce the void space and the time required for the product gas to flow through the remaining portion of the reactor. Glass wool plugs were placed on both ends of the heater, to improve temperature uniformity. The resulting temperature profile of the reactor is included in the appendices. The outlet of the reactor was connected to a pressure regulator to maintain downstream pressure below the rating of the flow control devices. The product stream was also connected to a 6-port sampling valve (VICI). The 6-port valve was connected to a waste stream, a 2 cm 3 sample loop, a hydrogen supply and the inlet of a varian 3600 gas chromatograph, equipped with a flame ionization flame detector (FID). The GC was equipped with a 3 m long stainless 66 steel column (1.6 mm inner diameter) packed with 60-80 mesh poropak. Using a stream of helium saturated with methanol, a calibration curve was generated and is illustrated in the appendices, on page 93. 5.2.1 Cu/ZnO catalyst preparation Copper nitrate pentahemihydrate, Cu(N03)2 • 2.5H20, and sodium carbonate were obtained from Aldrich. Zinc nitrate hexahydrate, Zn(N03)2 • 6H20 was obtained from JT Baker. The procedure used for the preparation of the copper zinc oxide catalyst was based on the method described by Herman et al. [71]. A 1.0 M solution of copper nitrate was prepared by dissolving 21.6 g copper nitrate pentahemihydrate in 92.9 mL distilled water. Similarly, a 1.0 M zinc nitrate solution was prepared by dissolving 64.5 g in 216.7 ml distilled water. These nitrate solutions were mixed to obtain a 30:70 molar ratio of Cu:Zn. A 1.0 M solution of sodium carbonate was prepared by dissolving 50 g Na2C03 in 472 mL distilled water and was added dropwise to the 310 mL metal nitrates solution at 90° C, until the pH was raised from 2 to 7.0. The titration took 5 h and consumed approximately 360 mL sodium carbonate. Following a 12 h digestion at room temperature, the turquoise precipitate was filtered over glass frit and dried overnight at 85-105°C. The subsequent calcination of the copper/zinc carbonates was carried out in air by heating from 150 to 350°C in 2 h, with the maximum temperature maintained for 4 h. The resulting copper/zinc oxides were pelletized from an aqueous slurry, dried at ambient temperature and crushed and screened to a uniform size of 650 ± 200 |j.m. Samples of 2 g were placed in the reactor, covering a length of 6 cm. The catalyst was reduced under flow of 2% hydrogen in helium, for 12-16 h at 250°C and 1 bar. A standard BET method was used for the determination of surface area from argon adsorption at -196°C and the surface area of the reduced, used catalyst, was 30.3 m2/g. This is in the same range as measurements made by Herman et al., who reported a surface area of 37.1 m2/g for catalyst prepared by a similar method, and used under commercial methanol synthesis conditions [71]. 67 5.3 Experimental procedure The flow diagram for the experimental setup used for the methanol synthesis reactor is illustrated in figure 5.1. H2/ CO He MV1 -fc<r-MeOH Reactor H/CO/CHjOH ryCO/CH3OH -CXr Figure 5.1: Experimental flow diagram for methanol synthesis Commercial low pressure methanol synthesis is typically performed between 200-270°C and at 50 - 100 bar [78]. The practical pressure for [uC]methanol production is about 50 bar, due to pressure rating of commonly used valves, tubing and fittings in automated synthesis units. Aspen generated equilibrium data for the system containing 50 ppm CO, is illus trated in figure 5.2, as conversion of CO to methanol as a function of temperature and pressure. The conversion was calculated by dividing equilibrium amounts of methanol by initial amounts of carbon monoxide. Due to the exothermic nature of methanol synthe sis, as temperature increases, the equilibrium conversion of carbon monoxide to methanol decreases. For a given temperature, as the pressure increases, the equilibrium conversion of carbon monoxide to methanol increases. At 50 bar, equilibrium conversion of CO to methanol is 100% for temperatures below 180°C and decreases to 90% at 240°C. 5.3.1 Preliminary experiments: Cu/ZnO catalyst for CH3OH synthe sis Preliminary experiments were performed using a continuous feed containing 50 ppm CO in hydrogen at temperatures ranging from 180 to 240°C, flowrates ranging from 2 to 126 68 100 200 300 400 500 Temperature (°C) I— -2bar -10 bar- - -5.0 bar- 250bar| Figure 5.2: Aspen generated equilibrium conversion of 50 ppm CO to methanol, in hydro gen cm3/min(STP) and pressures ranging from atmospheric to 2, 10 and 55 bar. The catalyst was pretreated by reduction at 250°C with 2% H2 in helium for initial experiments. Subse quent experiments were performed using the same catalyst reduction conditions, however the catalyst was passivated by exposure to compressed air at 20°C. The feed gas, con taining 50 ppm CO in hydrogen, was continuously fed through the reactor and the product stream gas was sampled every 5-30 minutes and analyzed using the gas chromatograph for quantification of methanol produced. 5.3.2 Effect of flowrate and temperature on CH3OH synthesis In the final application, with carbon-11, the process will be performed semi-batchwise. Accordingly, further experiments were carried out semi-batchwise. Prior to experiments, the catalyst was reduced as described previously. Prior to each experiment, the catalyst was oxidized by exposing it to compressed air at ambient temperature. 69 Effect of flowrate on methanol production: The system was pressurized with helium at 55 bar, and flowmeter set to either 26, 93, 241, 468 and 935 cm3/min (STP). The reactor heater was turned on and set to 180°C, and samples of the product stream were analyzed using the gas chromatograph to ensure that no methanol was present. The feed gas was then switched to 50 ppm CO in hydrogen at 55 bar, for a period of 10-300 minutes giving between 0.3-0.9 cm3 (STP) carbon monoxide. Using the 6-port sampling valve, samples were analyzed using the gas chromatograph to quantify methanol concentration, typically at 2-5 minute intervals. After the predetermined CO feed time had elapsed, the tubing prior to reactor was vented and loaded with helium. When the reactor pressure reached 2 bar, the supply gas was switched to 2 bar helium and the flow rate was set to 126 cm3/min (STP). The product stream was sampled and analyzed using the gas chromatograph until methanol was no longer observed. Effect of temperature on methanol production: The system was pressurized with helium at 55 bar, and flowmeter set to 126 cm3/min (STP). The reactor heater was turned on and set to either 154, 178, 209, 224 or 240°C, and sam ples of the product stream were analyzed using the gas chromatograph to ensure that no methanol was present. Although commercial methanol synthesis is performed between 200-300°C, the experiments were limited to 240°C to avoid irreversible deactivation of the catalyst, which is reported to occur when catalyst is operated above 245°C and in the absence of an oxidizing agent [72, 71, 69]. The feed gas was then switched to 50 ppm CO in hydrogen at 55 bar, for a period of 20 minutes. The time was the same for all temperatures, and corresponds to 0.126 cm3 (STP) of carbon monoxide. Using the 6-port sampling valve, samples were analyzed using the gas chromatograph to quantify methanol concentration, typically at 2 minute intervals. After the predetermined CO feed time had elapsed, the tubing prior to reactor was vented and loaded with helium. When the reactor pressure reached 2 bar, the supply gas was switched to 2 bar helium and the flow rate was 70 set to 126 cm3/min (STP). The product stream was sampled and analyzed using the gas chromatograph until methanol was no longer observed. 5.4 Results and discussion: 5.4.1 Preliminary experiments: Cu/ZnO catalyst Preliminary experiments were performed using a continuous feed of 50 ppm CO in H2, at temperatures ranging from 180 to 240°C, flowrates ranging from 2 to 126 cm3/min(STP) and pressures of 2, 10 and 55 bar, using the reduced copper zinc oxide catalyst. No methanol was measured in the product stream under these conditions. The catalyst was then passivated with compressed air at 20°C, and the experiments were repeated. Exper iments performed at 55 bar resulted in measurable amounts of methanol in the product stream. However, experiments performed at 2 and 10 bar using the same experimental conditions failed to produce any detectable amount of methanol in the product stream. Using the passivated catalyst and operating pressure of 55 bar, further experiments were performed to measure the methanol produced as a function of time, for a continu ous feed of H2/CO. The amount of methanol in the product stream increases with time, then reaches a maximum, followed by a gradual decrease, as illustrated in figure 5.3. The methanol production appears to gradually stabilize, however there is no clear indication that a steady state is reached. For the experiment at 180°C, 55 bar and 2 cm3/min (STP), the concentration of methanol increases to a maximum of 45 ppm after about 150 minutes and then decrease to just under 18 ppm at 400 minutes. For the experiment at at 200°C, 55 bar and 26 cm3/min (STP), the concentration of methanol increases to a maximum of 12 ppm after about 75 minutes and then decreases to 7 ppm at 200 minutes. The initial peak in methanol production is likely due to the presence of adsorbed carbon 71 150 200 250 300 350 400j Time(min) 1180 °C; 55 bar, 2 cm3,'min(STP) x 200 °C, 55 bar, 26 cm3/min (STP)J Figure 5.3: Methanol produced for continuous feed of H2/CO monoxide on the catalyst. While the reactor was heated to the operating temperature, the feed gas was 50 ppm CO in H2. Thus carbon monoxide may have accumulated on the cold catalyst surface and reacted once the temperature was sufficiently high. Adsorbption of carbon monoxide on a copper zinc oxide catalyst at ambient temperatures has been previously described [72, 74]. Klier [72] reports that for a catalyst with 30/70 ratio of Cu/ZnO, 1.7 mol of CO / g catalyst reversibly chemisorbs to the catalyst surface. In summary, the preliminary results confirm that methanol can be produced from a feed stream containing 50 ppm CO in H2 using an activated and passivated Cu/ZnO cata lyst. These experiments also indicate that an operating pressure of 55 bar is adequate for methanol synthesis, while operating pressures below 10 bar are insufficient. The data sug gests that carbon monoxide accumulated on the catalyst at ambient temperature and only appeared in the product stream as methanol once the operating temperature was reached. The experimental procedure for subsequent experiments was adapted accordingly: the cat alyst was passivated prior to each experiment and the reactor was allowed to reach its operating temperature under helium flow before switching to the H2/CO feed gas. 72 20. O-5. c o 510 ra £ 5 2,500 5,000 7500 10,000 12,500 Cumulative Volume [cmJ, STP) l^e- 26 seem —— 93 seem -*- 241 seem -*- 468 seem -&- 935 seem | Figure 5.4: Semi-batch methanol produced, 180°C, 50 bar for different flowrates 5.4.2 Effect of flowrate and temperature on CH3OH synthesis For experiments performed under semi-continuous feed of H2/CO, the concentration of methanol in the product stream vs. cumulative product stream volume is illustrated in figures 5.4 and 5.5. Effect of flowrate on methanol production: Experiments were performed at 180°C, 55 bar and flowrates were varied between 26 and 925 cm3/min (STP). As the flowrate in creases from 26 to 935 cm3/m (STP), the conversion of carbon monoxide to methanol decreases from 26% to 0.5% (Table on the next page). As can be seen in figure 5.4, the methanol is released in two distinct peaks. The first methanol peak was released while H2/CO was fed to the reactor while the second peak was released during the he lium purge, at 180°C, 126 cm3/m (STP) and 2 bar. As the flowrate increases from 26 to 935 cm3/m (STP), the percentage of methanol released during the helium purge phase decreases from 48% to 26% (Table on the following page). The fact that the methanol produced is released in two distinct peaks, suggests that methanol synthesis has at least 2 rate limiting steps. One of the rate limiting steps is likely 73 Table 5.1: Effect of flowrate on conversion of CO to methanol (50bar, 180°C) Flowrate (STP) Methanol Yield % methanol released during purge 26 cm3/min 26% 48% 93 cm3/min 21% 35% 240 cm3/min 10% 38% 468 cm3/min 8% 29% 935 cm3/min 0.5% 26% Table 5.2: Effect of temperature on conversion of CO to methanol at 55bar, 126 cm3/min(STP) Temperature Methanol Yield 154°C 8% 178°C 14% 209°C 23% 224°C 25% 240°C 48% associated with the rate of formation of methanol. The second methanol peak occurs when the flow is switched to helium and the pressure is dropped from 55 bar to 2 bar, indicating that methanol is more readily released at atmospheric pressure than at 55 bar. Moreover, the fact that the percentage of methanol released during the purging was higher at low flowrate, suggests that methanol desorption is a second rate limiting step, which is in agreement with earlier studies of the kinetics of low-temperature methanol synthesis [79]. Effect of temperature on methanol production: Experiments were performed at 126 cm3/min (STP), 55 bar and the temperature of the reactor was varied between 154 and 240°C. As the temperature increases from 154 to 240°C, the conversion of carbon monox ide to methanol increases from 8% to 48% (5.2). As can be seen in figure 5.5, most of the methanol produced is released in one major peak which occured during the helium purge. Although at 240°C the methanol yield is the highest, a much larger volume of helium purge gas was required to release the methanol produced. At first glance, it appears that methanol is released from the catalyst as a single peak for operating temperatures between 154-220°C. This suggests that methanol synthesis has one 74 14 i 12 -. 10 - 1 2,000 4,000 6,000 8,000 10,000 12,000 14,000 16,000 Cumulative Volume (cm3, STP) |-o-154"C 178 "C -»-209°C -*- 224 °C -a- 24o"°c] Figure 5.5: Semi-batch methanol produced, 120 cm3/min, 50 bar for different tempera tures rate limiting step. However, upon closer examination, three of the profiles reveal a small satellite peak appearing just before the major methanol peak. The amount of H2/CO gas fed to the reactor in the temperature experiments was 2500 cm3 (STP), while up to twice as much was used in the flow experiments. In the latter experiments (figure (5.4)), the first methanol peak is released at about 2500 cm3 (STP), and the second peak is released during the helium purge at over 5000 cm3 (STP). During the temperature experiments, the major peak was observed while the reactor was purged with helium, at a cumulative volume of ap proximately 2000 cm3 (STP). Accordingly, the two peaks observed in the flow experiments would overlap in the temperature experiments. Thus, even though there are likely two or more rate limiting steps, only one peak appears in the temperature experiments. At 240°C, the methanol is released in a similar initial peak, but significant trailing suggests that an ad ditional rate limiting step occurs. This is consistent with studies reporting that intra-particle diffusion limits the rate of methanol synthesis at temperature above 245°C [79, 80]. 75 Table 5.3: Kinetic parameters for Leonov's model For 154-240 °C, 55 bar and 26-935 cm3/min(STP) Value units ko 1.3E-4 mol/(cm3sbar084) E„ 73 kJ/mol 5.4.3 Kinetic Model Leonov's proposed kinetic expression for methanol synthesis, illustrated in eq. 5.1, was used as a base kinetic expression to model the semi continuous CO/H2 feed experimental results for temperature and flow experiments, given in tables 5.1 and 5.2. The values of k and Ea, for which the error between model and experimental semi-continuous results was minimized, are represented in table 5.3. /p0.5 p p0.34 \ I P0.66 p0.5 . p .TS I V rCH3OH rCO rH2 ^eq/ k = ko-e*p(-p^) (5-2) Figure 5.6 illustrates the conversion of 50 ppm carbon monoxide in hydrogen to methanol, as a function of temperature, at 55 bar and 126 cm3/min (STP), for the semi-continuous experimental results, for the kinetic model generated using Hysys, and for equilibrium data generated using Hysys. As the temperature increases from 100 to 175°C, the equilibrium conversion of carbon monoxide to methanol remains at 100%, after which it decreases to 44% as the temperature increases further to 300°C. As the temperature increases from 154 to 240° C, the experimental conversion of carbon monoxide to methanol increases exponen tially from 8% to 48%. As the temperature increases from 100 to 270°C, the conversion of carbon monoxide computed from the kinetic model increases exponentially from 2% to a maximum of 55%. As the temperature increases beyond 270° C, the conversion of carbon monoxide computed from the kinetic model decreases following a similar trend as 76 240 260 280 300 Reactor temperature (°C) f X Experimental Data Equilibrium Data • Kinetic Model Kinetic Model (26 seem) | Flowrate 126 cm3/min (STP) and pressure 55 bar Figure 5.6: Conversion of carbon monoxide to methanol vs. temperature the equilibrium data, with an offset of approximately 6%, to reach a conversion of carbon monoxide to methanol of 38% at 300°C. The average difference between the experimen tal conversion of carbon monoxide to methanol and the value computed from the kinetic model is 3.6%. Figure 5.7 illustrates the conversion of 50 ppm carbon monoxide in hydrogen as a function of feed flowrate, at 180°C and 55 bar for the semi-continuous experimental data and for the kinetic model generated using Ffysys. As the flowrate increases from 26 to 935 cm3/min (STP), the experimental conversion of carbon monoxide to methanol decreases exponentially from 28% down to less than 1%. As the flowrate increases from 3 to 935 cm3/min (STP), the conversion of carbon monoxide computed from the kinetic model decreases exponentially from 100% to 4%, while for flowrates below 3 cm3/mm (STP) the conversion of carbon monoxide is 100%. The average difference between the experimental conversion of carbon monoxide to methanol and the value computed from the kinetic model is 3.3%. Applying these results to the use of carbon-11 for the synthesis of [nC]methanol re-77 200 400 600 800 Gas Flowrate (cm3/mln, STP) j X Experimental Data Kinetic Model I 1000 Figure Temperature 180°C and pressure 55 bar 5.7: Conversion of carbon monoxide to methanol vs. flowrate quires many considerations. Firstly, the short half life of carbon-11 limits the time allocated to methanol synthesis to less than 5 minutes. Secondly, the [11C]CO would be delivered in approximately 100 cm3 (STP) in hydrogen, which is an order of magnitude less than what was used in the semi-continuous experiments. As illustrated in figure 5.5, the cumulative volume required to release most of the methanol produced is less than 5000 cm3 (STP), which is twice as much as the feed gas volume. Assuming the same correlation applies for the release of [nC]methanol, this would translate to an elution volume of less than 400 cm3 (STP). Together with the 5 minutes time allocated for methanol synthesis, the mini mum flowrate would thus be 20 cm3/min (STP). The highest conversion of carbon monox ide to methanol computed from the kinetic model occurs at a temperature at approximately 270°C (figure 5.6). At temperatures above 245°C intra particle diffusion limitations have been observed [80, 79]. Moreover, as illustrated in figure 5.5, at high temperatures the amount of sweep gas required to elute the methanol produced is significantly higher than at temperatures below 224°C. This suggests that the optimal temperature for the carbon-11 application should be around 224°C. At 20cm3/min (STP), 224°C and 55 bar, the kinetic 78 model predicts a conversion of carbon monoxide to methanol of over 60%. 79 Chapter 6 Conclusion and Recommendations 6.1 Conclusions Carbon molecular sieves, in particular when cooled to -20°C, quantitatively trap and release carbon dioxide upon heating to 100°C. A trap has been developed which quantitatively retains and releases nC02 in less than 3.5 minutes. Though many existing traps are capable of quantitative trapping, the net advantage of this design lies in its compact size, rapid heating and cooling times, and use of TEC's as opposed to liquid nitrogen. This enables repeated use of the apparatus, without addition of liquid nitrogen. Automation of the system would allow delivery of a semi-continuous supply of nC02 for downstream processing, at less than 10 minute intervals. Carbon dioxide reacts with molybdenum to form molybdenum dioxide and carbon monoxide. Trace amounts of carbon oxides remain adsorbed on reduced molybdenum, and desorb at 800°C, in equilibrium ratios. Reduced, then passivated molybdenum is suitable for reduction of 50 ppm carbon dioxide in helium, to yield carbon monoxide at 800-880°C, 2 bar and flow rates under 70 cm3/min (STP). Conversions in the order of 70% are pos sible at these conditions. Aspen, a commercially available process simulator, was used to predict the equilibrium conversion of trace amounts of carbon dioxide to carbon monox-80 ide, by reaction with molybdenum. Conversions predicted with this process simulator were consistent with the experimental results. Trace amounts of carbon monoxide react with hydrogen to form methanol, on a copper zinc oxide catalyst. Reduced, then passivated copper zinc oxide is suitable to catalyze the reaction of 50 ppm carbon monoxide with hydrogen, to form methanol at 180-240°C, 55 bar and 2-935 cm3/min (STP). Based on experimental data, a kinetic model was created using a commercially available process simulator, Hysys. The kinetic model was used to predict optimal operating conditions for practical quantities of [nC]methanol, i.e. over 60% conversion of [uC]carbon monoxide, at 224°C, 55 bar and 20 cm3/min (STP). 6.2 Recommendations for future work The proposed nC02 trap can be incorporated into any process requiring UC02. However, experiments for uCO production suggested that the removal of oxygen from the trap was insufficient, using a 30 s helium flush at 200 cm3 (STP) while the trap was at -20°C. It is recommended to flush the trap with helium during the heating step or adding a step in which helium flows through the trap at room temperature to ensure that all the oxygen is removed. This will enable a supply of oxygen free nC02 to the downstream process, avoiding potential contamination with oxygen. When implementing this trap in a process, final adjustments should be done to the helium purge step to ensure that all the oxygen from the target gas is removed. The proposed molybdenum reactor to convert C02 to CO can be readily incorporated in a process requiring nCO. The experimental results suggest that carbon monoxide and/or carbon dioxide remain adsorbed on the molybdenum surface at ambient temperatures and desorb at about 800°C. Accordingly, care must be taken to remove any traces of 12C02 or 12CO from the molybdenum prior to use for nCO production, to ensure that this step does not reduce the overall specific activity of the final product. This may be accomplished by 81 flushing the reactor with UHP helium prior to use, with the reactor heated slightly above operating temperature. The reactor should also remain under inert gas while not used, preferably slightly under pressure, to avoid contamination with carbon-12. Experiments performed with 50 ppm C02 indicate that conversions of nC02 to 11 CO in the order of 70% are attainable. The proposed methanol reactor would be suitable to incorporate in a process requiring uCH3OH, such as the production of nCH3I with high specific activity. The experimen tal results suggest that carbon monoxide and/or carbon dioxide remained adsorbed on the copper-zinc oxide surface at ambient temperatures and desorb at about 200°C. Accord ingly, care must be taken to remove any traces of 12C02 or 12CO prior to catalyst use, to ensure that the final product specific activity remains high. This may be accomplished by flushing the reactor with UHP helium prior to use, with the reactor heated slightly above operating temperature. The reactor should also remain under inert gas while not used, preferably slightly under pressure, to avoid contamination with carbon-12. Based on ex perimental results obtained using 50 ppm nCO and the kinetic model, conversion of nCO to nCH3OH in the order of 60% are expected. Combining the nC02 trap, molybdenum reactor and the gas phase methanol reactor, the entire process has the potential to produce uCH3OH in clinically usable quantities. The advantage of the proposed gas phase synthesis over the conventional liquid phase method is the potential to obtain high specific activity carbon-11 radiopharmaceuticals. 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Intra-particle diffusion limitations in low pressure methanol synthesis. Chemical Engineering Sci-ence, 45, 4:773-783, 1990. [81] Thermochemical properties of inorganic substances. Springer-Verlag, Berlin, 1973. 90 Appendix I: Flowmeter calibration curves The commercially available MKS mass flow controller was calibrated. The mass control valve input voltage was varied from 0-5V, and the output flow of helium was measured using soap-bubble technique. The flowrates were normalized to STP using ideal gas law. The resulting calibration curve is illustrated in figure 6.1, for which a linear trendline was added. The equation relating input voltage signal to actual flow is shown in eq. 6.1, for which the R-squared value was 0.9996 indicating a good correlation. The 65 mm correlated ball flowmeter, obtained from Cole-Parmer, was calibrated in a similar fashion. The needle valve was adjusted so the reading was 10, 20, 30, 40, 50 and 60. At each point, the flow was measured using soap bubble technique, and adjusted to STP using ideal gas law. The resulting calibration curve is illustrated in figure 6.2, for which a linear trendline was added. The equation relating scale reading to actual flow is shown in eq. 6.2, for which the R-square value was 0.996 indicating a good correlation. FMFC(VJ) = 13.45V; (6.1) FcFc(Vi) = 28.89Vi (6.2) 91 80 0 1 2 3 4 5 6 Input Voltage (V) Figure 6.1: Mass flow control valve calibration curve Figure 6.2: Correlated ball flowmeter calibration curve 92 Appendix II: C02, CO, CH3OH calibration curves Samples of carbon monoxide, carbon dioxide or methanol were injected in Varian 3600 gas chromatograph equipped with a flame ionization detector and a custom built methanizer. The column used was a 3 m long, 3.2 mm outer diameter, stainless steel tube packed with 60-80 mesh carbon molecular sieve, obtained from Alltech. A typical chromatogram is illustrated in figure 6.3, for a sample containing 50 ppm carbon monoxide. The calibration curves for carbon dioxide, carbon monoxide and methanol are illus trated in figure 6.4. All three calibration curves show good linearity, with R-squared values over 0.98. Equations relating the peak area to the amount of carbon dioxide, carbon monox ide and methanol are shown in eqs. 6.3, 6.4 and 6.5, respectively. Preliminary calibrations, prior to installation of the methanizer, indicated good linearity between 10 and 500 ppm carbon monoxide. Calibration curves were generated by measuring gas chromatogram peak area of samples containing different amount of either carbon monoxide, carbon dioxide or methanol. The carbon monoxide and carbon dioxide samples were prepared by injecting different volumes of certified gas containing 50 ppm of carbon monoxide or carbon diox ide. Methanol samples were prepared by mixing different ratios of a gas stream saturated with methanol and UHP helium. Based on the temperature, the amount of methanol was calculated, assuming gas stream was saturated with methanol. 93 Molecular Sieve 13x column, FID Detector, 30 cm3/min (STP) He Figure 6.3: Gas chromatogram of CO containing sam CCo2 = 0.00138A + 4.22 Ceo = 0.00115A - 1.30 CcHsOH = 0.00166A - 23.6 94 140.0 20.0 0,0 •) 1 1 1 1 1 20,000 40,000 60,000' 80,000 100,000 Chromatogram Peak Area + Methanol x C02 • CO Figure 6.4: C02, CO and CH3OH calibration curves 95 Appendix III: Surface Molybdenum During Aspen simulations to obtain equilibrium data for the He, CO, C02, C, Mo, MoO, Mo02, M0O3, MoC and Mo2C system, an estimate for required amount of Mo. For equi librium reactors in Aspen, the reactants must all be specified in the feed stream. Thus, a rough estimate of the amount of Mo present was calculated. The lowest amount available, was calculated assuming that the molybdenum wire is non-porous and thus only molyb denum surface molecules are available for reaction. The highest amount available, was calculated assuming all the molybdenum wire is available for reaction. Table 6.1 illustrates the data used to determine the amount of Mo available for reaction. Based on the results illustrated in table 6.1 and 6.2, the number of hours the reactor could operate would range from 100 minutes to 4.5 years. The 100 minutes result was obtained assuming that the surface is not porous and that only surface atoms are available Table 6.1: Mo surface moles rough estimate Description value units Atomic Radius 0.140 nm Atomic cross section area 6.16E-20 mA2 Mo wire Surface Area 0.039 m2 Mo "surface" Atoms 6.4E17 atoms Mo "surface" moles 1.0E-6 moles Feed C02 50 ppm Feed Flowrate 4 seem Molar Flowrate C02 1E-8 mole/min Mo reaction time* 100 min *Assuming 100% Mo conversion to Mo02 96 Table 6.2: Mo total moles Description value units Molecular Weight 95.94 g/mole Weight Mo used in reactor 2.2385 g Mo total moles 0.023 moles Feed C02 50 ppm Feed Flowrate 4 seem Molar Flowrate C02 1E-8 mole/min Mo reaction time* 4.5 years * Assuming 100% Mo conversion to Mo02 for reaction. Typically reactions take place for less than five minutes per synthesis. Molyb denum being in excess of C02 in the reactant stream is thus a reasonable assumption. 97 Appendix IV: Temperature Profile The temperature profile was measured for the molybdenum reactor with open ends and for the reactor with quartz wool plugged ends, with a temperature setpoint of 740°C. The position of a K-type thermocouple was moved from one end to the other of the reactor, monitoring the temperature each 2 cm. As illustrated in figure 6.5, the addition of quartz wool plugs improves the temperature gradient. The molybdenum was place across a 10 cm length, from L = 2cm to L=12 cm. Over this length, the temperature varies from ap proximately 580°C to 740° C for the open ended reactor, and from approximately 680° C to 740°C for the plugged ends reactor. Thus the net effect of the quartz wool plugs was to reduce the temperature variance from 160°C to 60° C. 98 800 700 _^ 600 O 500 400 300 •< o Open Ends x Plugged Ends 0 2 4.6 8 10 12 14 L(cm) Figure 6.5: Reactor temperature profile, at 740°C 99 Appendix V: Process simulator Hysys is suitable for mainly gas/liquid phase reactions, with possible solid products. Car bon exists in the Hysys database while other solids can be custom created. Since Aspen has a built in database containing many solid compounds, including molybdenum, it was selected to carry out the equilibrium reactions. First, to validate the simulator, Aspen gen erated equilibrium data was compared to those reported in literature, for the reactions of methane with molybdenum and hydrogen with carbon. We can see in figures 6.7 and 6.6 that the equilibrium relationships generated using Aspen are quite similar to those reported [81]. The equilibrium curves for the formation of dimolybdenum carbide follow a similar pattern, however there is an offset on the tem perature scale of about 25 K. The equilibrium curves for the formation of dimolybdenum carbide follows a similar pattern, however there is an offset on the temperature scale of about 100 K. Although the temperature difference is significant, the shape of the curves are near identical. Thus Aspen was used to generate equilibrium curves. The following description represents the steps required to set-up an Aspen simulation to obtain equilib rium data for the Mo, MoO, Mo02, M0O3, C02, CO, 02, C system. Equilibrium curves generated for other component systems follow a similar procedure and differ only in the components used, temperature range and pressure range. 1. Setup Units: SI Stream Class: MIXCISLD, for use when conventional solids are present with no 100 (a) CH4 ^ C{s) + 2H2 (b) CHA + 2 • Mo ^ Mo2C + 2H2 Obtained from [81] Figure 6.6: Equilibrium relationships at atmospheric pressure Mo-C-Mo2C-H2-CH4 101 •100% 5* 200 400 600 800 1000 1200 1400 1600 T0<) | •• CH4 + 2Mo = Mo2C t 2H2 CH4 = C f 2H2 | (a) C#4 ^ C(8) + 2H2 (b) C#4 + 2 • Mo ^ Mo2C + 2H2 Figure 6.7: Aspen generated equilibrium relationships at atmospheric pressure Mo-C-M02C-H2-CH4 102 particle size distribution. 2. Possible Components: To begin with, here is a list of the compounds that can be present in the system, based on a feed of C02 through a reactor containing Mo. Solids need to be defined as type solid in Aspen, while gases are defined as type conventional Conventional: C02, CO, 02, Ar Solid: Mo, C, MoO, Mo2Os, Mo02, Mo205, M0O3, Mo2C, MoC Note: Components Mo203, M02O5 not part of database. 3. Properties Base Method: Peng-Robinson 4. Create Gibbs Reactor, with a feed stream and an equilibrium stream Set temperature: 273 K Set pressure: 2 bar 5. Define Feed stream Set composition of feed to desired mole fraction of each component Set temperature: 273 K Set pressure: 2 bar Set flowrate: 1 mole/sec 6. Model Analysis Tools Sensitivity Create new sensitivity analysis Define variables: all components in equilibrium stream in terms of mole fractions Temperature range 273-1573 K, 150 data points 103 The molar flow rate for each component was tabulated, copied to excel. From molar flowrate, molar fractions were easily calculated and plotted. 104 APPENDIX VI: Estimation of C02 concentrations The exact amount of CO2 contained in the target gas at Sherbrooke facilities is unknown. Sherbrooke facilities are not set-up to measure specific activity and by no means require high specific activity for their use of carbon-11. Thus, their system is not optimized and no special precautions were taken to obtain high specific activity from their target. The range of reported specific activities is 0.1-16.5 Ci/umol [45, 1, 21]. In practice, between 200-1000 mCi NC02 will be produced for each clinical run. During experiments at the CHUS, 250 mCi was produced each run. The content of C02 entering the molybdenum reactor can be estimated based on the flowrate of pushed used and the time required to eluted all the NC02. As can be seen in table 6.3, this corresponds to between 28-560 ppm C02. The time required to elute all the nC02 is estimated to be between 2-5 minutes, at flowrates between 25-200 cm3/min and a pressure of 2 bar. This corresponds to a broad range of C02 concentrations, roughly between 1 and 2,000 ppm C02, as can be seen in table 6.3. Gases containing 50 ppm of C02 or 50 ppm CO were selected to represent quantities used in routine carbon-11 radiopharmaceutical synthesis. Table 6.3: CQ2 concentration estimates SA (Ci/umol) nC02(mCi) umol C02 Q (c3m/min) P (bar) t (min) ppm C02 CHUS 0.1 250 2.5 25-200 2 2-5 28-560 Low SA 0.1 200-1000 2-10 25-200 2 2-5 22-2,200 High SA 16.5 200-1000 0.01-0.06 25-200 2 2-5 0.7-27 105 

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