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    • 专利摘要:
    The present invention relates to the synthesis and application of gold catalysts supported on mixed oxides cuo/zno/al2 o3 prepared from their corresponding solids with hydrotalcite structure as catalysts in the displacement reaction of water gas, for use in fuel processors coupled to fuel cells. (Machine-translation by Google Translate, not legally binding)
    公开号:ES2588034A1
    申请号:ES201400824
    申请日:2014-10-14
    公开日:2016-10-28
    发明作者:Jose Antonio Odriozola Gordon；Svetlana LYUBOMIROVA IVANOVA；José Luis SANTOS MUÑOZ；Miguel Ángel CENTENO GALLEGO；Tomás REINA RAMÍREZ；Tatyana TODOROVA TABAKOVA；Vasko DANAILOV IDAKIEV；Ivan IVANOV BOGOEV
    申请人:Consejo Superior de Investigaciones Cientificas CSIC；Universidad de Sevilla；
    IPC主号:
    专利说明:

    CO removal from these streams, catalytic processes have shown more
    efficient, such as the water gas shift reaction (Water Gas Shift, WGS, Equation 1) and the selective oxidation reaction of CO in the presence of H2 (Preferential CO Oxidation, PrOx, Equation 2).
    ca + H20 ~ CO2 + H2 ~ Ho = -41.2 KJ / mol (Ec.1) ca + ~ O2 + ~ CO2 (in H2 current) ~ Ho = -283 KJ / mol (Ec.2)
    One of the most studied aspects is the development of highly efficient and innovative catalysts for the reaction of water gas displacement (WGS). The WGS process constitutes the mandatory stage of cleaning (elimination) of CO from hydrogen currents, as amounts of up to 9-11% of CO can reach the WGS unit. Two aspects are relevant according to the characteristics of the reaction and the integrated nature of the hydrogen production and cleaning process. 1) With respect to the reaction itself, it is a reversible and exothermic process (llHo = -41.2 kJ / mol). Due precisely to the fact that we are facing a moderately exothermic process, the WGS reaction is thermodynamically disadvantaged at high temperatures. However, from the kinetic perspective, the catalytic process is more favorable at elevated temperatures. Therefore, in order to overcome this thermodynamic limitation, maintaining high reaction rates, the reaction usually takes place in multiple adiabatic stages, for example, high temperature shift (HTS) is normally the first stage with high operating temperatures (350 ° C-600 ° C), while low temperature shift (LTS) occurs as a second stage with a temperature range between 150 ° C and 300 ° C, interspersing an intermediate cooling stage to obtain a high overall conversion. 2) The second aspect to consider is that the WGS reactor is usually, by far, the largest in the integrated process since the water gas shift reaction is favored at low space velocities. To facilitate the implementation of this technology in mobile applications, the reduction of the reactor volume is of vital importance. In this sense, the development of catalysts capable of carrying out the
    WGS reaction at high space velocities constitutes one of the largestchallenges in the present scientific problem.Generally, four types of catalysts are distinguished for the WGS reaction:-Catalysts based on doped iron oxide, which operate at temperaturesslightly elevated (350-450 ° C) and are therefore used in the high WGStemperature (HTS).
    Copper-zinc mixed oxide catalysts, typically known as low temperature catalysts (LTS) because they are used at relatively low temperatures (19D-250 ° C). -The third type of catalysts uses cobalt and molybdenum sulfides as active phases and are resistant to sulfide poisoning. -Finally, the fourth type of catalysts is made up of those that operate at intermediate temperatures (MTS medium temperature shift) usually between HTS and LTS catalysts. They are usually copper-zinc catalysts like those used in LTS but modified (usually with iron oxide) to operate at slightly higher temperatures (275-350 ° C) than typical LTS catalysts. Since commercial catalysts for the reaction of WGS at low temperature (typically mixtures of CuO / ZnO) have a number of drawbacks such as their pyrophoricity, their need for prior activation treatment and in many cases their deactivation by sintering of the particles In metal, catalysts based on noble metals (mainly Au and Pt) are currently widely studied as an alternative to those mentioned above. In particular, catalysts that use gold as the active phase have been studied in detail and have obtained promising results during the last decade. Gold-based catalysts offer some advantages in the 180-250 ° C temperature range where the Pt group catalysts are not sufficiently active [D. Andreeva, 1. Ivanov, L. lieva, J.W. Sobczak, G. Avdeev, T. Tabakova, "Nanosized gold catalysts supported on ceria and ceria-alumina for WGS reaction: Influence of the preparation method"; Appl. Catal. A: Gen, Volume 333, 2007, Page 153-160.]. By
    For example, they are not pyrophoric and do not require any special pretreatment
    before using them. Recently [Robbie Burch, "Gold catalysts for pure hydrogen production in the water-gas shift reaction: Activity, structure and reaction mechanism"
    Phys. Chem. Chem. Phys., 2006, Volume 8, Page 5483-5500] have summarized the advantages and disadvantages of gold catalysts for the WGS reaction. It is well established that in the case of gold catalysts the method of preparation as well as pretreatment exert a great influence on the subsequent catalytic activity. The wide variety in the behavior of published gold catalysts is essentially attributed to the method of preparation of gold nanoparticles and the great diversity of supports used. However, there is general agreement on the importance of using an active support and more specifically Ce02 as a support for metal nanoparticles for the WGS reaction [Andreeva, D., Ivanov, l., Iieva, L., Sobezak, JW, Avdeev, G., Petrov, K. (2007) "Gold based catalysts on ceria and ceria-alumina for WGS reaction (WGS Gold catalysts"; Topics in Catalysis, Volume 44, (1-2), Page 173-182.] The main advantage of gold-based catalysts is that they allow operating at low reaction temperatures where the thermodynamic limitation is practically nil allowing high conversions of CO to be achieved. Patent documents can find the use of mixtures of CuO-ZnO as efficient systems. in the WGS reaction, for example, a system widely used in the industry is that developed by Larson in the 1960s (US1797426 Manufacture of hydrogen) More recently, patents filed by Farrauto and collaborators allude to the use of Pt supported in m Mixes CuO-Ce02Ab03 (US20020147103 Enhanced stability water gas shift reaction catalysts and US20020061277 Non-pyrophoric toilet gas shift reaction catalysts). In these catalysts the use of cerium oxide decreases pyrophoricity and increases stability. The latter is especially relevant for industrial applications. As proposed in the Shore patent (US6913739 Platinum group metal promoted copper oxidation catalysts and methods for carbon monoxide remediation)
    where the fact that the WGS catalyst is not pyrophoric is crucial is crucial
    before possible on and off events. The same inventors designed
    Pt-based catalysts for WGS with low methane production (US20030230029 Suppression of methanation activity of platinum group metal watergas shift catalysts). Catalysts with Fe203 / CuO / ZnO / Ab03 formulation have been applied with high efficiency in the reaction of WGS at intermediate temperatures, their preparation and use is set out in the patent (US7964114 B2 Iron-based water gas shift catalysts). The use of Fe-AI-Cu systems with different Fe / Cu ratios is also patented as very effective catalysts for hydrogen production via WGS (US 7947251 B2 Catalyst for hydrogen production from water gas shift reaction). The conventional CuO / ZnO / AI203 system can be improved by the addition of promoters. In the patent (US 6627572 Bl Water gas shift catalyst) it is explained how the doping of said system with elements chosen between K, Rb, Cs as alkalis and metals such as Ti, V, Mn, Mo, Zr, Ru, Pd, Re, La, Ce, Ba and Rh leads to the improvement of the catalyst in the WGS process. This strategy of doping the CuO / ZnO reference system with alkaline elements has been used since the 1990s as stated in the Klier et al. Patent (US 5021233 Water gas shift reaction alkalidoped catalysts).
    As for gold, a small percentage of patents describe the application of systems containing gold in (WGS) for the production of hydrogen. Such patents usually refer to the preparation of catalysts (for example Au on zirconium sulfate) for this application (US2007128100 Method for making hydrogen using a gold containing catalyst, [2007) or even show that gold catalysts may have more of a function, for example the application of gold-based catalysts for WGS in order to obtain hydrogen and simultaneously the use of the same catalyst in the oxidation of CO (US2008089823, Method For Making Hydrogen Using A Gold Containing Water-Gas Shift Catalyst, 2008 ). The deposition of gold in compounds with pyrochlorine structure (US2007269359
    Compound having a pyrochlore-structure and its use as a catalyst carrier in water gas shift reaction 2007), and in metal oxides (ceria and / or zirconia) in which at least
    40% of gold is present as Au3 + (W02005087656 Water gas shift catalyst, 2005) have also given rise to patents in this area. The Japanese National Institute of Industry and Advanced Technology has also filed three patents for the WGS reaction that involve gold in the composition of its catalysts. One with a catalyst based on gold and copper oxide (JP20020129816 20020501, Catalyst for water gas shift reaction, 2003), another with catalysts of arbitrary composition, where at least one metal oxide of the following elements Mg, Al, Mn is present , Fe, Co, Ni, Zn, Zr, or Ce (JP2004009011 Catalyst for water gas shift reaction). And in the third patent, a catalyst for WGS is proposed in a reforming gas stream composed of gold and metal oxides whose cations have a Pauling electronegativity in the range of 10-14 (JP2004066003, Catalystfor water gas shift reaction offuel reformed gas).
    The Korean Institute of Science and Technology also joins the list of entities with patents that allude to WGS in this case with catalysts based on Au, Ag, Cu, Ni, Zn, Cr and Al supported in a ceramic. Said ceramic can be ceria, zirconia, bismuth perovskite or bismuth oxides (KR20040036106, Catalyst of ceramic supported on metal for water gas shift reaction and method for preparing the same,
    2004). However, among the scientific articles or patents described there are no references to the use of a combined system based on the CuO / ZnO / AI20 3 system and a noble metal. Therefore, the possible combination of properties with added value of the two types of catalysts would be desirable as an interesting alternative with respect to the requirements necessary for the use of these in portable energy production devices. The present invention focuses on the synthesis and application of supported gold catalysts in mixed CuO / ZnO / AI 20 3 oxides with different CuO / ZnO ratios and prepared from their corresponding solids with hydrotalcite structure as highly efficient catalysts in the reaction of WGS
    Explanation of the invention In a first aspect an object of the present invention is a catalyst comprising gold supported on CuO / ZnO / AI203, which comprises between 10% and 80% of AI203 and between 90% and 20% of CuO / ZnO. In successive embodiments, the CuO / ZnO / AI203 support precursor has a hydrotalcite structure, the proportions between the compounds being: - Cu + Zn / AI ratio between 0.5 and 3 - CU / Zn ratio between 1 and 6. And the percentages by weight: -from 0.5 to 4% w / w Au -from 10 to 90% w / w CuO / ZnO In a second aspect, the method of the present invention is also an object of the present invention. preparation of said catalyst comprising the following steps: -synthesis of hydrotalcites as precursors of mixed oxides of CuO / ZnO / AI203. -deposition of gold on the substrate of CuO / ZnO / A1203. In a preferred embodiment, the synthesis of hydrotalcites takes place by coprecipitation at low supersaturation of Cu, Zn and Al salts at a pH between 7 and 10 and temperatures between 20 and 80 ° C. Preferably, the salts used as precursors are Cu (N03h.2H20, Zn (N03h.6H20 and AI (N03h.9H20 and 1M Na2C03 is used as a precipitating agent, the precipitation being maintained for a period of 48 h. drying at a temperature between room temperature and 100 ° C, followed by subsequent calcination at 300 ° C for 4 hours with a ramp of 10 ° C / min. In another preferred embodiment of the process of the invention, the deposition of Au is carried out by direct anion exchange assisted by NH3, starting from an aqueous solution of HAuCI4 to which the support is added.Another way of effecting the deposition of Au is by precipitation-deposit, in which the Au is deposited in the form of auric hydroxide in the oxide layers under stirring at constant pH.
    In a third aspect, it is also an object of the present invention to use the
    catalyst in the gas gas displacement reaction. In a preferred embodiment, the reaction takes place in reactive streams with a composition comprising: - between 4.5% and 9% of ca - between O and 11% of CO2 - between 30 and 50% of H20, performing the reaction at a temperature between 140 and 350 ° C and at a spatial speed between 4000 and 8000 h-1.
    Brief description of the figures Figure 1.-X-ray diffraction patterns A) X-ray diffraction patterns of uncalcined samples. B) X-ray diffraction patterns of the calcined sample. C) Comparison of diffraction patterns of a pre-reaction calcined sample
    and the same sample after use in WGS. D) Comparison of a calcined mixed oxide and its corresponding catalyst with
    gold. Figure 2.- Results of catalytic activity in WGS of the systems where M2 + / M3 + remained fixed at 1 and gold was deposited by the assisted anion exchange method. A) Comparison of the activity of mixed oxides with those of their corresponding
    Gold catalysts supported under ideal conditions (mixture of the described model) B) Comparison of the activity of mixed oxides with those of their corresponding gold catalysts supported under industrial conditions described.
    Figure 3.-Catalyst Au / HT_2 A) Continuous stability under real operating conditions B) Start / stop cycles under industrial mixing Detailed description of the invention The present invention relates to the synthesis and application of gold catalysts supported in mixed oxides CuO / ZnO / Ab03 prepared from their corresponding solids with hydrotalcite structure as catalysts in the WGS reaction. In the first place, the invention describes the synthesis of mixed oxides of zinc and alumina copper (CuO / ZnO / AI20 3) in an extremely controlled manner, by using a defined structure of the hydrotalcite type as a precursor to them. As a result, these solids have a stability against significant sintering that is reflected in a constant and lasting catalytic activity. The contribution of a minimum amount of gold results in a maximum increase (maximum allowed by thermodynamics in the temperature window 140-250 ° C) of the activity to which other advantages are added such as the omission of the catalyst preconditioning stage, decrease of its deactivation, increase of its durability and an important stability against changes of flow or temperature or cycles of on and off.
    Synthesis of hydrotalcites as a precursor of CuO / ZnO / AI203 The synthesis of hydrotalcites as precursors of mixed oxides CuO / ZnO / AI20 3 takes place by co-precipitation at low supersaturation, where salts and alkaline solution are added slowly, ensuring that the pH and temperature remain constant. The most used conditions are: between 10-80% in w / w of Ab03 and 90-20% in w / w of CuO / ZnO; pH between 7 and 10 (pH at which most hydroxides precipitate); temperatures between 20 and 80 QC; low concentrations and reagent flows; washing after filtration with hot water, to completely remove sodium ions; and drying at low temperatures (maximum 120 QC). First, an aqueous solution of 1 M concentration of Na2C03 is prepared as the precipitating agent. Subsequently, the required amount of each of the precursors used is deposited in a beaker of 1L volume. In
    In all cases, the precursors used were the nitrates of these metals, Cu
    (N03h2H20, Zn (N03h6H20, Al (N03h-9H20 because it does not generate solid waste andallows to obtain the cleanest hydrotalcite. These were dissolved in a0.8 L volume of distilled water and magnetically stirred throughout the entire phase ofprecipitation. The color resulting from the solution is a light blue color,characteristic of copper hydrotalcites. The precipitation of the hydroxides, ismaintained for a period of 48 hours. It is then allowed to dry, at atemperature below 100 ° C, being able to use a stove for it, orleave them at room temperature for a couple of days. Finally after the phase ofdried, the sample is calcined. Finally, the samples arecalcined with a temperature of 300 ° C, and a heating ramp of 10 ° C / minover a period of 4 hours.This process has two great advantages: on the one hand it allows the integration ofstructure a large group of anions and cations, and on the other hand, its preparation toLarge scale is of less complexity.
    Gold deposition methodTwo different gold impregnation methods have been used. In both methodsGold deposition has swept loads between 0.5 -4% (w / w) gold.1) Direct anion exchange method assisted by ammonia [S. Ivanova, C. Petit,
    V. Pitchon, "A new preparation method for the formation of gold nanoparticles on an oxide support" Applied Catalysis A-General Volume 267, 2004, pages 191201]. Said method consists in taking an aqueous solution of HAuCI4, with concentrations of 10-4 M which is heated to a temperature of approximately 70 ° C. Once this temperature is reached, the support is added to the solution and the mixture is left under stirring for 20 minutes. After this period of time, the solution is cooled to approximately 40 ° C and 20 mL of 30% NH3 (v / v) are added. Stir again for 20 minutes and then filter and collect the solid. Finally, it is dried and calcined at 300 ° C for 4 hours.
    2) Deposit precipitation method [D. Andreeva, T. Tabakova, V. Idakiev, P.
    Christov, R. Giovanoli, "Au / alpha-Fe203 catalyst for water-gas shift reactionprepared by deposition-precipitation "Applied Catalysis A-General Volume 169,1998, pages 9-14].The precipitation was carried out by means of an automatic system (Contalab),which allows the control of all precipitation parameters (pH, temperature,stirring speed, reagent feed flow, etc ...) Gold isdeposited in the form of auric hydroxide, Au (OHh, in the oxide layers, undervigorous stirring, keeping the pH constant at 7. After filtration and washingcareful, the precursors were dried under vacuum and calcined in air at 400 ° Cduring two hours.
    Embodiment of the invention As an example, the most representative results of a series of gold catalysts supported on mixed CuO / ZnO / Ab03 oxides, which are not intended to be representative of their scope, are described below. Chemical composition Elemental analysis was carried out by X-ray microfluorescence spectrometry (XRMFS) on an Eagle 111 EDAX spectrometer with a Rh radiation source. For the synthesis of a series of precursor hydrotalcites of the mixed oxides CuO / ZnO / Ab03., M2 + / M3 + ratios were swept from 1 to 6. In addition, for each of these relationships M2 + / M3 + the ratio M2 + / M2 + was varied between 1 and 6
    Table 1 shows the relationships of some of the representative M2 + / M3 + relationships. Table 1. M2 + / M3 + relationships for hydrotalcite synthesis
    Molar Ratio
    0.5 2
    (Cu + Zn) / AI
    Similarly for the M2 + / M3 + ratio in Table 2 some of the different Cu2 + / Zn2 + molar ratios, which were prepared, are exemplified.
    Table 2. M2 + / M2 + ratios for the synthesis of hydrotalcites
    Molar Ratio
    1.4 2.8 5.6
    CU / Zn
    With this, a representative sweep of relations is sought, in order to find or at least approximate as much as possible the ideal M (II) / M (II) relationship. Table 3 presents the composition of some of the prepared solids (HT) keeping the ratio M2 + / M3 + constant at one, where M3 + is A1 3+ and M2 + is a
    10 mixture of Cu2 + / Zn2 + whose ratio Cu2 + / Zn2 + varies from 1.4 to 5.6.
    Table 3. Chemical composition of some of the solids prepared, keeping M2 + / M3 + constant.
    Sample CuO (%)ZnO (%)AI20 3 (%)Rel. Cu / Zn TheoreticalRel. Cu / Zn Real
    HT1.4 35.8225.9738.211.41.38
    HT2.8 17.4047.7334.872.82.74
    HT5.6 51.9510.3437.715.65.02
    In all cases, a Cu / Zn ratio close to that intended in the synthesis was achieved. X-ray diffraction (DRX) analysis (XRD) was performed on an X'Pert Pro PANalytical device. Diffraction patterns were recorded.
    20 using the Cu radiation Ka (40 mA, 45 kV) in a range of 28 between 3 and BO ° and a sensitive position of the detector using a step size of 0.05 ° and a step time of 240 s. The DRX patterns of the synthesized solids are presented in Figure 1. Figure 1 shows the X-ray diffraction patterns of the uncalcined samples. In all cases the typical hydrotalcite signals are obtained and in addition a certain proportion of the malachite phase appears. Once the sample is calcined, Figure 1B, the mixed oxide CuO-ZnO-AI20 3 is obtained as shown by the diffractogram reflections. The diffraction patterns of a pre-reaction calcined sample and the same sample after use in WGS are compared in Figure 1C. It is clearly seen how copper oxide passes to metallic copper during the reaction. The latter is the active species in the water gas shift process. Finally, Figure 10 shows the comparison of a calcined mixed oxide and its corresponding catalyst with gold. No typical reflections of metallic gold or any kind of gold were observed, indicating that the gold nanoparticles are small (they are less than 5 nm in size, which is the detection limit of the diffractometer) and are well dispersed over the mixed oxide CuO-ZnO-Ah03. The WGS reaction was carried out in a team of its own design. The typical gas mixtures used for the water gas shift reaction were: Model Mix: 4.5% CO in Ar (Abelló Linde); 30% H20 (0.024 mL / min H20 (1). Industrial Conditions (imitating the output of an ethane reformer): 9% CO (Abelló Linde); 11% CO2 (Abelló Linde); 50% H2 (Abelló Linde) ; 30% H20 (0.024 mL / min H20 (1). Figure 2 shows the results of catalytic activity of the systems where
    M 23
    + / M + remained fixed at 1 and gold was deposited by the assisted anion exchange method. Figure 2A compares the activity of the mixed oxides with those of their corresponding supported gold catalysts under ideal conditions (model mixture described above). Within the mixed oxides, the ratio CuO / ZnO = 2, B and 5.6 appear to be the optimum, achieving equilibrium conversions at 330 ° C. Gold systems have a much higher activity than their corresponding supports. Balance conversions are achieved practically
    since the beginning of the reaction making these systems very catalytic
    promising and superior to the current industrial systems of "water gas shift" at low temperature. In Figure 2B the supported gold systems are tested under realistic operating conditions (industrial conditions described above). Solids with Cu / Zn lA and 2.8 ratios reach equilibrium at 270 ° C, the Au_HT 2.8 system being the most active in the entire temperature range studied.
    Frequently, from an industrial point of view, the stability of the catalyst is more important than the catalytic activity itself being this factor, the stability in determining operating conditions when selecting a catalyst. Figure 3A shows the stability of one of the Au / CuO-ZnO / Ab03 systems synthesized by the deposit precipitation method under industrial conditions. Specifically, it is a system with relation (Cu + Zn) / AI = 2 and the relation Cu / Zn = 5.6 named as Au / HT_2. The catalyst loses activity slightly in the first 14 hours of operation (70 to 65% Ca conversion). After this period, the steady state is reached and the ac conversion remains high and stable. It should be noted that the temperature of the stability test is very low 220 ° C and therefore the performance of this catalyst considering the high activity and the good stability shown at such a low temperature is excellent and exceeds the catalysts currently used in the industry based on CuO / ZnO for the reaction of water gas shift at low temperature.
    In addition to continuous stability, it is vitally important to check the strength of the catalyst in start / stop cycles. Start / stop cycles involve lowering the temperature in reaction mixture to room temperature (approximately 30 ° C) and maintaining this situation for 40 minutes (always with gases and water flowing through the catalytic bed). After this period, the system is heated again to the stability test temperature (220ºC). The latter assumes that the catalyst will come into contact with liquid water. The selected catalyst was able to successfully tolerate up to four stop and start cycles without showing any deactivation. This result is
    quite promising and makes the catalysts studied very suitable
    for WGS processes in both stationary and portable applications. It should be noted that in all catalytic tests the reaction mixture, once stabilized, flows directly over the catalyst. In other words, it is not done
    5 no activation pretreatment. The catalysts are activated directly in the reaction mixture which is an additional advantage in view of possible applications in continuous-working fuel processors. The results of activity and stability as a whole are quite satisfactory considering the benefits offered by the catalysts that exist
    10 currently on the market, making these systems promising candidates for direct application in real processes of hydrogen stream purification.
    权利要求:
    Claims (10)
    [1]

    [8]
    8. Method according to claim 7, characterized in that Cu (N03h.2H20, Zn (N03h.6H20 and AI (N03h.9H20 as precursors and Na2C03 1M as precipitating agent) are used, the precipitation being maintained for a period of 48 h.
    [9]
    9. Method according to any one of claims 7 and 8, characterized in that after precipitation, drying is carried out at a temperature between room temperature and 100 ° C, followed by subsequent calcination at 300 ° C for 4 hours with a ramp of 10 ° C / min.
    [10]
    10. Method according to any one of claims 6 to 9, characterized in that the deposition of Au is carried out by direct anion exchange assisted by NH3.
    [11]
    11. Method according to claim 10, characterized in that it is based on an aqueous solution of HAuCI4 to which the support is added.
    [12]
    12. Method according to any one of claims 6 to 9, characterized in that the deposition of Au is carried out by precipitation-deposition.
    [13]
    13. Method according to claim 12, characterized in that the Au is deposited in the form of auric hydroxide in the oxide layers under stirring at constant pH.
    [14]
    14. Use of a catalyst as defined in claims 1 to 5 in the water gas displacement reaction.
    [15]
    15. Use according to claim 14, characterized in that the reaction takes place in reactive currents with a composition comprising: - between 4.5% and 9% of CO - between 0 and 11% of CO2 - between 30 and 50% of H20
    [16]
    16. Use according to claims 14 and 15, characterized in that the reaction is carried out at a temperature between 140 and 350 ° C and at a spatial speed between
    5 4000 and 8000 h-1.
    (') or (') B
    20 30 40 50 60 70 80 20 40 60 80 2theta 2theta
    and
    (CuO --HT calcined Cu / Zn 5.6 (pre reaction)., Cu --HT calcined Cu / Zn 5.6 (post reaction)
    e e e.,.,
     Figure 1
    -
    ~
    or
    -
    or
    OR
    s ::
    orF
    ~
    O o
    250 300 350
    Temperature (OC)
    -
    ~ o
    Or 60
    s ::
    "
    OR
    '¡¡
    ..
    el) 40
    AND:
    OR
    "
    o ~ - ~ ---- ~ - ~ ---- ~ - ~ ---- ~ - ~~ - ~
    200 250 300 350 Temperature (OC)
    Figure 2
     80, -------------------------------------------, 
    70 60 ~ 50
    OR
    i (,) e 40
    or
    30 or 20 10
    70 60
    -
    fI. fifty
    -
    OR
    (,)
    e.; or 30
    ~
    or
    OR
    TO
    0 ')' "Y} -____> --___-.;. ()
    - '1o') ')' Y'J ') - O -r> _i) ... ,, · .F> oo
     GHSV = 4000 ho1
    T = 220 ° C
    gas mixture = 30% H0 + 9% CO + 11% CO + 50% H
    2 2
    or 5 10 15 20 25 30 35 40 45
    time (h)
    OR
    2. 3. 4
     no cycles
    Figure 3
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