Patent Application
20140205533
The present invention relates to a process for the production of chlorine by thermo-catalytic gas phase oxidation of hydrogen chloride and oxygen, comprising at least (1) a cerium oxide catalyst and (2) an adiabatic reaction cascade, containing at least two adiabatic stages connected in series with intermediate cooling, wherein the molar O2/HCl-ratio is equal or above 0.75 in any part of the cerium oxide catalyst beds.
The catalytic oxidation of hydrogen chloride with oxygen in an exothermic equilibrium reaction was developed by DEACON in 1868 and constituted the first industrial route for chlorine production:
4 HCl+O2→2Cl2+2 H2O
However, the Deacon process was pushed severely into the background with the introduction of the chlor-alkali industry. Virtually the entire production of chlorine was by electrolysis of aqueous sodium chloride solutions (Ullmann Encyclopedia of Industrial Chemistry, seventh release, 2006). However, the Deacon process has recently attracted renewed interest, since the worldwide demand for chlorine is growing faster than the demand for sodium hydroxide solution. The process for the preparation of chlorine by oxidation of hydrogen chloride, which is unconnected with the preparation of sodium hydroxide solution, can support this demand. Furthermore, hydrogen chloride is obtained as a linked product in large quantities, for example, in phosgenation reactions, as in the preparation of isocyanates.
The first catalysts for oxidation of hydrogen chloride contained copper in chloride or oxide form as the active component and were already described by Deacon in 1868. These catalysts were shown to rapidly deactivate as a consequent of volatilization of the active phase at the high operational temperatures.
The oxidation of hydrogen chloride with catalysts based on chromium oxide is known. However, chromium catalysts are prone to form chromium(VI) oxide under oxidizing conditions, which is a ver toxic substance. Also a short catalyst lifetime is assumed in other publications (WO 2009/035234 A, page 4, line 10).
First catalysts for the oxidation of hydrogen chloride containing ruthenium as the catalytically active component were described in 1965. Such catalysts were, starting from RuCl3 for example, supported on silicon dioxide and aluminum oxide (DE 1567788). However, the activity of the RuCl3/SiO2 catalysts was very low. Further Ru-based catalysts with the active mass of ruthenium oxide, ruthenium mixed oxide or ruthenium chloride and various oxides, such as e.g., titanium dioxide, zirconium dioxide, tin oxide etc., as the support material has also been described (EP 743277, U.S. Pat. No. 5,908,607, EP 2026905, and EP 2027062). In such catalysts, the content of ruthenium oxide is generally 0.1 wt. % 20 wt.
The ruthenium-based catalysts have a quite high activity and stability at temperatures up to 350-400° C. But the stability of ruthenium-based catalysts at temperatures above 350-400° C. is still not proven (WO 2009/035234 A, page 5, line 17). Furthermore, the platinum group element ruthenium is highly expensive, very rare and the world market price is unsteady, thus making commercialization of such a catalyst difficult.
Cerium oxide catalysts for the thereto-catalytic HCl-oxidation are known from DE 10 2009 021 675 A1 and WO 2009/035234 A2. In both patent applications similar cerium oxide catalyst systems are described. WO 2009/035234 A2 speculates about the stability of cerium oxide catalysts (page 8, line 4) without providing adequate examples (only 2 h time on stream). The catalysts are preferably applied at temperatures below 400° C. (page 12, line 23) and in particles of 100 nm to 100 μm size (page 12, line, 1), preventing overheating of the catalyst by the exothermic reaction (age 12, line 3), which is indicative of the use in an isothermal reaction (e.g. fluidized bed). DE 10 2009 021 675 A1 speculates about possible reaction conditions fin a cerium oxide catalyst ([0058] or claim 15: “the volume ratio of HCl to oxygen is preferably in the range of 1:1 to 20:1, more preferably in the range of 2:1 and 8:1 and even more preferably in the range of 2:1 and 5:1”), indicating that even a stoichiometric amount or even excess of HCl is most preferable. DE 10 2009 021 675 also speculates about the possible implementation of cerium oxide in an adiabatic reaction cascade ([0051-0053]), without providing as examples to prove these speculations. Consequently, there is still a lack of knowledge regarding how to apply the known cerium oxide catalysts to known reaction systems reaching a long-term stable and cost-efficient production of chlorine from HCl and oxygen.
Accordingly one object of the present invention is to provide a catalytic reaction process for the long-term stable and cost-efficient production of chlorine from HCl and oxygen.
A “stage” or an “adiabatic stage” of an adiabatic reaction cascade is understood as one logic modular part of an adiabatic reaction cascade. In more detail, the first “stage” is understood as the part including a reaction zone of the adiabatic reaction cascade between the (first) HCl inlet and the end of an intermediate cooling zone. The second stage is understood as the part of the adiabatic reaction cascade between the end of a first intermediate cooling and a second intermediate cooling zone, also including a reaction zone. A reaction zone can comprise two or more reaction sub zones. The definition of further stages is similar, continuing the counting in stages number and intermediate cooling number. Logically, after the last stage of the adiabatic reaction cascade there is no intermediate but a final cooling zone. Two preferred embodiments are visualized for better understanding in the
Subject matter of the invention is a process for the production of chlorine by thermo-catalytic gas phase oxidation of hydrogen chloride gas with oxygen in the presence of a catalyst, and separation of the chlorine from the reaction products comprising chlorine, hydrogen chloride, oxygen and water, characterized in that
In a preferred embodiment, the molar O2/HCl-ratio is equal or above 1 in any part of the cerium oxide catalyst beds. In a more preferred embodiment, the molar O2/HCl-ratio is equal or above 1.5 in any part of the cerium oxide catalyst beds. In an even more preferred embodiment, the molar O2/HCl-ratio is equal or above 2 in any part of the cerium oxide catalyst beds. The O2/HCl-ratio throughout this description is understood as molar O2/HCl-ratio.
In a preferred embodiment of the invention, the process is carried out in an adiabatic reaction cascade having 3 to 7 adiabatic stages.
In another preferred embodiment a so called split HCl-injection is applied, i.e. not the total HCl amount to be converted is fed into the first adiabatic stage (see examples 13/14 and
More preferably, fresh HCl is fed into all adiabatic stages, except the last. By applying a split HCl-injection strategy the O2/HCl-ratio can be kept at a higher level at the inlet of the 1st adiabatic stage as if the total HCl amount would be fed to the 1st adiabatic stage (compare graph 1).
The preferred process is characterized in that the temperature of the cerium oxide catalyst is kept in the range of 200 to 600° C. in any reaction zone of the adiabatic reaction cascade, in particular by keeping the inlet gas temperature of any reaction zone at a temperature of at least 200° C. and keeping the outlet temperature of the reaction gases of each reaction zone at a temperature of at last 600° C. Particular preferred this is achieved by controlling the temperature of each catalyst bed via controlling the gas stream. In a very particular preferred embodiment the temperature control is achieved by controlling the amount of HCl gas compared to the amount of the whole inlet gas stream to a respective reaction zone.
In a more preferred embodiment of the invention, the temperature of the cerium oxide catalyst is kept in the range of 250-500° C. in any stage of the adiabatic reaction cascade. Significantly below 250° C. the activity of the cerium oxide catalyst is very low. Significantly above 500° C. typically applied nickel-based materials of construction are not long-term stable against the reaction conditions.
In another preferred embodiment of the invention, the outlet gas temperature of the reaction zone of the last adiabatic stage is controlled via the composition of the educt gas stream entering the preceding reaction stages to be at last 450° C., more preferably at last 420° C.
The preferred process is characterized in that the outlet gas temperature of the reaction zone of the last adiabatic stage is kept lower than the outlet gas temperature of each preceding reaction zone of the other adiabatic stages. It is advantageous to lower the outlet gas temperature of the reaction zone of the last adiabatic stage to shift the equilibrium of the reaction to the products, thus enabling higher HCl-conversion, whereas the outlet gas temperature of the reaction zone in any other adiabatic stages should be as high as possible, limited by the stability of construction materials and the equilibrium limitations, to improve cerium oxide utilization.
In a preferred embodiment, the absolute pressure in the adiabatic reaction cascade is kept in the range of 2-10 bar (2000 to 10000 hPa), more preferably in the range of 3-7 bar (3000 to 7000 hPa).
The preferred process is characterized in that a catalyst is used comprising ruthenium metal and/or ruthenium compounds and cerium oxide as catalytically active components. Another preferred variant of the new process is characterized in that at least two different types of catalysts are present in different reaction zones, wherein a first type of catalyst comprises ruthenium metal and/or ruthenium compounds as catalytically active component and a second type of catalyst comprises cerium oxide as catalytically active component.
Another preferred embodiment of the process is characterized in that the ruthenium based catalyst is applied in a reaction zone with a gas temperature in the range of 200 to 400° C., whereas the cerium oxide catalyst is applied in a reaction zone with a gas temperature in the range of 300 to 600° C.
More preferably, the ruthenium based catalyst is applied in a reaction zone with a gas temperature in the range of 250 to 400° C., whereas the cerium oxide catalyst is applied in a reaction zone with a gas temperature in the range of 350 to 500° C., if such a combination is used.
Another preferred embodiment of the process is characterized in that at least one adiabatic reaction zone comprises at least two reaction sub zones, a first reaction sub zone comprising a ruthenium based catalyst and a second reaction sub zone comprising a cerium oxide catalyst.
More preferably, the reaction zone of the last adiabatic stage contains only a ruthenium based catalyst. Even more preferably, all adiabatic stages contain two reaction sub zones: a first reaction sub zone always contains a ruthenium-based catalyst and a second reaction sub zone always contains a cerium oxide catalyst, except the last adiabatic stage, which contains a ruthenium-based catalyst only.
Another preferred variant of the process is characterized in that during operation of the process the initial activity of the cerium oxide catalyst is restored by raising the ratio of O2/HCl, preferably by lowering the amount of HCl, particularly preferred raising the ratio of O2/HCl to the double, and particularly keeping the raised ratio of O2/HCl for a period of about at least half an hour and then returning to the previous ratio of O2/HCl.
Preferably, the O2/HCl-ratio to partly restore the activity is equal or above 2, more preferably equal or above 5, even more preferably the HCl-feed is completely stopped (HCl/O2=0). The time period to restore the activity is preferably below 5 h, more preferably equal or below 2 h and even more preferably equal or below 1 h. The temperature range for partly restoring the initial activity is preferably approximately similar as described for regular operation.
In a preferred embodiment, the cerium oxide catalyst used in the new process is pre-calcined during its preparation at a temperature of 500° C. to 1100° C., more preferably in a temperature range of 700 to 1000° C. and most preferably at approximately 900° C. Preferably, calcination is carried out under oxidizing conditions, in particular under air-similar conditions. The calcination period is preferably in the range of 0.5-10 h, more preferably approximately 2 h. A pre-calcination improves the resistance of the catalyst against formation of CeCl3.6H2O or CeCl3 phases and/or bulk chlorination, which is believed to be a significant catalyst deactivation cause.
In a preferred embodiment, the cerium oxide catalyst does not exhibit X-ray diffraction reflections which are characteristic for CeCl3.6H2O or CeCl3 phases during or after use. X-ray analysis is done according to example 10. Therefore a process is preferred, which is characterized in that a cerium oxide catalyst is used in the new process which comprises no CeCl3.6H2O or CeCl3 phases, and which in particular does not exhibit significant X-ray diffraction reflections which are characteristic for CeCl3.6H2O or CeCl3 phases.
In another preferred embodiment, less than 3 theoretical layers of oxygen in the cerium oxide catalyst are exchanged by chlorine during or after use. Hence a process is preferred which is characterized in that cerium oxide catalyst used in the process will be subjected to a activity restoring treatment at increased molar O2/HCl-ratio as described above or replaced by fresh catalyst if more than 3 theoretical layers of oxygen in the cerium oxide catalyst are exchanged by chlorine during use of the catalyst.
More preferably, less than 2 theoretical layers of oxygen in the cerium oxide catalyst are exchanged by chlorine during or after use. This is proven by nitrogen adsorption and X-ray photoelectron spectroscopy according to example 11.
Preferably, the cerium oxide catalyst and/or the ruthenium based catalyst is a supported catalyst. Suitable support materials are silicon dioxide, aluminum oxide, titanium oxide, tin oxide, zirconium oxide, or their mixtures.
Preferably, the content of cerium oxide (calculated as CeO2) is 1-30% of the total amount of the calcined catalyst. More preferably, the content of cerium oxide (calculated as CeO2) is 5-25% of the total amount of the calcined catalyst. Even more preferably, the content of cerium oxide (calculated as CeO2) is approximately 15% of the total amount of the calcined catalyst.
It is understood, that a supported or unsupported cerium precursor component catalyst could be also calcined in the reactor(s) even during the HCl oxidation operation to get the final cerium oxide catalyst, as it is described e.g. in DE 10 2009 021 675 A1, its disclosure being incorporated here by reference.
Suitable cerium oxide catalysts for the new process, their preparation and properties are generally known from DE 10 2009 021 675 A1, its disclosure being incorporated here by reference. Suitable ruthenium-based catalysts for the new process, their preparation and properties are generally known from EP 743277, U.S. Pat. No. 5,908,607, EP 2026905 or EP 2027062 their specific disclosure being incorporated here by reference. The manifold advantages of an adiabatic reaction cascade are generally known from EP 2027063 which disclosure being incorporated here by reference as well.
The conversion of hydrogen chloride in a single pass can preferably be limited to 15 to 90%, preferably 40 to 90%, particularly preferably 50 to 90%. Some or all of the unreacted hydrogen chloride can be recycled into the catalytic hydrogen chloride oxidation after being separated off.
The heat of reaction of the catalytic hydrogen chloride oxidation can be used in an advantageous manner for generation of high pressure steam. This can be used for operation of a phosgenation reactor and/or of distillation columns, in particular isocyanate distillation columns.
In a last step of the new process, the chlorine formed is separated off under generally known conditions. The separating step conventionally comprises several stages, namely separating off and optionally recycling unreacted hydrogen chloride from the product gas stream of the catalytic hydrogen chloride oxidation, drying of the stream obtained, which essentially contains chlorine and oxygen, and separating off chlorine from the dried stream.
The separating of unreacted hydrogen chloride, and of the steam formed, can be carried out by condensing aqueous hydrochloric acid out of the product gas stream of the hydrogen chloride oxidation by cooling. Hydrogen chloride can also be absorbed into dilute hydrochloric, acid or water.
The invention will now be described in further detail with reference to the figures and the following non-limiting examples.
A supported cerium oxide catalyst was prepared by: (1) Incipient wetness impregnation of an alumina carrier from Saint-Gobain Norpro (SA 6976, 1.5 mm, 254 m2/g) with an aqueous solution of commercial cerium (III)chloride heptahydrate (Aldrich, 99.9 purity), followed by (2) drying at 80° C. for 6 h and (3) calcination at 700° C. for 2 h. The final load after calcination calculated as CeO2 was 15.6 wt. % based on the total amount of catalyst.
The cerium oxide catalyst from example 1 was crushed to a sieve fraction (100-250 μm particle diameter).
1 g of the cerium oxide catalyst from example 1 as prepared was filled into a tube (8 mm inner diameter) for each experiment. The catalyst in the tube was heated up under nitrogen flow. After reaching steady conditions, a gas mixture of HCl and oxygen (see table 1) was fed to the tube at 430° C. under approximately atmospheric pressure. By trace heating of the tube the temperature was kept constant at 430° C. Several times the product stream was passed through a sodium iodide solution (20 wt. % in water) for approximately 15 min and the thereby produced iodine was titrated with a 0.1 N thiosulfate-solution. The space time yield (STY) was calculated by using the following equation:
Space time yield [g/gh]=mCl2×mcatalyst−1×tsampling−1
Wherein mCl2 is the amount of chlorine, mcatalyst is the amount of catalyst which was used and tsampling is the sampling time.
The supported cerium oxide catalyst from example 1 gets rapidly deactivated at an O2/HCl-ratio below 0.75. Although the HCl partial pressure is high (compared to example 4), the equilibrated STY is very low.
1 g of the cerium oxide catalyst from example 1 was used for each experiment. The arrangement and the execution of the experiments were equal as in example 3, except that the gas flows were varied. Results are listed in table 2.
Evaluation:
Although the HCl partial pressure is 2.6-6 times lower (compared to example 3), the equilibrated activity under a sufficient O2/HCl-ratio equal or above 0.75 is 3-6.5-times higher than under an insufficient O2/HCl-ratio below 0.75. The initial deactivation during equilibration is also much less pronounced at a sufficient O2/HCl-ratio equal or above 0.75.
1 g of the sieve fraction (100-250 μm) from example 2 was diluted by 4 g of spheri glass and filled into a tube for each experiment. The catalyst in the tube was heated up under nitrogen flow. After reaching steady conditions, a gas mixture of HCl and oxygen as indicated in table 3 were fed to the tube at 400° C. under approximately atmospheric pressure. By trace heating of the tube the temperature was kept constant at 400° C. over the time on stream. Several times the product stream was passed through a sodium iodide solution (20 wt. % in water) and the thereby produced iodine was titrated with a 0.1 N thiosulfate-solution. The HCl-conversion was calculated by using the following equation:
HCl-conversion [%]=2×nCl2×nHCl−1×100%
Wherein nCl2 is the titrated molar amount of chlorine and nHCl is the fed molar amount of HCl in the same time period.
1HCl-conversion at x min. 3 in mmol/min
Evaluation:
At an O2/HCl-ratio below 0.75 the HCl-conversion is at a very low level, with underlying strong deactivation trend.
1 g of a sieve fraction (100-250 μm) from example 2 was used. The arrangement and the execution of the experiments were equal as in example 4, except that the gas flows were varied (table 4).
1HCl-conversion at x min, 3 in mmol/min
Evaluation:
The higher the O2/HCl-ratio is, the higher the HCl-conversion is. At an O2/HCl-ratio equal or above 0.75 the deactivation is only minor
1 g of the cerium oxide catalyst from example 1 as prepared was filled into a tube (8 mm inner diameter). The catalyst in the tube was heated up under nitrogen flow. After reaching steady conditions, 1 L/h HCl, 4 L/h O2 and 5 L/h N2 were fed to the tube at 430° C. under approximately atmospheric pressure. By trace heating of the tube the temperature was kept constant at 430° C. Several times the product stream was passed through a sodium iodide solution (20 wt. % in water) for approximately 15 min and the thereby produced iodine was titrated with 0.1 N thiosulfate-solution (table 5). The space time yield was calculated by using the following equation:
Space time yield [g/gh]=mCl2×mcatalyst−1×tsampling
Wherein mCl2 is the amount of chlorine, mcatalyst is the amount of catalyst which was used and tsampling is the sampling time.
Evaluation:
The activity of the supported cerium oxide catalyst from example 1 after equilibration (compare example 4) is very stable at an O2/HCl-ratio equal or above 0.75.
80 g of the cerium oxide catalyst from example 1 as prepared were filled into a tube (14 mm inner diameter, 1.5 m length, including an inner tube with moveable thermocouple). The catalyst inside the tube was heated up under a preheated nitrogen flow. After reaching steady conditions, 0.3 mol/h HCl and 0.75 mol/h oxygen (O2/HCl-ratio of 2.5) under approximately atmospheric pressure were fed to the tube. By pre-heating of the gas mixture and trace heating of the tube the temperature profile was kept approximately constant over 5005 h time on stream (table 6). Several times the product stream was passed through a sodium iodide solution (20 wt. % in water) for approximately 15 min and the thereby produced iodine was titrated with a 0.1 N thiosulfate-solution (table 7). The HCl-conversion was calculated by using the following equation:
HCl-conversion [%]=2×nCl2×nHCl−1×100%
Wherein nCl2 is the titrated molar amount of chlorine and nHCl is the fed molar amount of HCl in the same time period.
The process condensate (saturated hydrochloric acid at room temperature) was sampled three times: after 671 h, 1127 h and 3253 h time on stream. According to ICP-OES analysis the alumina content in the condensate was always below 2 wt. ppm (671 h, 1127 h) and even below 0.5 wt. ppm after 3253 h. The cerium content in the condensate was always similar or below 0.3 wt. ppm!
Evaluation:
At an O2/HCl-ratio of 2.5 only a very minor deactivation is observable over 5005 h time on stream! Based on condensate analysis the estimated percentage loss of cerium and alumina is below 0.1% over 5005 h time on stream. Consequently the loss of catalyst constituents is negligible, which is a further proof for catalyst stability.
Cerium oxide powder (Aldrich, nanopowder) was calcined at 900° C. for 5 h. For each experiment 0.5 g of the calcined sample (particle size=0.4-0.6 mm) was filled into a tube (8 mm inner diameter). The catalyst powder inside the tube was heated up under nitrogen flow. After reaching steady conditions, HCl, O2 and N2 were fed under approximately atmospheric pressure to the tube. By trace heating of the tube the catalyst temperature was kept constant at 430° C. The O2/HCl ratio was varied between 0.5 and 7, keeping the partial pressure of HCl constant, and between 0.25 and 2, keeping the oxygen partial pressure constant. After 1 h time on stream in each O2/HCl ratio the outlet gas was passed through a sodium iodide solution (2 wt. % in water) for approximately 5 min and the thereby produced iodine was titrated with 0.1 M sodium thiosulfate solution. The HCl-conversion was calculated by using the following equation:
HCl-conversion [%]=2×nCl2×nHCl−1×100%
Wherein nCl2 is the titrated molar amount of chlorine and nHCl is the fed molar amount of HCl in the same time period.
Evaluation:
An increase of the O2/HCl ratio appears beneficial to achieve higher conversion levels in the low O2/HCl-ratio range. In particular, an increase of the O2/HCl-ratio from 0.25 to 0.5 (g-h-i) improves the HCl-conversion by a factor of 7, while an increase of the O2/HCl-ratio from 1 to 7 improves the HCl-conversion only by a factor of 2. Consequently, at O2/HCl ratios below 0.75 the process economics can be dramatically optimized by increasing the O2/HCl-ratio, whereas at O2/HCl-ratios equal or above 0.75 one has to balance surplus oxygen costs (running) against catalyst costs (one time). Consequently, experiments b-f and j-k are recognized as according to the invention, whereas experiments a and g-i are considered as comparative examples.
Note that the equilibration of an unsupported cerium oxide powder catalyst is assumed to be much faster than the equilibration of a supported, pelletized catalyst. The observed HCl-conversion is accordingly treated as nearly equilibrated. Longer equilibration times would have resulted in substantially identical HCl-conversion levels for O2/HCl-ratios equal or above 0.75, but in even lower activity levels for O2/HCl-ratios below 0.75, shown to lead to deactivation. This point is further detailed in Example 12.
X-Ray diffraction phase analysis (PAN analytical X′Pert PRO-MPD diffractometer, 10-70° 2θ range, angular step size of 0.017° and a counting time of 0.26 s per step;
Evaluation:
After treatment of the cerium oxide sample calcined at 900° C. in a feed with an O2/HCl-ratio of 2 the XRD pattern (b) only shows the characteristic reflexions of CeO2. After treatment of cerium oxide calcined at 900° C. in a feed with O2/HCl-ratios of 0 or 0.25 reflexions specific to CeCl3.6H2O are as well evidenced in appreciable intensity. After treatment of cerium oxide calcined at 900° C. in a feed with an O2/HCl-ratio of 0.75 the diffractogram only shows the characteristic reflexions of CeO2. Diffraction lines specific to CeCl3.6H2O, if present, are not distinguishable from the noise. The XRD pattern of the cerium oxide sample calcined at 500° C. and treated in a feed with O2/HCl ratio of 0 evidences the presence of CeCl3.6H2O and in higher amount with respect to the cerium oxide sample calcined at 900° C. and similarly treated. Consequently, we believe that the deactivation of the cerium oxide catalyst, observed at O2/HCl-ratios below 0.75, is caused by the formation of the CeCl3.6H2O phase, which is much less active in HCl-oxidation than CeO2 (see also Example 11). Furthermore, calcination of cerium oxide at higher temperatures (900° C.) seems to result in a catalyst better resistant to chlorination.
Cerium oxide powder (Aldrich, nanopowder) was calcined at 500° C. and 900° C. for 5 h (table 9) and from 300° C. to 1100° C. for 5 h respectively (table 10). The calcined catalyst samples were further treated in O2/HCl=2 at 430° C. for 3 h (label O2/HCl=2 in table 9, table 10) or in O2/HCl=0 at 430° C. for 3 h (label O2/HCl=0 in table 9). The fresh samples (table 10) and the treated samples (table 9) were analyzed by nitrogen adsorption to measure their surface area (Quantachrome Quadrasorb-SI gas adsorption analyzer, BET-method) and X-ray photoelectron spectroscopy to assess the degree of surface chlorination (Phoibos 150, SPECS, non-monochromatized Al Kα (1486.6 eV) excitation, hemispherical analyzer).
1Calculated by model IMFP with inelastic mean free path of 22 Angström (by TPP-2M)
Evaluation:
For the unsupported cerium oxide powder sample pre-calcined at 500° C. and treated with an O2/HCl-ratio of 2, only 1-2 theoretical layer of oxygen are exchanged by chlorine (some of the detected chlorine could also be related to adsorbed chlorine on the catalyst surface), whereas after a treatment with an O2/HCl-ratio of 0.5-6 theoretical layer of oxygen are exchanged by chlorine. The cerium oxide samples pre-calcined at 900° C. exhibit a similar but very less pronounced effect (1 theoretical layer versus 2-3 theoretical layers). The results are in line with the bulk chlorination detected by XRD analysis (Example 10), confirming the postulated relationship between deactivation and CeCl3.6H2O phase formation. Calcination of cerium oxide at temperatures in the range of 300-1100° C. produces materials with different initial surface areas (decreasing with increasing calcination temperature, table 10). Contrarily, the surface area values of the samples calcined at 500° C. drops significantly after treatment either in O2/HCl=2 or 0 while that of the sample calcined at 900° C. and equally treated is changed to minor extent (table 9). Thus, calcination at higher temperature is beneficial to obtain a stabilized catalyst and is the feasible origin of the higher resistance towards chlorination shown by XRD (Example 10) and XPS.
Cerium oxide powder (Aldrich, nanopowder) was calcined at 900° C. for 5 h. For each experiment 0.5 g of the calcined powder was filled into a tube (8 mm inner diameter). The catalyst powder inside the tube was heated up under nitrogen flow. After reaching steady conditions, experiments were carried out at 430° C. combining a deactivation step, in which the catalyst was exposed to a not inventive feed composition O2/HCl=0 (3 h) or 0.25 (5 h), and a regeneration step (inventive), in which excess of oxygen was fed (O2/HCl=2 or 7) for 2 h in order to study the reoxidation of the catalyst.
Evaluation:
A progressive decrease in activity is observed with O2/HCl=0.25 (table 11, experiment 1). Upon increasing the O2 content in the feed (O2/HCl=2), the activity is slowly restored. However, the activity level expected for the O2/HCl=2 feed composition (HCl conversion=22%, Example 9) is not completely reached within 2 h. Regeneration with O2/HCl=7 is on the other hand extremely fast (table 11, experiment 2). This evidence supports chlorination of the catalyst (Example 10) in the deactivation phase and fast chlorine displacement by excess oxygen.
When performing the deactivation phase in O2/HCl=0 (table 11, experiment 3) the catalyst activity is logically completely lost in 3 h. In Example 10 it is shown that cerium oxides indeed chlorinated to larger extent in the presence of the sole HCl. Still, regeneration in O2/HCl=7 fully restores the original activity in 1 h.
As feed streams 1.37 kmol/h HCl, 0.69 kmol/h O2, 0.03 kmol/h Cl2, 0.08 kmol/h H2O and 0.38 kmol/h N2 are provided at approximately 5 bar (gauge). The HCl feed split, the inlet and outlet temperatures of the adiabatic stages and other relevant parameter are provided in table 1. The minimal O2/HCl-ratio is 0.84 for the inlet of the 4th adiabatic stage. Note that the minimal O2/HCl-ratio is always at the inlet of a catalyst bed due to the reaction stoichiometry (4 moles of HCl converted per mol of oxygen).
Feed streams are equal as in example 13, feed streams are provided at approximately 5 bar (gauge). The HCl feed split, the inlet and outlet temperatures of the adiabatic stages and other relevant parameter are provided in table 13. There are two reaction sub zones in the 1st adiabatic stage (1a/b) and 2nd adiabatic stage (2a/b). The first reaction sub zone contains a ruthenium-based catalyst (a), the second reaction sub zone contains a cerium oxide catalyst (b). In the 3rd adiabatic stage only a ruthenium-based catalyst is applied. The minimal O2/HCl-ratio for the cerium oxide catalyst is 0.75 for the inlet of the (cerium oxide catalyst containing) 2nd reaction zone (2b). Note that the minimal O2/HCl-ratio is always at the inlet of a catalyst bed due to the reaction stoichiometry (4 moles of HCl converted per mol of oxygen).
25 g of the cerium oxide catalyst from example 1 as prepared were filled into a tube (21 mm inner diameter, 330 mm length, including an inner tube with moveable thermocouple). The catalyst inside the tube was heated up under a preheated nitrogen flow. After reaching steady conditions, varying gas feeds under approximately 4 bar (gauge) were fed to the tube (table 14). Two times (after 60 min and 120 min) the product stream was passed through a sodium iodide solution (20 wt. % in water) and the thereby produced iodine was titrated with a 0.1 N thiosulfate-solution (table 7). The HCl-conversion was calculated by using the following equation:
Space time yield [g/gh]=mCl2×mcatalyst−1×tsampling−1
Wherein mCl2 is the amount of chlorine, mcatalyst is the amount of catalyst which was used and tsampling is the sampling time. In table 14 the average value of the two titrations is given.
Evaluation:
At an O2/HCl-ratio of 2.5 the cerium oxide catalyst exhibits a sufficient activity at 276° C. and at 400° C.
| Number | Date | Country | Kind |
|---|---|---|---|
| 11172624.6 | Jul 2011 | EP | regional |
| Filing Document | Filing Date | Country | Kind | 371c Date |
|---|---|---|---|---|
| PCT/EP2012/062801 | 7/2/2012 | WO | 00 | 3/25/2014 |
