WO2009035234A2 - Process for the chlorine by oxidation of hydrogen chloride - Google Patents
Process for the chlorine by oxidation of hydrogen chloride Download PDFInfo
- Publication number
- WO2009035234A2 WO2009035234A2 PCT/KR2008/005241 KR2008005241W WO2009035234A2 WO 2009035234 A2 WO2009035234 A2 WO 2009035234A2 KR 2008005241 W KR2008005241 W KR 2008005241W WO 2009035234 A2 WO2009035234 A2 WO 2009035234A2
- Authority
- WO
- WIPO (PCT)
- Prior art keywords
- cerium
- catalyst
- hydrogen chloride
- compound
- chlorine
- Prior art date
Links
- 238000000034 method Methods 0.000 title claims abstract description 60
- 239000000460 chlorine Substances 0.000 title claims abstract description 47
- 229910052801 chlorine Inorganic materials 0.000 title claims abstract description 47
- ZAMOUSCENKQFHK-UHFFFAOYSA-N Chlorine atom Chemical compound [Cl] ZAMOUSCENKQFHK-UHFFFAOYSA-N 0.000 title claims abstract description 46
- VEXZGXHMUGYJMC-UHFFFAOYSA-N Hydrochloric acid Chemical compound Cl VEXZGXHMUGYJMC-UHFFFAOYSA-N 0.000 title claims abstract description 44
- IXCSERBJSXMMFS-UHFFFAOYSA-N hydrogen chloride Substances Cl.Cl IXCSERBJSXMMFS-UHFFFAOYSA-N 0.000 title claims abstract description 32
- 229910000041 hydrogen chloride Inorganic materials 0.000 title claims abstract description 32
- 230000008569 process Effects 0.000 title abstract description 13
- 230000003647 oxidation Effects 0.000 title description 16
- 238000007254 oxidation reaction Methods 0.000 title description 16
- 239000003054 catalyst Substances 0.000 claims abstract description 69
- 239000007789 gas Substances 0.000 claims abstract description 15
- QVGXLLKOCUKJST-UHFFFAOYSA-N atomic oxygen Chemical compound [O] QVGXLLKOCUKJST-UHFFFAOYSA-N 0.000 claims abstract description 8
- 239000001301 oxygen Substances 0.000 claims abstract description 8
- 229910052760 oxygen Inorganic materials 0.000 claims abstract description 8
- 150000001785 cerium compounds Chemical class 0.000 claims description 41
- HSJPMRKMPBAUAU-UHFFFAOYSA-N cerium(3+);trinitrate Chemical compound [Ce+3].[O-][N+]([O-])=O.[O-][N+]([O-])=O.[O-][N+]([O-])=O HSJPMRKMPBAUAU-UHFFFAOYSA-N 0.000 claims description 14
- 229910000420 cerium oxide Inorganic materials 0.000 claims description 11
- BMMGVYCKOGBVEV-UHFFFAOYSA-N oxo(oxoceriooxy)cerium Chemical compound [Ce]=O.O=[Ce]=O BMMGVYCKOGBVEV-UHFFFAOYSA-N 0.000 claims description 11
- 239000000203 mixture Substances 0.000 claims description 10
- BASFCYQUMIYNBI-UHFFFAOYSA-N platinum Chemical group [Pt] BASFCYQUMIYNBI-UHFFFAOYSA-N 0.000 claims description 10
- VYLVYHXQOHJDJL-UHFFFAOYSA-K cerium trichloride Chemical compound Cl[Ce](Cl)Cl VYLVYHXQOHJDJL-UHFFFAOYSA-K 0.000 claims description 8
- 239000002245 particle Substances 0.000 claims description 8
- XMPZTFVPEKAKFH-UHFFFAOYSA-P ceric ammonium nitrate Chemical compound [NH4+].[NH4+].[Ce+4].[O-][N+]([O-])=O.[O-][N+]([O-])=O.[O-][N+]([O-])=O.[O-][N+]([O-])=O.[O-][N+]([O-])=O.[O-][N+]([O-])=O XMPZTFVPEKAKFH-UHFFFAOYSA-P 0.000 claims description 7
- VGBWDOLBWVJTRZ-UHFFFAOYSA-K cerium(3+);triacetate Chemical compound [Ce+3].CC([O-])=O.CC([O-])=O.CC([O-])=O VGBWDOLBWVJTRZ-UHFFFAOYSA-K 0.000 claims description 7
- GHLITDDQOMIBFS-UHFFFAOYSA-H cerium(3+);tricarbonate Chemical compound [Ce+3].[Ce+3].[O-]C([O-])=O.[O-]C([O-])=O.[O-]C([O-])=O GHLITDDQOMIBFS-UHFFFAOYSA-H 0.000 claims description 7
- LJBTWTBUIINKRU-UHFFFAOYSA-K cerium(3+);triperchlorate Chemical compound [Ce+3].[O-]Cl(=O)(=O)=O.[O-]Cl(=O)(=O)=O.[O-]Cl(=O)(=O)=O LJBTWTBUIINKRU-UHFFFAOYSA-K 0.000 claims description 7
- MMXSKTNPRXHINM-UHFFFAOYSA-N cerium(3+);trisulfide Chemical compound [S-2].[S-2].[S-2].[Ce+3].[Ce+3] MMXSKTNPRXHINM-UHFFFAOYSA-N 0.000 claims description 7
- WXANAQMHYPHTGY-UHFFFAOYSA-N cerium;ethyne Chemical compound [Ce].[C-]#[C] WXANAQMHYPHTGY-UHFFFAOYSA-N 0.000 claims description 7
- OKJMLYFJRFYBPS-UHFFFAOYSA-J tetraazanium;cerium(4+);tetrasulfate Chemical compound [NH4+].[NH4+].[NH4+].[NH4+].[Ce+4].[O-]S([O-])(=O)=O.[O-]S([O-])(=O)=O.[O-]S([O-])(=O)=O.[O-]S([O-])(=O)=O OKJMLYFJRFYBPS-UHFFFAOYSA-J 0.000 claims description 7
- 229910052751 metal Inorganic materials 0.000 claims description 6
- 239000002184 metal Substances 0.000 claims description 6
- 150000002739 metals Chemical class 0.000 claims description 6
- 150000002736 metal compounds Chemical class 0.000 claims description 3
- 230000001590 oxidative effect Effects 0.000 claims description 3
- 230000003197 catalytic effect Effects 0.000 abstract description 13
- 229910052684 Cerium Inorganic materials 0.000 abstract description 11
- GWXLDORMOJMVQZ-UHFFFAOYSA-N cerium Chemical compound [Ce] GWXLDORMOJMVQZ-UHFFFAOYSA-N 0.000 abstract description 11
- 238000006864 oxidative decomposition reaction Methods 0.000 abstract 1
- 238000006243 chemical reaction Methods 0.000 description 40
- 230000000694 effects Effects 0.000 description 8
- 238000004519 manufacturing process Methods 0.000 description 6
- MYMOFIZGZYHOMD-UHFFFAOYSA-N Dioxygen Chemical compound O=O MYMOFIZGZYHOMD-UHFFFAOYSA-N 0.000 description 5
- 229910001882 dioxygen Inorganic materials 0.000 description 5
- XEEYBQQBJWHFJM-UHFFFAOYSA-N Iron Chemical compound [Fe] XEEYBQQBJWHFJM-UHFFFAOYSA-N 0.000 description 4
- 230000008901 benefit Effects 0.000 description 4
- 239000006227 byproduct Substances 0.000 description 4
- 238000007796 conventional method Methods 0.000 description 4
- 239000000376 reactant Substances 0.000 description 4
- KZBUYRJDOAKODT-UHFFFAOYSA-N Chlorine Chemical compound ClCl KZBUYRJDOAKODT-UHFFFAOYSA-N 0.000 description 3
- VYZAMTAEIAYCRO-UHFFFAOYSA-N Chromium Chemical compound [Cr] VYZAMTAEIAYCRO-UHFFFAOYSA-N 0.000 description 3
- MWUXSHHQAYIFBG-UHFFFAOYSA-N Nitric oxide Chemical compound O=[N] MWUXSHHQAYIFBG-UHFFFAOYSA-N 0.000 description 3
- HEMHJVSKTPXQMS-UHFFFAOYSA-M Sodium hydroxide Chemical compound [OH-].[Na+] HEMHJVSKTPXQMS-UHFFFAOYSA-M 0.000 description 3
- 150000001875 compounds Chemical class 0.000 description 3
- 238000010438 heat treatment Methods 0.000 description 3
- 229910001925 ruthenium oxide Inorganic materials 0.000 description 3
- VYPSYNLAJGMNEJ-UHFFFAOYSA-N silicon dioxide Inorganic materials O=[Si]=O VYPSYNLAJGMNEJ-UHFFFAOYSA-N 0.000 description 3
- RYGMFSIKBFXOCR-UHFFFAOYSA-N Copper Chemical compound [Cu] RYGMFSIKBFXOCR-UHFFFAOYSA-N 0.000 description 2
- 238000007138 Deacon process reaction Methods 0.000 description 2
- WCUXLLCKKVVCTQ-UHFFFAOYSA-M Potassium chloride Chemical compound [Cl-].[K+] WCUXLLCKKVVCTQ-UHFFFAOYSA-M 0.000 description 2
- KJTLSVCANCCWHF-UHFFFAOYSA-N Ruthenium Chemical compound [Ru] KJTLSVCANCCWHF-UHFFFAOYSA-N 0.000 description 2
- QAOWNCQODCNURD-UHFFFAOYSA-N Sulfuric acid Chemical compound OS(O)(=O)=O QAOWNCQODCNURD-UHFFFAOYSA-N 0.000 description 2
- 230000015572 biosynthetic process Effects 0.000 description 2
- 238000005660 chlorination reaction Methods 0.000 description 2
- 229910052802 copper Inorganic materials 0.000 description 2
- 239000010949 copper Substances 0.000 description 2
- ORTQZVOHEJQUHG-UHFFFAOYSA-L copper(II) chloride Chemical compound Cl[Cu]Cl ORTQZVOHEJQUHG-UHFFFAOYSA-L 0.000 description 2
- 239000006185 dispersion Substances 0.000 description 2
- 230000007613 environmental effect Effects 0.000 description 2
- 238000010574 gas phase reaction Methods 0.000 description 2
- 239000011521 glass Substances 0.000 description 2
- 239000008187 granular material Substances 0.000 description 2
- 238000005470 impregnation Methods 0.000 description 2
- 229910052742 iron Inorganic materials 0.000 description 2
- 239000012071 phase Substances 0.000 description 2
- 238000002360 preparation method Methods 0.000 description 2
- 230000009467 reduction Effects 0.000 description 2
- 229910052707 ruthenium Inorganic materials 0.000 description 2
- WOCIAKWEIIZHES-UHFFFAOYSA-N ruthenium(iv) oxide Chemical compound O=[Ru]=O WOCIAKWEIIZHES-UHFFFAOYSA-N 0.000 description 2
- 239000000377 silicon dioxide Substances 0.000 description 2
- 238000003786 synthesis reaction Methods 0.000 description 2
- QPLDLSVMHZLSFG-UHFFFAOYSA-N Copper oxide Chemical compound [Cu]=O QPLDLSVMHZLSFG-UHFFFAOYSA-N 0.000 description 1
- 239000005751 Copper oxide Substances 0.000 description 1
- 229910021592 Copper(II) chloride Inorganic materials 0.000 description 1
- VGGSQFUCUMXWEO-UHFFFAOYSA-N Ethene Chemical compound C=C VGGSQFUCUMXWEO-UHFFFAOYSA-N 0.000 description 1
- 239000005977 Ethylene Substances 0.000 description 1
- 239000012327 Ruthenium complex Substances 0.000 description 1
- XUIMIQQOPSSXEZ-UHFFFAOYSA-N Silicon Chemical compound [Si] XUIMIQQOPSSXEZ-UHFFFAOYSA-N 0.000 description 1
- GWEVSGVZZGPLCZ-UHFFFAOYSA-N Titan oxide Chemical compound O=[Ti]=O GWEVSGVZZGPLCZ-UHFFFAOYSA-N 0.000 description 1
- RTAQQCXQSZGOHL-UHFFFAOYSA-N Titanium Chemical compound [Ti] RTAQQCXQSZGOHL-UHFFFAOYSA-N 0.000 description 1
- WGLPBDUCMAPZCE-UHFFFAOYSA-N Trioxochromium Chemical compound O=[Cr](=O)=O WGLPBDUCMAPZCE-UHFFFAOYSA-N 0.000 description 1
- 229910021536 Zeolite Inorganic materials 0.000 description 1
- QCWXUUIWCKQGHC-UHFFFAOYSA-N Zirconium Chemical compound [Zr] QCWXUUIWCKQGHC-UHFFFAOYSA-N 0.000 description 1
- ROZSPJBPUVWBHW-UHFFFAOYSA-N [Ru]=O Chemical class [Ru]=O ROZSPJBPUVWBHW-UHFFFAOYSA-N 0.000 description 1
- 238000010521 absorption reaction Methods 0.000 description 1
- 238000010306 acid treatment Methods 0.000 description 1
- 229910052782 aluminium Inorganic materials 0.000 description 1
- XAGFODPZIPBFFR-UHFFFAOYSA-N aluminium Chemical compound [Al] XAGFODPZIPBFFR-UHFFFAOYSA-N 0.000 description 1
- PNEYBMLMFCGWSK-UHFFFAOYSA-N aluminium oxide Inorganic materials [O-2].[O-2].[O-2].[Al+3].[Al+3] PNEYBMLMFCGWSK-UHFFFAOYSA-N 0.000 description 1
- 239000007864 aqueous solution Substances 0.000 description 1
- 229910052799 carbon Inorganic materials 0.000 description 1
- 239000003518 caustics Substances 0.000 description 1
- 230000008859 change Effects 0.000 description 1
- 229910000423 chromium oxide Inorganic materials 0.000 description 1
- 238000000975 co-precipitation Methods 0.000 description 1
- 229910000431 copper oxide Inorganic materials 0.000 description 1
- 238000013461 design Methods 0.000 description 1
- QDOXWKRWXJOMAK-UHFFFAOYSA-N dichromium trioxide Chemical compound O=[Cr]O[Cr]=O QDOXWKRWXJOMAK-UHFFFAOYSA-N 0.000 description 1
- 230000003292 diminished effect Effects 0.000 description 1
- HNPSIPDUKPIQMN-UHFFFAOYSA-N dioxosilane;oxo(oxoalumanyloxy)alumane Chemical compound O=[Si]=O.O=[Al]O[Al]=O HNPSIPDUKPIQMN-UHFFFAOYSA-N 0.000 description 1
- 238000005868 electrolysis reaction Methods 0.000 description 1
- 238000002474 experimental method Methods 0.000 description 1
- 238000001914 filtration Methods 0.000 description 1
- XLYOFNOQVPJJNP-ZSJDYOACSA-N heavy water Substances [2H]O[2H] XLYOFNOQVPJJNP-ZSJDYOACSA-N 0.000 description 1
- 230000000977 initiatory effect Effects 0.000 description 1
- 208000037805 labour Diseases 0.000 description 1
- 239000007791 liquid phase Substances 0.000 description 1
- 238000011068 loading method Methods 0.000 description 1
- 238000013021 overheating Methods 0.000 description 1
- RVTZCBVAJQQJTK-UHFFFAOYSA-N oxygen(2-);zirconium(4+) Chemical compound [O-2].[O-2].[Zr+4] RVTZCBVAJQQJTK-UHFFFAOYSA-N 0.000 description 1
- 229910052697 platinum Inorganic materials 0.000 description 1
- 239000011148 porous material Substances 0.000 description 1
- 239000001103 potassium chloride Substances 0.000 description 1
- 235000011164 potassium chloride Nutrition 0.000 description 1
- 238000010298 pulverizing process Methods 0.000 description 1
- 239000012495 reaction gas Substances 0.000 description 1
- 230000035484 reaction time Effects 0.000 description 1
- 230000001105 regulatory effect Effects 0.000 description 1
- 150000003304 ruthenium compounds Chemical class 0.000 description 1
- 229910052710 silicon Inorganic materials 0.000 description 1
- 239000010703 silicon Substances 0.000 description 1
- 239000000243 solution Substances 0.000 description 1
- 239000000126 substance Substances 0.000 description 1
- 239000010936 titanium Substances 0.000 description 1
- 229910052719 titanium Inorganic materials 0.000 description 1
- OGIDPMRJRNCKJF-UHFFFAOYSA-N titanium oxide Inorganic materials [Ti]=O OGIDPMRJRNCKJF-UHFFFAOYSA-N 0.000 description 1
- 239000010457 zeolite Substances 0.000 description 1
- 229910052726 zirconium Inorganic materials 0.000 description 1
- 229910001928 zirconium oxide Inorganic materials 0.000 description 1
Classifications
-
- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
- C01B7/00—Halogens; Halogen acids
- C01B7/01—Chlorine; Hydrogen chloride
- C01B7/03—Preparation from chlorides
- C01B7/04—Preparation of chlorine from hydrogen chloride
-
- B—PERFORMING OPERATIONS; TRANSPORTING
- B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
- B01J—CHEMICAL OR PHYSICAL PROCESSES, e.g. CATALYSIS OR COLLOID CHEMISTRY; THEIR RELEVANT APPARATUS
- B01J23/00—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00
- B01J23/10—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of rare earths
-
- B—PERFORMING OPERATIONS; TRANSPORTING
- B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
- B01J—CHEMICAL OR PHYSICAL PROCESSES, e.g. CATALYSIS OR COLLOID CHEMISTRY; THEIR RELEVANT APPARATUS
- B01J35/00—Catalysts, in general, characterised by their form or physical properties
- B01J35/40—Catalysts, in general, characterised by their form or physical properties characterised by dimensions, e.g. grain size
-
- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
- C01P2004/00—Particle morphology
- C01P2004/60—Particles characterised by their size
- C01P2004/61—Micrometer sized, i.e. from 1-100 micrometer
-
- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
- C01P2004/00—Particle morphology
- C01P2004/60—Particles characterised by their size
- C01P2004/64—Nanometer sized, i.e. from 1-100 nanometer
Definitions
- the present invention relates to a method for preparing chlorine, in which hydrogen chloride is decomposed to produce chlorine, precisely hydrogen chloride is reacted with oxygen containing gas in the presence of a cerium catalyst to produce chlorine .
- Chlorine is widely used in the production of various compounds and is in increasing demand.
- hydrochloric acid (liquid phase) or hydrogen chloride (gas phase) the byproducts generated during chlorination, cannot find its usability, and thus is discarded, which requires high costs and labors. And the amount of such byproduct is gradually increasing.
- most of hydrochloric acid and hydrogen chloride are prepared in the phase of aqueous solution (20% or 35% hydrochloric acid) for sale or are discarded after being neutralized.
- the above treatment method not only causes economical damage but also causes environmental problems. Therefore, a method for converting hydrochloric acid generated massively as a byproduct in chlorination industry into chlorine can be an efficient and positive way to reduce hydrochloric acid treatment costs and to cope with environmental problems because the conversion of hydrochloric acid into chlorine does not break the balance between supply and demand of sodium hydroxide generated during electrolysis and only increases the production of chlorine.
- Deacon Process is a kind of contact oxidation using CuCl 2 as a catalyst, which requires high reaction temperature of 450 ⁇ 500 ° C. So, at this high temperature, a catalyst is easily decomposed and it is difficult to design a device specifically to treat corrosive substances at that high temperature. Thus, this process could not be commercialized. But, based on this process, different catalytic oxidation methods have been tried as follows.
- MT-Chlor process is a method for preparing chlorine using chrome-silica fluid-bed catalyst.
- Kel-Chlor process is a method for preparing chlorine by non-contact oxidation developed by Kellog, in which nitrogen oxide is used as a catalyst and sulfuric acid is used as a circulatory catalyst.
- Shell-Chlor process is a modified contact oxidation method using a copper oxide catalyst which has been improved from the original contact oxidation method developed by Deacon in 1868 and established by Shell in 1960 which enables lower temperature reaction (350 ⁇ 400°C) .
- a chrome based catalyst using chrome oxide has been proposed as an alternative for the said copper or iron based catalyst (British Patent No. 676667) . Even if this catalyst provides high hydrogen chloride conversion rate (60-75%) , the chrome based catalyst is also reacted at high temperature of at least 400 ° C. So, short life time of the catalyst is still a problem with this chrome based catalyst.
- Dichrome trioxide catalyst generally represented as MT- Chlor catalyst has been proposed (Japanese Patent Publication Nos. 62-153103, 62-191403, 62-241805, and 62-275001, Korean Patent No. 10-0032752) . And also cerium chloride containing dichrome trioxide catalyst was proposed (Korean Patent Publication No. 1999-0000001) . But the activity and short life time of the catalyst was still a problem. In addition, the process of producing this catalyst was very complicated.
- the present invention provides a method for preparing chlorine from hydrogen chloride, in which cerium oxide having excellent stability and durability and far less expensive than the said platinum based catalyst is used as a catalyst for oxidation.
- the method of the present invention is characterized by using a cerium compound as a catalyst for the production of chlorine by oxidizing hydrogen chloride with oxygen containing gas .
- the cerium compound herein is preferably cerium oxide, cerium complex oxide or a mixture thereof, and the cerium compound is preferably selected from the group consisting of cerium acetate, cerium ammonium nitrate, cerium ammonium sulfate, cerium carbide, cerium carbonate, cerium chloride, cerium nitrate, cerium perchlorate, cerium sulfide and a mixture thereof .
- the cerium compound is preferably an oxide of a compound selected from the group consisting of cerium acetate, cerium ammonium nitrate, cerium ammonium sulfate, cerium carbide, cerium carbonate, cerium chloride, cerium nitrate, cerium perchlorate, cerium sulfide and a mixture thereof.
- the cerium compound is more preferably cerium oxide.
- the catalyst above is preferably prepared by loading the cerium compound in a support or by oxidation of the cerium compound loaded in a support .
- the content of the cerium compound in the support is preferably 1-10 weight%.
- the cerium compound is preferably in the shape of particle of 100 ran - 100 ⁇ m in size.
- the cerium compound is used as a main catalyst and one or more metals selected from platinum group elements or one or more metal compounds of metals selected from platinum group elements as a cocatalyst.
- the preferable content of the cocatalyst in the catalyst is 1-50 weight%.
- the method of the present invention is characterized by preparing chlorine at 250-400°C in the presence of the cerium based catalyst (a catalyst using the said cerium compound) .
- the cerium based catalyst used for the preparation of chlorine in this invention has lower reaction temperature of up to 400 ° C, has high activity, and has high stability, so that it maintains catalytic activity for a long time of reaction and thus has a merit for economy.
- Figure 1 is a graph illustrating the result of X-ray fraction with the cerium oxide before and after the reaction of Example 8.
- the key technique of the method of the present invention is to produce chlorine by oxidizing hydrogen chloride with oxygen containing gas in the presence of a cerium compound.
- the method of the present invention is to commercialize the process of chlorine production based on gas phase reaction of hydrogen chloride in a catalytic reactor.
- the present invention relates to a catalyst that is capable of preventing the reduction of catalytic activity by exothermic reaction and thus is economical.
- the reaction between hydrogen chloride and oxygen in a catalytic reactor is represented by the following reaction formula 1.
- reaction formula 1 theoretical ratio of hydrogen chloride to oxygen(0 2 ) is 4:1 and the reaction is exothermic reaction. So, it is economically advantageous and more effective in preventing damage of a catalyst to generate chlorine at a temperature as low as possible as long as the catalyst maintains its catalytic activity.
- the cerium compound herein is preferably cerium oxide, cerium complex oxide or a mixture thereof , and the cerium compound is preferably selected from the group consisting of cerium acetate, cerium ammonium nitrate, cerium ammonium sulfate, cerium carbide, cerium carbonate, cerium chloride, cerium nitrate, cerium perchlorate, cerium sulfide and a mixture thereof .
- the cerium compound is preferably an oxide of a compound selected from the group consisting of cerium acetate, cerium ammonium nitrate, cerium ammonium sulfate, cerium carbide, cerium carbonate, cerium chloride, cerium nitrate, cerium perchlorate, cerium sulfide and a mixture thereof.
- the cerium compound is more preferably cerium oxide.
- the cerium compound of the present invention can be prepared by the conventional method. Or a commercial cerium compound can be used.
- the method for preparing cerium complex oxide is exemplified by coprecipitation method, dispersion method (dispersion and heat treatment) and impregnation method.
- the cerium compound is prepared as particles having the size of 100 nm - 100 jM or as granules composed of the particles.
- This particle type or granule type cerium compound can be filled in a reactor or can be loaded in a support .
- the catalyst is loaded in a support.
- the cerium compound of the present invention is not cerium oxide, the cerium compound is loaded in a support first and then oxidized.
- cerium acetate, cerium ammonium nitrate, cerium ammonium sulfate, cerium carbide, cerium carbonate, cerium chloride, cerium nitrate, cerium perchlorate, cerium sulfide or a mixture thereof is loaded in a support and oxidized in the presence of oxygen at 450-1300 ° C to produce a cerium oxide catalyst.
- the support herein is any support used for the commercial reaction of chlorine preparation from hydrogen chloride by gas phase reaction, which is preferably exemplified by titanium oxide, alumina, silica, zirconium oxide, zeolite, titanium complex oxide, zirconium complex oxide, aluminum complex oxide and silicon complex oxide.
- the support herein preferably has micro-pores. To load a cerium compound into a support, impregnation method or equilibrium absorption method can be used.
- the content of the cerium compound loaded in a support is preferably 1 - 10 weight% by the support.
- the above range of the content is preferable condition for a catalyst to maintain the catalytic activity with minimizing the reduction of specific surface area of the support.
- the cerium compound is preferably in the shape of particle of 100 nm - 100 ⁇ m in size. This sized particle is advantageous for maintaining stability at high temperature, for preventing over-heating by exothermic reaction to produce chlorine and for obtaining high conversion rate (high chlorine yield) by maximizing surface area of the catalyst.
- the cerium compound of 100 nm - 100 ⁇ m in size can be loaded in a support or fills a reaction tube as a catalyst.
- the size of the cerium compound particle can be regulated by pulverizing a commercial cerium compound and filtering thereof, or by optimizing heat -treatment temperature and heat- treatment time after synthesis, or by optimizing synthesis condition itself .
- the cerium compound is used as a main catalyst and one or more metals selected from platinum group elements or one or more metal compounds of metals selected from platinum group elements as a cocatalyst.
- the cocatalyst herein is added in order to increase the activity of the cerium compound and preferable content of such cocatalyst is 1-50 weight% by the total weight of the catalyst.
- the method of the present invention is characterized by lower temperature reaction of at 250-400 ° C, more preferably at 300-350 ° C, in the presence of the cerium based catalyst (cerium compound catalyst as mentioned above) to produce chlorine.
- a glass reactor having 1" of inside diameter was used. Hydrogen chloride gas and oxygen gas, the reactants, were added to the reactor at the ratio of 1:1. Flow rates of the reactants were 25 ml/min respectively.
- the reactor was filled with cerium oxide (Hanwha Chemical Co., Cat. #: CED30S) of 10 ⁇ m in mean diameter at the density of 0.4 g/cm 3 .
- the reactor was 20 cm long and the temperature of the reactor was maintained as 350°C .
- Conversion Rate (%) (amount of chlorine gas generated*2) / (amount of hydrogen chloride before the reaction) *100
- a glass reactor (inside diameter: 1", length: 100 cm) was filled with the cerium compound of Example 1 at the density of 0.4g/cm 3 .
- Hydrogen chloride gas and oxygen gas, the reactants, were provided to the reactor at the molar ratio of 1:2.
- Flow rate of the hydrogen chloride gas: oxygen gas was 25:50 ml/min.
- temperature of the reactor was maintained at 350 ° C.
- Example 5 Experiments were performed by the same manner as described in Example 5 except that the flow rate of hydrogen chloride gas: oxygen gas was adjusted to 17:34 ml/min and temperature of the reactor was maintained at 300 ° C (Example 6) and the flow rate of hydrogen chloride gas: oxygen gas was adjusted to 17:34 ml/min and temperature of the reactor was maintained at 350 ° C (Example 7) . From 2 hours after the reaction was started, in Examples 5 - 7, generated gas was captured and analyzed by Orsat method and the results are shown in Table 2.
- Reaction was induced by the same manner as described in Example 5 except that the temperature of the reactor was maintained at 400 ° C.
- the catalytic activity was examined by analyzing reaction gas (conversion rate for the first 2 hours: 53.5%, conversion rate for 100 hours: 52.7%) .
- Non-used catalyst and used catalyst after 100 hours of the reaction were investigated by X-ray fraction and the results are shown in Figure 1. As shown in Figure 1 , there was no change in the structure of the catalyst used for 100 hours of the reaction at the high temperature of 400 ° C.
- Examples 1 - 8 pure cerium compound alone was used as a catalyst.
- the method for preparing chlorine using the cerium based catalyst of the present invention was confirmed to have economical advantages because it gives high conversion rate of at least 60% at up to 400 ° C ; maintains catalytic activity at even high temperature of 400°C, maintains stable structure, activity and stability at high-temperature without platinum group elements.
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- Chemical & Material Sciences (AREA)
- Organic Chemistry (AREA)
- Inorganic Chemistry (AREA)
- Engineering & Computer Science (AREA)
- Materials Engineering (AREA)
- Chemical Kinetics & Catalysis (AREA)
- Catalysts (AREA)
Abstract
The present invention relates to a method for preparing chlorine by decomposing hydrogen chloride, in which hydrogen chloride is reacted with oxygen containing gas in the presence of a cerium based catalyst at comparatively low temperature of up to 400°C to produce chlorine. The cerium based catalyst of the present invention maintains its catalytic activity for a long time, compared with other catalysts prepared by the conventional processes, has excellent stability at high temperature, and has high economical efficiency, so that it paves the way to the development of an economically excellent oxidative decomposition process to produce chlorine from hydrogen chloride.
Description
[DESCRIPTION!
[invention Title]
PROCESS FOR THE CHLORINE BY OXIDATION OF HYDROGEN CHLORIDE
[Technical Field]
The present invention relates to a method for preparing chlorine, in which hydrogen chloride is decomposed to produce chlorine, precisely hydrogen chloride is reacted with oxygen containing gas in the presence of a cerium catalyst to produce chlorine .
[Background Art]
Chlorine is widely used in the production of various compounds and is in increasing demand. However, hydrochloric acid (liquid phase) or hydrogen chloride (gas phase) , the byproducts generated during chlorination, cannot find its usability, and thus is discarded, which requires high costs and labors. And the amount of such byproduct is gradually increasing. In Korea, except the case of preparing VCM by reacting hydrogen chloride with ethylene in an oxychlorination reactor, most of hydrochloric acid and hydrogen chloride are prepared in the phase of aqueous solution (20% or 35% hydrochloric acid) for sale or are discarded after being
neutralized.
The above treatment method not only causes economical damage but also causes environmental problems. Therefore, a method for converting hydrochloric acid generated massively as a byproduct in chlorination industry into chlorine can be an efficient and positive way to reduce hydrochloric acid treatment costs and to cope with environmental problems because the conversion of hydrochloric acid into chlorine does not break the balance between supply and demand of sodium hydroxide generated during electrolysis and only increases the production of chlorine.
It has long been tried to recover chlorine from hydrogen chloride produced as a byproduct to solve the unbalance between the production of chlorine and the generation of hydrogen chloride. Deacon introduced a method to produce chlorine from hydrogen chloride by catalytic oxidation. Since then, methods modified from the catalytic oxidation have been tried and some of them made progress to be practical . The key point of the method producing chlorine from hydrogen chloride by oxidation is the selection of a catalyst and the success of this method depends on the efficiency of a selected catalyst.
The first method to produce chlorine from hydrogen
chloride by oxidation, "Deacon Process" was named after the inventor. Deacon process is a kind of contact oxidation using CuCl2 as a catalyst, which requires high reaction temperature of 450~500°C. So, at this high temperature, a catalyst is easily decomposed and it is difficult to design a device specifically to treat corrosive substances at that high temperature. Thus, this process could not be commercialized. But, based on this process, different catalytic oxidation methods have been tried as follows. MT-Chlor process is a method for preparing chlorine using chrome-silica fluid-bed catalyst. Kel-Chlor process is a method for preparing chlorine by non-contact oxidation developed by Kellog, in which nitrogen oxide is used as a catalyst and sulfuric acid is used as a circulatory catalyst. Shell-Chlor process is a modified contact oxidation method using a copper oxide catalyst which has been improved from the original contact oxidation method developed by Deacon in 1868 and established by Shell in 1960 which enables lower temperature reaction (350~400°C) .
To improve the copper based catalyst, so called Deacon catalyst, various catalysts and different processes have been reported (US Patent No. 2418930, US Patent No. 2418931, US Patent No. 4119705, Japanese Patent Publication No. 53-125989, etc) . However, reaction temperatures for the processes are all at least 400 "C .
An iron based catalyst was once proposed (US Patent No. 2577808) , which has also a problem of temperature limitation to at least 400°C making the catalyst life short.
A chrome based catalyst using chrome oxide has been proposed as an alternative for the said copper or iron based catalyst (British Patent No. 676667) . Even if this catalyst provides high hydrogen chloride conversion rate (60-75%) , the chrome based catalyst is also reacted at high temperature of at least 400°C. So, short life time of the catalyst is still a problem with this chrome based catalyst.
Dichrome trioxide catalyst generally represented as MT- Chlor catalyst has been proposed (Japanese Patent Publication Nos. 62-153103, 62-191403, 62-241805, and 62-275001, Korean Patent No. 10-0032752) . And also cerium chloride containing dichrome trioxide catalyst was proposed (Korean Patent Publication No. 1999-0000001) . But the activity and short life time of the catalyst was still a problem. In addition, the process of producing this catalyst was very complicated.
There is another method for preparing chlorine by hydrogen chloride oxidation, which has been developed by Sumitomo Co. and commercialized (Japanese Patent Publication Nos. 95-119866 and 95-157959, Korean Patent No. 10-0424502) . This method is characterized by lower reaction temperature using smaller amount of highly active ruthenium oxide catalyst
for producing chlorine. The key technique of this method is to use ruthenium compounds (ruthenium oxides or ruthenium complex oxides) as a catalyst for oxidation. Precisely, by taking advantage of high activity of ruthenium, oxidation is induced at lower temperature of 300 "C with smaller amount of the catalyst.
In the meantime, Mitsui Toatus Chemical Inc reported the reaction process and reactor comprising two different reaction areas and heat exchange system using copper chloride, potassium chloride, chromium oxide or ruthenium oxide as a catalyst with suggesting the possibility of commercialization (US Patent Publication Nos . 94-278804, 95-226090 and 95- 228749, Korean Patent Publication No. 1996-0016957, PCT No. 88-00171, Korean Patent Publication No. 1988-0701212) . However, to lower reaction temperature and to commercialize, highly expensive ruthenium, the platinum group element, has to be used. Moreover the stability at high temperature is still in doubt and the increase of chlorine production cost resulted from the expensive catalyst make commercialization difficult.
Most of catalysts used in the conventional methods demonstrated high activity at high reaction temperature. But, the efficiency of the catalyst is diminished within several months when high temperature operation continues . To overcome
the said problems of the conventional methods, the present invention provides a method for preparing chlorine from hydrogen chloride, in which cerium oxide having excellent stability and durability and far less expensive than the said platinum based catalyst is used as a catalyst for oxidation.
[Disclosure]
[Technical Problem]
It is an object of the present invention, to overcome the problems of the conventional methods, to provide a method for preparing chlorine using a novel catalyst which requires lower reaction temperature, has high activity and stability enough to maintain catalytic activity for a long reaction time, and has benefits for economy.
[Technical Solution]
The method of the present invention is characterized by using a cerium compound as a catalyst for the production of chlorine by oxidizing hydrogen chloride with oxygen containing gas .
The cerium compound herein is preferably cerium oxide, cerium complex oxide or a mixture thereof, and the cerium compound is preferably selected from the group consisting of cerium acetate, cerium ammonium nitrate, cerium ammonium
sulfate, cerium carbide, cerium carbonate, cerium chloride, cerium nitrate, cerium perchlorate, cerium sulfide and a mixture thereof .
The cerium compound is preferably an oxide of a compound selected from the group consisting of cerium acetate, cerium ammonium nitrate, cerium ammonium sulfate, cerium carbide, cerium carbonate, cerium chloride, cerium nitrate, cerium perchlorate, cerium sulfide and a mixture thereof.
The cerium compound is more preferably cerium oxide. The catalyst above is preferably prepared by loading the cerium compound in a support or by oxidation of the cerium compound loaded in a support .
The content of the cerium compound in the support is preferably 1-10 weight%. The cerium compound is preferably in the shape of particle of 100 ran - 100 μm in size.
In this invention, the cerium compound is used as a main catalyst and one or more metals selected from platinum group elements or one or more metal compounds of metals selected from platinum group elements as a cocatalyst. The preferable content of the cocatalyst in the catalyst is 1-50 weight%.
The method of the present invention is characterized by preparing chlorine at 250-400°C in the presence of the cerium based catalyst (a catalyst using the said cerium compound) .
[Advantageous Effect]
The cerium based catalyst used for the preparation of chlorine in this invention has lower reaction temperature of up to 400°C, has high activity, and has high stability, so that it maintains catalytic activity for a long time of reaction and thus has a merit for economy.
[Description of Drawings]
The above and other objects, features and advantages of the present invention will become apparent from the following description of preferred embodiments given in conjunction with the accompanying drawings, in which:
Figure 1 is a graph illustrating the result of X-ray fraction with the cerium oxide before and after the reaction of Example 8.
[Best Mode]
The key technique of the method of the present invention is to produce chlorine by oxidizing hydrogen chloride with oxygen containing gas in the presence of a cerium compound.
The method of the present invention is described in more detail hereinafter. Technical and scientific terms used herein indicate general meanings understood by those in the art, if
stated otherwise. Hereinafter, well-known functions and compositions that might lure to wrong direction are rather not described.
The method of the present invention is to commercialize the process of chlorine production based on gas phase reaction of hydrogen chloride in a catalytic reactor. Particularly, the present invention relates to a catalyst that is capable of preventing the reduction of catalytic activity by exothermic reaction and thus is economical. The reaction between hydrogen chloride and oxygen in a catalytic reactor is represented by the following reaction formula 1.
4HCl + O2 <→ 2Cl2 +2H2O (1)
As shown in reaction formula 1, theoretical ratio of hydrogen chloride to oxygen(02) is 4:1 and the reaction is exothermic reaction. So, it is economically advantageous and more effective in preventing damage of a catalyst to generate chlorine at a temperature as low as possible as long as the catalyst maintains its catalytic activity.
The cerium compound herein is preferably cerium oxide, cerium complex oxide or a mixture thereof , and the cerium
compound is preferably selected from the group consisting of cerium acetate, cerium ammonium nitrate, cerium ammonium sulfate, cerium carbide, cerium carbonate, cerium chloride, cerium nitrate, cerium perchlorate, cerium sulfide and a mixture thereof .
The cerium compound is preferably an oxide of a compound selected from the group consisting of cerium acetate, cerium ammonium nitrate, cerium ammonium sulfate, cerium carbide, cerium carbonate, cerium chloride, cerium nitrate, cerium perchlorate, cerium sulfide and a mixture thereof.
The cerium compound is more preferably cerium oxide.
The cerium compound of the present invention can be prepared by the conventional method. Or a commercial cerium compound can be used. The method for preparing cerium complex oxide is exemplified by coprecipitation method, dispersion method (dispersion and heat treatment) and impregnation method.
To be used as a catalyst, the cerium compound is prepared as particles having the size of 100 nm - 100 jM or as granules composed of the particles. This particle type or granule type cerium compound can be filled in a reactor or can be loaded in a support .
If the cerium compound of the present invention is cerium oxide or cerium complex oxide, the catalyst is loaded in a
support. Or, if the cerium compound of the present invention is not cerium oxide, the cerium compound is loaded in a support first and then oxidized. Preferably, cerium acetate, cerium ammonium nitrate, cerium ammonium sulfate, cerium carbide, cerium carbonate, cerium chloride, cerium nitrate, cerium perchlorate, cerium sulfide or a mixture thereof is loaded in a support and oxidized in the presence of oxygen at 450-1300°C to produce a cerium oxide catalyst.
The support herein is any support used for the commercial reaction of chlorine preparation from hydrogen chloride by gas phase reaction, which is preferably exemplified by titanium oxide, alumina, silica, zirconium oxide, zeolite, titanium complex oxide, zirconium complex oxide, aluminum complex oxide and silicon complex oxide. The support herein preferably has micro-pores. To load a cerium compound into a support, impregnation method or equilibrium absorption method can be used.
The content of the cerium compound loaded in a support is preferably 1 - 10 weight% by the support. The above range of the content is preferable condition for a catalyst to maintain the catalytic activity with minimizing the reduction of specific surface area of the support.
The cerium compound is preferably in the shape of
particle of 100 nm - 100 μm in size. This sized particle is advantageous for maintaining stability at high temperature, for preventing over-heating by exothermic reaction to produce chlorine and for obtaining high conversion rate (high chlorine yield) by maximizing surface area of the catalyst. The cerium compound of 100 nm - 100 μm in size can be loaded in a support or fills a reaction tube as a catalyst.
The size of the cerium compound particle can be regulated by pulverizing a commercial cerium compound and filtering thereof, or by optimizing heat -treatment temperature and heat- treatment time after synthesis, or by optimizing synthesis condition itself .
In this invention, the cerium compound is used as a main catalyst and one or more metals selected from platinum group elements or one or more metal compounds of metals selected from platinum group elements as a cocatalyst. The cocatalyst herein is added in order to increase the activity of the cerium compound and preferable content of such cocatalyst is 1-50 weight% by the total weight of the catalyst.
The method of the present invention is characterized by lower temperature reaction of at 250-400 °C, more preferably at 300-350°C, in the presence of the cerium based catalyst (cerium
compound catalyst as mentioned above) to produce chlorine.
(Example 1)
A glass reactor having 1" of inside diameter was used. Hydrogen chloride gas and oxygen gas, the reactants, were added to the reactor at the ratio of 1:1. Flow rates of the reactants were 25 ml/min respectively. The reactor was filled with cerium oxide (Hanwha Chemical Co., Cat. #: CED30S) of 10 μm in mean diameter at the density of 0.4 g/cm3. The reactor was 20 cm long and the temperature of the reactor was maintained as 350°C . After 2 hours from the initiation of the reaction after supplying necessary gases (reactants) to the reactor, generated gas was captured and analyzed by Orsat method. Reactions were induced by the same manner as described in Example 1 except that different reactors and reaction temperatures were used (30 cm / 300°C: Example 2, 50 cm / 350°C: Example 3, 100 cm / 350°C: Example 4) .
Results of the reactions in Examples 1 - 4 are shown in Table 1.
Conversion rate was calculated by the comparison of the amount of chlorine gas generated from the reaction and the amount of non-reacted hydrogen chloride gas, according to the following formula:
Conversion Rate (%) = (amount of chlorine gas generated*2) / (amount of hydrogen chloride before the reaction) *100
(Table 1)
(Example 5)
A glass reactor (inside diameter: 1", length: 100 cm) was filled with the cerium compound of Example 1 at the density of 0.4g/cm3. Hydrogen chloride gas and oxygen gas, the reactants, were provided to the reactor at the molar ratio of 1:2. Flow rate of the hydrogen chloride gas: oxygen gas was 25:50 ml/min. At that time, temperature of the reactor was maintained at 350°C.
Experiments were performed by the same manner as described in Example 5 except that the flow rate of hydrogen chloride gas: oxygen gas was adjusted to 17:34 ml/min and temperature of the reactor was maintained at 300°C (Example 6) and the flow rate of hydrogen chloride gas: oxygen gas was adjusted to 17:34 ml/min and temperature of the reactor was maintained at 350 °C (Example 7) .
From 2 hours after the reaction was started, in Examples 5 - 7, generated gas was captured and analyzed by Orsat method and the results are shown in Table 2.
(Table 2)
(Example 8)
Reaction was induced by the same manner as described in Example 5 except that the temperature of the reactor was maintained at 400°C. The catalytic activity was examined by analyzing reaction gas (conversion rate for the first 2 hours: 53.5%, conversion rate for 100 hours: 52.7%) . Non-used catalyst and used catalyst after 100 hours of the reaction were investigated by X-ray fraction and the results are shown in Figure 1. As shown in Figure 1 , there was no change in the structure of the catalyst used for 100 hours of the reaction at the high temperature of 400°C.
In Examples 1 - 8 , pure cerium compound alone was used as a catalyst. As a result, the method for preparing chlorine using the cerium based catalyst of the present invention was confirmed to have economical advantages because it gives high
conversion rate of at least 60% at up to 400°C; maintains catalytic activity at even high temperature of 400°C, maintains stable structure, activity and stability at high-temperature without platinum group elements.
Those skilled in the art will appreciate that the conceptions and specific embodiments disclosed in the foregoing description may be readily utilized as a basis for modifying or designing other embodiments for carrying out the same purposes of the present invention. Those skilled in the art will also appreciate that such equivalent embodiments do not depart from the spirit and scope of the invention as set forth in the appended claims.
Claims
[CLAIMS]
[Claim l]
A method for preparing chlorine by oxidizing hydrogen chloride with oxygen containing gas, in which a cerium compound is used as a catalyst.
[Claim 2]
The method for preparing chlorine according to claim 1, wherein the cerium compound is cerium oxide.
[Claim 3]
The method for preparing chlorine according to claim 1, wherein the cerium compound is cerium acetate, cerium ammonium nitrate, cerium ammonium sulfate, cerium carbide, cerium carbonate, cerium chloride, cerium nitrate, cerium perchlorate, cerium sulfide or a mixture thereof.
[Claim 4]
The method for preparing chlorine according to claim 2, wherein the cerium compound is an oxide of cerium acetate, cerium ammonium nitrate, cerium ammonium sulfate, cerium carbide, cerium carbonate, cerium chloride, cerium nitrate, cerium perchlorate, cerium sulfide or a mixture thereof.
[Claim 5]
The method for preparing chlorine according to claim 1, wherein the catalyst is prepared as loaded in a support.
[Claim 6]
The method for preparing chlorine according to claim 4, wherein the catalyst is loaded in a support and oxidized therein.
[Claim 7]
The method for preparing chlorine according to claim 5, wherein the content of cerium compound in a support is 1 - 10weight%.
[Claim 8]
The method for preparing chlorine according to claim 1, wherein the cerium compound is in the shape of particle of 100 nm - 100 μm in size.
[Claim 9]
The method for preparing chlorine according to claim 1, wherein the catalyst contains a cerium compound as a main catalyst and additionally includes one or more metals selected from platinum group elements or one or more metal compounds of metals selected from platinum group elements as a cocatalyst.
[Claim 10]
The method for preparing chlorine according to claim 9, wherein the content of the cocatalyst is 1 - 50 weight% by the total weight of the catalyst.
[Claim 11]
The method for preparing chlorine according to any of claim 1 - claim 10, wherein the chlorine is prepared at 250 - 400°C.
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KR1020070091300A KR20090026381A (en) | 2007-09-10 | 2007-09-10 | Process for the chlorine by oxidation of hydrogen chloride |
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Cited By (6)
Publication number | Priority date | Publication date | Assignee | Title |
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WO2010133313A1 (en) * | 2009-05-16 | 2010-11-25 | Bayer Materialscience Ag | Process for preparing chlorine by gas phase oxidation of hydrogen chloride in the presence of a cerium oxide catalyst |
WO2013004649A1 (en) | 2011-07-05 | 2013-01-10 | Bayer Intellectual Property Gmbh | Process for the production of chlorine using a cerium oxide catalyst in an adiabatic reaction cascade |
WO2013004651A1 (en) | 2011-07-05 | 2013-01-10 | Bayer Intellectual Property Gmbh | Process for the production of chlorine using a cerium oxide catalyst in an isothermic reactor |
WO2013060628A1 (en) | 2011-10-24 | 2013-05-02 | Bayer Intellectual Property Gmbh | Catalyst and method for producing chlorine by means of a gas-phase oxidation |
EP3421416A1 (en) | 2017-06-29 | 2019-01-02 | Covestro Deutschland AG | Photocatalytic oxidation of hydrogen chloride with carbon monoxide |
EP3670444A1 (en) | 2018-12-18 | 2020-06-24 | Covestro Deutschland AG | Photocatalytic oxidation of hydrogen chloride with oxygen |
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KR950016873A (en) * | 1993-12-01 | 1995-07-20 | 김은영 | Cerium chloride-dichromium trioxide catalyst for the production of chlorine by oxidation of hydrogen chloride and preparation method thereof |
KR970015456A (en) * | 1995-09-12 | 1997-04-28 | 랑핑거, 스타인호프 | Preparation of chlorine from hydrogen chloride |
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KR970015456A (en) * | 1995-09-12 | 1997-04-28 | 랑핑거, 스타인호프 | Preparation of chlorine from hydrogen chloride |
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WO2010133313A1 (en) * | 2009-05-16 | 2010-11-25 | Bayer Materialscience Ag | Process for preparing chlorine by gas phase oxidation of hydrogen chloride in the presence of a cerium oxide catalyst |
JP2014520742A (en) * | 2011-07-05 | 2014-08-25 | バイエル インテレクチュアル プロパティー ゲゼルシャフト ミット ベシュレンクテル ハフツング | Method for producing chlorine using cerium oxide catalyst in adiabatic reaction cascade |
WO2013004649A1 (en) | 2011-07-05 | 2013-01-10 | Bayer Intellectual Property Gmbh | Process for the production of chlorine using a cerium oxide catalyst in an adiabatic reaction cascade |
WO2013004651A1 (en) | 2011-07-05 | 2013-01-10 | Bayer Intellectual Property Gmbh | Process for the production of chlorine using a cerium oxide catalyst in an isothermic reactor |
CN103764548A (en) * | 2011-07-05 | 2014-04-30 | 拜耳知识产权有限责任公司 | Process for the production of chlorine using a cerium oxide catalyst in an isothermic reactor |
WO2013060628A1 (en) | 2011-10-24 | 2013-05-02 | Bayer Intellectual Property Gmbh | Catalyst and method for producing chlorine by means of a gas-phase oxidation |
CN103889568A (en) * | 2011-10-24 | 2014-06-25 | 拜耳知识产权有限责任公司 | Catalyst and method for producing chlorine by means of a gas-phase oxidation |
JP2014534062A (en) * | 2011-10-24 | 2014-12-18 | バイエル・インテレクチュアル・プロパティ・ゲゼルシャフト・ミット・ベシュレンクテル・ハフツングBayer Intellectual Property GmbH | Catalyst and method for producing chlorine by gas phase oxidation |
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JP2018089625A (en) * | 2011-10-24 | 2018-06-14 | バイエル・インテレクチュアル・プロパティ・ゲゼルシャフト・ミット・ベシュレンクテル・ハフツングBayer Intellectual Property GmbH | Catalyst and method for producing chlorine by vapor phase oxidation |
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WO2020127022A1 (en) | 2018-12-18 | 2020-06-25 | Covestro Intellectual Property Gmbh & Co. Kg | Photocatalytic oxidation of hydrochloric acid using oxygen |
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WO2009035234A3 (en) | 2009-05-07 |
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