WO2010133313A1 - Procédé de fabrication de chlore par oxydation en phase gazeuse de chlorure d'hydrogène en présence d'un catalyseur oxyde de cérium - Google Patents

Procédé de fabrication de chlore par oxydation en phase gazeuse de chlorure d'hydrogène en présence d'un catalyseur oxyde de cérium Download PDF

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Publication number
WO2010133313A1
WO2010133313A1 PCT/EP2010/002962 EP2010002962W WO2010133313A1 WO 2010133313 A1 WO2010133313 A1 WO 2010133313A1 EP 2010002962 W EP2010002962 W EP 2010002962W WO 2010133313 A1 WO2010133313 A1 WO 2010133313A1
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hydrogen chloride
active component
catalyst
cerium oxide
oxygen
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PCT/EP2010/002962
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German (de)
English (en)
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Aurel Wolf
Leslaw Mleczko
Stephan Schubert
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Bayer Materialscience Ag
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Publication of WO2010133313A1 publication Critical patent/WO2010133313A1/fr

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    • 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
    • B01J23/00—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00
    • B01J23/002—Mixed oxides other than spinels, e.g. perovskite
    • 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
    • B01J23/14—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of germanium, tin or lead
    • 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
    • B01J27/00—Catalysts comprising the elements or compounds of halogens, sulfur, selenium, tellurium, phosphorus or nitrogen; Catalysts comprising carbon compounds
    • B01J27/06—Halogens; Compounds thereof
    • B01J27/08—Halides
    • B01J27/10—Chlorides
    • 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
    • B01J37/00—Processes, in general, for preparing catalysts; Processes, in general, for activation of catalysts
    • B01J37/08—Heat treatment
    • 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
    • B01J23/12—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of actinides
    • 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
    • B01J23/16—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of arsenic, antimony, bismuth, vanadium, niobium, tantalum, polonium, chromium, molybdenum, tungsten, manganese, technetium or rhenium
    • B01J23/18—Arsenic, antimony or bismuth
    • 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
    • B01J23/16—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of arsenic, antimony, bismuth, vanadium, niobium, tantalum, polonium, chromium, molybdenum, tungsten, manganese, technetium or rhenium
    • B01J23/24—Chromium, molybdenum or tungsten
    • B01J23/26—Chromium
    • 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
    • B01J23/16—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of arsenic, antimony, bismuth, vanadium, niobium, tantalum, polonium, chromium, molybdenum, tungsten, manganese, technetium or rhenium
    • B01J23/32—Manganese, technetium or rhenium
    • 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
    • B01J23/38—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of noble metals
    • B01J23/40—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of noble metals of the platinum group metals
    • 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
    • B01J23/38—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of noble metals
    • B01J23/48—Silver or gold
    • 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
    • B01J23/70—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of the iron group metals or copper
    • 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
    • B01J2523/00—Constitutive chemical elements of heterogeneous catalysts

Definitions

  • the present invention relates to a process for the production of chlorine by catalytic oxidation of hydrogen chloride in the presence of a catalyst comprising an active component and optionally a support material and wherein the active component comprises at least one ceria compound.
  • the oxidation of hydrogen chloride to chlorine is an equilibrium reaction.
  • the position of the equilibrium shifts with increasing temperature to the detriment of the desired end product. It is therefore advantageous to use catalysts with the highest possible activity, which allow the reaction to proceed at low temperature.
  • the first catalysts for the hydrogen chloride oxidation with the catalytically active component ruthenium were already described in DE-A-1567788 in 1965, in this case starting from RuCl 3 .
  • ruthenium-based catalysts with the active component of ruthenium oxide or ruthenium mixed oxide were described in DE-A 19748299.
  • the content of ruthenium oxide is from 0.1% by weight to 20% by weight and the average particle diameter of ruthenium oxide is from 1.0 nm to 10.0 nm.
  • ruthenium chloride catalysts described therein which also contain at least one of the compounds titanium dioxide and zirconium dioxide
  • a number of Ruthenium starting compounds are given, such as, for example, ruthenium-carbonyl complexes, ruthenium salts of inorganic acids, ruthenium-nitrosyl complexes, ruthenium-amine complexes, ruthenium complexes of organic amines or ruthenium-acetylacetonate complexes.
  • titanium dioxide in the form of rutile was used as carrier.
  • the ruthenium catalysts according to the above disclosures already have quite a high activity; however, for industrial use in hydrogen chloride oxidation, a further increase in activity with good long-term stability is desirable.
  • BE 658435 describes a process using ceria and tetravalent iridium, in which hydrogen chloride is oxidized to chlorine.
  • the process according to BE 658435 is in particular a process which starts from aqueous solutions of hydrogen chloride and which relies on the presence of the abovementioned iridium components or other cocatalysts.
  • aqueous phase either involves working at atmospheric pressure (1013 hPa) at low temperatures in order to prevent evaporation of the reaction solution, in which the co-catalyst components are dissolved or that an increasing pressure in the reaction zone would have to be generated in order to prevent evaporation of the reaction solution.
  • atmospheric pressure 1013 hPa
  • ceria-based catalysts have high activity for the gas phase oxidation of hydrogen chloride to chlorine.
  • ceria-based catalysts offer economic advantages because they are cheaper than the materials conventionally used in the art.
  • the present invention therefore provides a process for the production of chlorine by catalytic gas-phase oxidation of hydrogen chloride in the presence of a catalyst containing a active component and optionally a carrier material, characterized in that the active component comprises a cerium oxide.
  • the catalyst used also comprises a carrier material.
  • Suitable support materials for the catalyst include, for example, silica, alumina (e.g., in ⁇ or ⁇ modifications), titania (as rutile, anatase, etc.), tin dioxide, zirconia, uranium oxide, carbon nanotubes, or mixtures thereof.
  • Ceria in the context of the present invention, denotes a compound containing at least Cerium and oxygen.
  • the cerium oxide consists of cerium and oxygen in any non-stoichiometric composition.
  • cerium oxide CeO 2 is particularly preferred.
  • the cerium oxide may also contain chlorine in addition to cerium and oxygen.
  • the cerium oxide is then a cerium oxychloride (CeO x Cl Y ).
  • the aforementioned catalysts comprising cerium oxide are particularly advantageous because they surprisingly have an extremely high activity and stability for the gas phase oxidation of hydrogen chloride to chlorine.
  • the active component of the catalyst used in the process may be ceria alone or the active component may comprise other catalytically active substances for the gas phase oxidation of hydrogen chloride to chlorine.
  • Suitable further catalytically active substances are those selected from the list consisting of ruthenium, osmium, rhodium, iridium, palladium, platinum, copper, silver, gold, rhenium, bismuth, cobalt, iron, antimony, tin, zirconium, uranium, manganese, lanthanum and chrome.
  • ruthenium, gold, bismuth, uranium, lanthanum or zirconium and its compounds are used.
  • ruthenium is used in oxidic form or as a chloride compound or as an oxychloride compound.
  • the catalyst used in the process comprises a carrier material, the proportion of the active component of the catalyst used is usually in the range from 0.1 to 90% by weight, preferably in the range from 1 to 60% by weight. particularly preferably in the range of 1 to 50 wt .-%, based on the total mass of active component and support material.
  • the active component can be applied to the above-described support material by various methods so that the catalyst used in the process is obtained.
  • wet and wet impregnation of a support material with suitable, present in solution starting compounds or starting compounds in liquid or collodial form, up and co-Avemsocilclar, and ion exchange and gas phase coating (CVD, PVD) can be used.
  • Catalysts suitable in the process according to the invention can be obtained in the embodiments of the invention in which the catalyst also comprises a support material, for example by applying cerium or cerium compounds to a support material and subsequent drying or drying and calcination.
  • the catalytically active component is preferably applied to the carrier material in the form of an aqueous solution or suspension, and the solvent is then removed.
  • reducing preferably hydrogen, hydrides or hydrazine compounds
  • alkaline substances preferably NaOH, KOH or ammonia
  • the active component may be applied to the support material in a non-oxidic form and converted to the oxidized form in the course of the reaction.
  • the catalytically active component can be applied as an aqueous solution or suspension of cerium halides, oxides, hydroxides or oxyhalides, hydroxides, oxyhalides, nitrates, acetates or acetylacetonates each alone or in any desired mixture to the support material and the solvent is subsequently removed.
  • a compound for stabilizing the dispersion of the active component can be used.
  • Suitable dispersion stabilizers are, for example, scandium compounds, manganese oxides and lanthanum oxides.
  • the compounds for stabilizing the dispersion are preferably applied together with the active component by impregnation and / or precipitation.
  • the catalysts obtained according to the above methods for use in the process according to the invention can be dried under normal pressure or preferably under reduced pressure under a nitrogen, argon or air atmosphere at a temperature of 40 to 200 ° C.
  • the drying time is preferably 10 minutes to 6 hours.
  • the catalyst used does not comprise any support material, but only the active component which may contain cerium oxide and optionally further catalytically active substances for gas-phase oxidation of hydrogen chloride to chlorine.
  • the catalytically active component consists only of cerium oxide.
  • the catalytically active component consists only of cerium oxide and the catalyst used comprises no support material
  • the specific surface area determined and named according to the general method of Brunauer Emmet and Teller, also referred to below as BET surface area
  • BET surface area the specific surface area of the catalyst used in the process according to the invention between 1 and 500 m 2 / g, preferably between 5 and 300 m 2 / g.
  • the diameter of the cerium oxide used in the process according to the invention is then between 0.1 and 300 nm, preferably between 1 and 200 nm.
  • the catalyst used in the process according to the invention may contain promoters as further component.
  • Suitable promoters are basic metals (for example alkali metals and alkaline earth metals), preference is given to alkali metals, in particular Na and Cs, and alkaline earth metals, particular preference to alkaline earth metals, in particular Sr and Ba.
  • the promoters may, but are not limited to, be applied to the catalyst by impregnation and CVD processes, preferably an impregnation. If, according to the above embodiment, a catalyst comprising a carrier material is used in the process according to the invention, the above impregnation with promoters takes place particularly preferably after application of the catalytically active component to the carrier material.
  • the catalysts can be used uncalcined or calcined in the process according to the invention.
  • the calcination can be carried out in reducing, oxidizing or inert phase, preferably the calcination in an air or nitrogen stream.
  • the calcination is usually carried out in the absence of oxygen in a temperature range of 150 to 100 ° C, preferably in the range 200 to 1100 0 C. In the presence of oxidizing gases, the calcination takes place in a temperature range of 150 to 1500 0 C, preferably in the range 200 bis 1100 0 C.
  • the catalyst comprising cerium oxide used in the process according to the invention can also be subjected to a pretreatment.
  • the pretreatment is usually a pretreatment under the process conditions of use of the catalyst in the inventive method.
  • catalysts disclosed herein are preferably used in the oxidation of hydrogen chloride with oxygen, pretreatment with a stoichiometric mixture of oxygen and hydrogen chloride is preferred.
  • the pretreatment is usually carried out for at least 10 h. Preferably at least for 50 h, more preferably at least for 100 h.
  • the catalyst used in the process according to the invention and in particular that obtained according to the above embodiments is characterized by a high activity in the hydrogen chloride oxidation at low temperature.
  • cerium oxides form "oxygen defect lattice sites" and can thus actively support redox cycles, while at the same time possessing high stability towards hydrogen chloride.
  • the reaction temperature is usually 150 to 750 0 C, the usual reaction pressure is 1 to 25 bar. Since it is an equilibrium reaction, it is expedient to work at the lowest possible temperatures at which the catalyst still has sufficient activity. Furthermore, it is expedient to use oxygen in excess of stoichiometric amounts of hydrogen chloride. For example, a two to fourfold oxygen Excess. Since no loss of selectivity is to be feared, it may be economically advantageous to work at relatively high pressure and, accordingly, longer residence time than normal pressure.
  • the catalytic hydrogen chloride oxidation may adiabatically or preferably isothermally or approximately isothermally, discontinuously, but preferably continuously as flow or
  • Fixed bed process preferably as a fixed bed process, particularly preferably in tube bundle reactors of heterogeneous catalysts at a reactor temperature of 180 to 750 0 C, preferably 200 to
  • 650 0 C more preferably 220 to 600 0 C and a pressure of 1 to 25 bar (1000 to 25000 hPa), preferably 1.2 to 20 bar, more preferably 1.5 to 17 bar and in particular 2.0 to 15 bar be performed.
  • 1 to 25 bar 1000 to 25000 hPa
  • 1.2 to 20 bar more preferably 1.5 to 17 bar and in particular 2.0 to 15 bar be performed.
  • Typical reactors in which the catalytic hydrogen chloride oxidation is carried out are fixed bed or fluidized bed reactors.
  • the catalytic hydrogen chloride oxidation can preferably also be carried out in multiple stages.
  • a further preferred embodiment of a device suitable for the method consists in using a structured catalyst bed in which the catalyst activity increases in the flow direction.
  • Such a structuring of the catalyst bed can take place, for example, when using catalysts comprising a carrier material by different impregnation / impregnation of the carrier materials with active component or by different dilution of the catalyst with an inert material.
  • inert material for example, rings, cylinders or balls of titanium dioxide, zirconium dioxide or mixtures thereof, alumina, steatite, ceramic, glass, graphite or stainless steel can be used.
  • the inert material should preferably have similar external dimensions.
  • Suitable shaped catalyst bodies are shaped bodies with arbitrary shapes, preference being given to tablets, rings, cylinders, stars, carriage wheels or spheres, particular preference being given to spheres, rings, cylinders or star strands as molds.
  • the volume ratio of hydrogen chloride to oxygen at the reactor inlet is preferably between 1: 1 and 20: 1, preferably between 2: 1 and 8: 1, more preferably between 2: 1 and 5: 1.
  • the conversion of hydrogen chloride in a single pass can be limited to 15 to 90%, preferably 40 to 85%, particularly preferably 50 to 70%. After conversion, unreacted hydrogen chloride can be partly or completely recycled to the catalytic hydrogen chloride oxidation.
  • the process according to the invention results in particular in advantageous productivities expressed in terms of mass of chlorine produced per mass of catalyst material used and hour. These are usually in the range of 0.1 to 50 kg C i 2 per kg ⁇ ata! Ysato r and hour, in carrying out the inventive method according to its preferred variants between 5 and 50, in particularly preferred variants between 20 and 50 kgc ß / kg cat 'H.
  • the heat of reaction of the catalytic hydrogen chloride oxidation can be used advantageously for the production of high-pressure steam. This can be used to operate a phosgenation reactor and / or distillation columns, in particular of isocyanate distillation columns.
  • Example 1 Ceria catalyst with calcination at 300 0 C.
  • Example 2 Ceria catalyst with calcination at 500 ° C.
  • Example 3 Ceria catalyst with calcination at 600 0 C.
  • Example 4 Ceria catalyst with calcination at 700 ° C.
  • Example 5 Catalyst comprising cerium oxide on lanthanum zirconium oxide
  • Example 2 The procedure was analogous to Example 1, with the only difference that 2 g of a pulverulent commercial cerium oxide on lanthanum zirconium oxide (Ce / La / Zr 30/5/65, Fa. Priem) was used instead of the powdery cerium oxide.
  • a pulverulent commercial cerium oxide on lanthanum zirconium oxide Ce / La / Zr 30/5/65, Fa. Priem
  • Example 6 Catalyst comprising ceria on tin (TV) oxide support
  • the quartz reaction tube was heated to 500 ° C and subsequently operated at this temperature.
  • a gas mixture of 80 ml / min HCl and 80 ml / min oxygen was passed through the quartz reaction tube. After 30 minutes, the product gas stream was passed into a 16% by weight potassium iodide solution for 10 minutes, and the resulting iodine was back titrated with a 0.1 N thiosulfate solution to determine the amount of chlorine introduced.
  • Examples 16-19 Use of the Catalysts of Examples 1-4 in the HCl Oxidation at 600 0 C.
  • Example 20 Use of the catalyst according to Example 6 in the HCl oxidation at 300 0 C.

Abstract

La présente invention porte sur un procédé de fabrication de chlore par oxydation catalytique de chlorure d'hydrogène en présence d'un catalyseur qui comprend un composant actif et le cas échéant un matériau support, le composant actif comprenant au moins un composé oxyde de cérium.
PCT/EP2010/002962 2009-05-16 2010-05-14 Procédé de fabrication de chlore par oxydation en phase gazeuse de chlorure d'hydrogène en présence d'un catalyseur oxyde de cérium WO2010133313A1 (fr)

Applications Claiming Priority (2)

Application Number Priority Date Filing Date Title
DE200910021675 DE102009021675A1 (de) 2009-05-16 2009-05-16 Verfahren zur Herstellung von Chlor durch Gasphasenoxidation von Chlorwasserstoff in Gegenwart eines Ceroxid-Katalysators
DE102009021675.8 2009-05-16

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Cited By (3)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
JP2014520742A (ja) * 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 断熱反応カスケードにおける酸化セリウム触媒を使用する塩素の製造方法
CN108602060A (zh) * 2016-02-04 2018-09-28 科思创德国股份有限公司 通过气相氧化制备氯气的催化剂和方法
CN113135552A (zh) * 2020-01-19 2021-07-20 中南大学 一种氯化氢催化氧化制氯气的方法

Families Citing this family (2)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
EP2729408A1 (fr) 2011-07-05 2014-05-14 Bayer Intellectual Property GmbH Procédé pour la production de chlore utilisant un catalyseur à base d'oxyde de cérium dans un réacteur isotherme
IN2014CN02995A (fr) 2011-10-24 2015-07-03 Bayer Ip Gmbh

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US2451870A (en) * 1942-09-04 1948-10-19 Standard Oil Dev Co Chlorine manufacture
US3114607A (en) * 1959-09-01 1963-12-17 Kellogg M W Co Halogen production
US20070238909A1 (en) * 2006-02-03 2007-10-11 Gadewar Sagar B Continuous process for converting natural gas to liquid hydrocarbons
WO2009010168A1 (fr) * 2007-07-13 2009-01-22 Bayer Technology Services Gmbh Procédé de production de chlore par oxydation adiabatique en phase gazeuse à plusieurs niveaux
WO2009035234A2 (fr) * 2007-09-10 2009-03-19 Hanwha Chemical Corperation Processus de production de chlore par oxydation de chlorure d'hydrogène

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BE658435A (fr)
NL6404460A (fr) 1964-04-23 1965-10-25
CN1475434A (zh) 1996-08-08 2004-02-18 ס�ѻ�ѧ��ҵ��ʽ���� 氯的生产方法
CN1182717A (zh) 1996-10-31 1998-05-27 住友化学工业株式会社 氯气的生产方法

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Publication number Priority date Publication date Assignee Title
US2451870A (en) * 1942-09-04 1948-10-19 Standard Oil Dev Co Chlorine manufacture
US3114607A (en) * 1959-09-01 1963-12-17 Kellogg M W Co Halogen production
US20070238909A1 (en) * 2006-02-03 2007-10-11 Gadewar Sagar B Continuous process for converting natural gas to liquid hydrocarbons
WO2009010168A1 (fr) * 2007-07-13 2009-01-22 Bayer Technology Services Gmbh Procédé de production de chlore par oxydation adiabatique en phase gazeuse à plusieurs niveaux
WO2009035234A2 (fr) * 2007-09-10 2009-03-19 Hanwha Chemical Corperation Processus de production de chlore par oxydation de chlorure d'hydrogène

Cited By (3)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
JP2014520742A (ja) * 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 断熱反応カスケードにおける酸化セリウム触媒を使用する塩素の製造方法
CN108602060A (zh) * 2016-02-04 2018-09-28 科思创德国股份有限公司 通过气相氧化制备氯气的催化剂和方法
CN113135552A (zh) * 2020-01-19 2021-07-20 中南大学 一种氯化氢催化氧化制氯气的方法

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