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EP2178637A1 - Catalyseur et procédé pour la production de chore par oxydation en phase gazeuse de chlorure d'hydrogène - Google Patents

Catalyseur et procédé pour la production de chore par oxydation en phase gazeuse de chlorure d'hydrogène

Info

Publication number
EP2178637A1
EP2178637A1 EP08784582A EP08784582A EP2178637A1 EP 2178637 A1 EP2178637 A1 EP 2178637A1 EP 08784582 A EP08784582 A EP 08784582A EP 08784582 A EP08784582 A EP 08784582A EP 2178637 A1 EP2178637 A1 EP 2178637A1
Authority
EP
European Patent Office
Prior art keywords
uranium
catalyst
hydrogen chloride
active component
mixtures
Prior art date
Legal status (The legal status is an assumption and is not a legal conclusion. Google has not performed a legal analysis and makes no representation as to the accuracy of the status listed.)
Withdrawn
Application number
EP08784582A
Other languages
German (de)
English (en)
Inventor
Aurel Wolf
Leslaw Mleczko
Oliver Felix Karl SCHLÜTER
Stephan Schubert
Current Assignee (The listed assignees may be inaccurate. Google has not performed a legal analysis and makes no representation or warranty as to the accuracy of the list.)
Bayer Intellectual Property GmbH
Original Assignee
Bayer Technology Services GmbH
Priority date (The priority date is an assumption and is not a legal conclusion. Google has not performed a legal analysis and makes no representation as to the accuracy of the date listed.)
Filing date
Publication date
Priority claimed from DE200710033113 external-priority patent/DE102007033113A1/de
Priority claimed from DE102007033114A external-priority patent/DE102007033114A1/de
Application filed by Bayer Technology Services GmbH filed Critical Bayer Technology Services GmbH
Publication of EP2178637A1 publication Critical patent/EP2178637A1/fr
Withdrawn legal-status Critical Current

Links

Classifications

    • 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
    • B01J23/38—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of noble metals
    • B01J23/54—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of noble metals combined with metals, oxides or hydroxides provided for in groups B01J23/02 - B01J23/36
    • B01J23/56—Platinum group metals
    • B01J23/63—Platinum group metals with rare earths or 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
    • B01J23/70—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of the iron group metals or copper
    • B01J23/76—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of the iron group metals or copper combined with metals, oxides or hydroxides provided for in groups B01J23/02 - B01J23/36
    • B01J23/83—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of the iron group metals or copper combined with metals, oxides or hydroxides provided for in groups B01J23/02 - B01J23/36 with rare earths or actinides
    • 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
    • B01J23/16—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
    • B01J23/20—Vanadium, niobium or tantalum
    • B01J23/22—Vanadium
    • 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
    • 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
    • B01J23/54—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of noble metals combined with metals, oxides or hydroxides provided for in groups B01J23/02 - B01J23/36
    • B01J23/66—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
    • B01J37/00—Processes, in general, for preparing catalysts; Processes, in general, for activation of catalysts
    • B01J37/02—Impregnation, coating or precipitation
    • B01J37/0201—Impregnation

Definitions

  • the present invention relates to a catalyst and a process for the production of chlorine by catalytic oxidation of hydrogen chloride.
  • the catalyst comprises an active component and a carrier material, wherein the active component comprises at least uranium or a uranium compound.
  • the catalyst is characterized by a high stability and activity at a lower price compared to the precious metals.
  • 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 oxidation of hydrogen chloride with the catalytically active component ruthenium were described as early as 1965 in DE 1 567 788, in this case starting from RuCl 3 .
  • Ru-based catalysts with the active component of ruthenium oxide or ruthenium mixed oxide were described in DE-A 197 48 299.
  • 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.
  • Other supported on titanium oxide or zirconium Ru catalysts are known from DE-A 197 34 412.
  • Ru starting compounds such as, for example, ruthenium-carbonyl complexes, ruthenium salts of inorganic acids, ruthenium-nitrosyl complexes, ruthenium-amine.
  • Complex ruthenium complexes of organic amines or ruthenium-acetylacetonate complexes.
  • titanium dioxide in the form of rutile was used as carrier.
  • the known Ru catalysts already have a fairly high activity, for industrial use in the hydrogen chloride oxidation, a further increase in activity with good long-term stability is desirable. Although the activity of the Ru catalysts could be increased by increasing the reaction temperature, they tend to sinter and thus deactivate at higher temperatures.
  • uranium oxides are used as oxidation catalysts for a number of Komplett gr. Selective oxidations are suitable.
  • a typical example of the use of uranium-based catalysts is the oxidation of CO to CO 2 , as described, for example, by Campbell et al in J. Molec. Cat. A: Chem., (2006), 245 (1-2), 62-68.
  • Further known oxidations catalyzed by uranium-containing mixed oxides are, for example, those of isobutene to acrolein (Corberan et al., Ind. Eng. Chem. Prod. Res.
  • DE 1 078 100 discloses catalysts comprising salts or oxides of silver, uranium or thorium which are located on inert carriers of kaolin, silica gel, diatomaceous earth or pumice. It is not disclosed that the resulting catalysts are calcined, which results in low stability of the disclosed catalysts. It is always disclosed a composition that the presence of silver and salts or
  • the effect is aimed at first enabling a turnover in the interaction of the individual catalytically active constituents.
  • the object of the present invention was therefore to provide a catalyst which accomplishes the oxidation of hydrogen chloride with high activities with good long-term stability and the lowest possible cost.
  • Another object of the present invention was to provide a process for the catalytic gas phase oxidation of hydrogen chloride with oxygen using such a catalyst.
  • uranium-based catalysts have a high activity with good long-term stability for the oxidation of hydrogen chloride to chlorine.
  • uranium-based catalysts offer economic advantages since they are cheaper than the materials conventionally used in the prior art.
  • the present invention therefore provides a catalyst for the catalytic oxidation of hydrogen chloride, characterized in that it comprises at least uranium or a uranium compound and a carrier material as catalytically active components.
  • Suitable support materials for the catalyst include, for example, silica, alumina (e.g., in ⁇ or ⁇ modifications), titania (as rutile, anatase, etc.), tin dioxide, zirconia, ceria, carbon nanotubes, or mixtures thereof.
  • Suitable uranium compounds are, for example, uranium oxides, uranium chlorides and uranium oxychlorides.
  • suitable uranium oxides include, but are not limited to, UO 3 , UO 2 , UO or the non-stoichiometric phases resulting from the mixtures, such as U 3 O 5 , U 2 O 51 U 3 O 7 , U 3 O 8 , U 4 O 9 and / or Uj 3 O 34.
  • catalysts comprising uranium oxide or mixtures of uranium oxide as catalysts are particularly advantageous because they surprisingly have an extremely high activity and stability for oxidation reactions.
  • the chloride compounds or the oxychloride compounds can be used as a precursor for the uranium oxides.
  • the uranium or the uranium compound can be used alone or together with other catalytically active components.
  • Suitable further catalytically active components are those selected from the list containing ruthenium, osmium, rhodium, iridium, palladium, platinum, copper, silver, gold, rhenium, bismuth, cobalt, iron, antimony, tin, manganese and chromium.
  • ruthenium, gold, bismuth, cerium or Zr and its compounds are used.
  • ruthenium is used in oxidic form or as a chloride compound or as an oxychloride compound.
  • the proportion of the active component is usually in the range from 0.1 to 90% by weight, preferably in the range from 1 to 60% by weight, more preferably in the range from 1 to 50% by weight, based on the total mass of active Component and carrier material.
  • the active component can be applied to the substrate by various methods. For example, wet and wet impregnation of a support material with suitable solution starting compounds or starting compounds in liquid or collodial form, up and co-impingement methods, as well as ion exchange and gas phase coating (CVD, PVD) can be used. Suitable catalysts can be obtained, for example, by applying uranium or uranium compounds to the support material and then drying or drying and calcining.
  • a catalyst is preferred in which the active component is applied to the carrier material in the form of an aqueous solution or suspension and the solvent is subsequently 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.
  • a catalyst which is characterized in that the catalytically active constituent is in the form of an aqueous solution or suspension of uranium halides, oxides, hydroxides or oxyhalides, uranyl halides, oxides, hydroxides, Oxyhalides, nitrates, acetates or acetylacetonates each alone or in any mixture is applied to the carrier and the solvent is then removed.
  • the catalytically active constituent is in the form of an aqueous solution or suspension of uranium halides, oxides, hydroxides or oxyhalides, uranyl halides, oxides, hydroxides, Oxyhalides, nitrates, acetates or acetylacetonates each alone or in any mixture is applied to the carrier and the solvent is then removed.
  • the catalyst may contain promoters as further component.
  • Suitable promoters are basic-acting metals (for example alkali, alkaline earth and rare earth metals), preference is given to alkali metals, in particular Na and Cs, and alkaline earth metals, particularly preferably alkaline earth metals, in particular Sr, Ba, and the rare earth metal Ce.
  • the promoters may, but are not limited to, be applied to the catalyst by impregnation and CVD processes; preference is given to impregnation, particularly preferably after application of the main catalytic component.
  • the catalyst may contain as further component compounds for stabilizing the dispersion of the active component.
  • 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 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 catalysts can be used uncalcined or calcined.
  • 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 from 150 to 100 0 C, preferably in the range 200 to 1100 0 C.
  • oxidizing gases 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 a uranium or a uranium compound may be subjected to a pretreatment.
  • the pretreatment is usually a pretreatment under the process conditions of use of the catalyst. Since the catalysts disclosed herein are preferably used in the oxidation of HCl with oxygen, pretreatment with a stoichiometric mixture of oxygen and HCl is preferred. Particularly preferred is a pretreatment with a stoichiometric mixture of HCl and oxygen at at least 400 0 C, preferably at least 500 0 C.
  • 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 pretreatment can be carried out as long as desired at any temperatures. It has been shown that a longer and hotter pretreatment is better than a shorter and colder one.
  • the catalyst obtained as above is characterized by high activity in the hydrogen chloride oxidation at low temperature. Without being bound by theory, it is believed that uranium oxides form "oxygen defect lattice sites" and can thus actively support redox cycles, while uranium oxides have high stability to hydrogen chloride, particularly the most preferred uranium oxides or mixtures of uranium oxides with a stoichiometric Composition of UO 2, i to UO 2.9 .
  • Another object of the present invention is a process for the production of chlorine by catalytic oxidation of hydrogen chloride in the presence of a catalyst comprising an active component and a carrier material, characterized in that the active component comprises uranium or a uranium compound.
  • hydrogen chloride is oxidized to chlorine with oxygen in an exothermic equilibrium reaction in the presence of the catalyst already described above to produce water vapor.
  • 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 four-fold excess of oxygen is customary. 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
  • 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 structuring of the catalyst bed can be carried out by different impregnation of the catalyst support with active component or by different dilution of the catalyst with an inert material.
  • an 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 outer 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 shaping of the catalyst can take place after or preferably before the impregnation of the support material.
  • the conversion of hydrogen chloride in a single pass may preferably 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 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 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.
  • the following examples illustrate but do not limit the present invention.
  • Example 1 Uranium Oxide Catalyst on Tin (TV) Support
  • Example 3 Uranium oxide catalyst on alpha-Al 2 O 3 support
  • Example 5 Uranium oxide catalyst on Al 2 O 3 support with calcination at 800 ° C, and analysis
  • Example 4 Analogously to Example 4, 40 g of gamma-Al 2 O 3 shaped bodies (BET of 200 m 2 / g, Saint Gobain) were impregnated with uranium and calcined.
  • BET gamma-Al 2 O 3 shaped bodies
  • Example 6-8 Use of the catalysts from Examples 1-3 in the HCl oxidation at 500 ° C.
  • Example 1-3 0.2 g of the catalysts obtained according to Example 1-3 were ground and introduced as a mixture with 1 g of silica sand (100-200 microns) in a quartz reaction tube (diameter ⁇ 10 mm).
  • the quartz reaction tube was heated to 500 0 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.
  • Example 9 Use of the catalyst from Example 4 in the HCl oxidation at 540 ° C.

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  • Chemical & Material Sciences (AREA)
  • Organic Chemistry (AREA)
  • Engineering & Computer Science (AREA)
  • Materials Engineering (AREA)
  • Chemical Kinetics & Catalysis (AREA)
  • Inorganic Chemistry (AREA)
  • Catalysts (AREA)

Abstract

L'invention concerne un catalyseur et un procédé de production de chlore par oxydation catalytique de chlorure d'hydrogène. Le catalyseur comprend un composant actif et un matériau de support, le composant actif comprenant au moins de l'uranium ou un composé d'uranium. Ce catalyseur se distingue par une stabilité et une activité élevées pour un prix inférieur à celui des catalyseurs à métaux nobles.
EP08784582A 2007-07-13 2008-07-01 Catalyseur et procédé pour la production de chore par oxydation en phase gazeuse de chlorure d'hydrogène Withdrawn EP2178637A1 (fr)

Applications Claiming Priority (3)

Application Number Priority Date Filing Date Title
DE200710033113 DE102007033113A1 (de) 2007-07-13 2007-07-13 Temperaturstabiler Katalysator für die Chlorwasserstoffgasphasenoxidation
DE102007033114A DE102007033114A1 (de) 2007-07-13 2007-07-13 Verfahren zur Herstellung von Chlor durch Gasphasenoxidation von Chlorwasserstoff
PCT/EP2008/005353 WO2009010182A1 (fr) 2007-07-13 2008-07-01 Catalyseur et procédé pour la production de chore par oxydation en phase gazeuse de chlorure d'hydrogène

Publications (1)

Publication Number Publication Date
EP2178637A1 true EP2178637A1 (fr) 2010-04-28

Family

ID=39790915

Family Applications (2)

Application Number Title Priority Date Filing Date
EP08773671A Withdrawn EP2178636A1 (fr) 2007-07-13 2008-06-26 Catalyseur thermiquement stable pour l'oxydation de chlorure d'hydrogene en phase gazeuse
EP08784582A Withdrawn EP2178637A1 (fr) 2007-07-13 2008-07-01 Catalyseur et procédé pour la production de chore par oxydation en phase gazeuse de chlorure d'hydrogène

Family Applications Before (1)

Application Number Title Priority Date Filing Date
EP08773671A Withdrawn EP2178636A1 (fr) 2007-07-13 2008-06-26 Catalyseur thermiquement stable pour l'oxydation de chlorure d'hydrogene en phase gazeuse

Country Status (6)

Country Link
US (2) US7985395B2 (fr)
EP (2) EP2178636A1 (fr)
JP (2) JP5225377B2 (fr)
CN (2) CN101687178A (fr)
RU (2) RU2486006C2 (fr)
WO (2) WO2009010167A1 (fr)

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CN101687178A (zh) * 2007-07-13 2010-03-31 拜尔技术服务有限责任公司 用于氯化氢气相氧化的热稳定催化剂
DE102008050975A1 (de) * 2008-10-09 2010-04-15 Bayer Technology Services Gmbh Mehrstufiges Verfahren zur Herstellung von Chlor
DE102008050978A1 (de) * 2008-10-09 2010-04-15 Bayer Technology Services Gmbh Urankatalysator und Verfahren zu dessen Herstellung sowie dessen Verwendung
DE102009005320A1 (de) * 2009-01-16 2010-07-22 Bayer Technology Services Gmbh Verfahren und Vorrichtung zur Herstellung von Chlor
DE102009013905A1 (de) 2009-03-19 2010-09-23 Bayer Technology Services Gmbh Urankatalysator auf Träger besonderer Porengrößenverteilung und Verfahren zu dessen Herstellung, sowie dessen Verwendung
DE102009033640A1 (de) 2009-07-17 2011-03-03 Bayer Technology Services Gmbh Verfahren zur Herstellung von Chlor durch Gasphasenoxidation von Chlorwasserstoff in Anwesenheit von Schwefeloxiden
DE102009056700A1 (de) * 2009-12-02 2011-06-16 Bayer Technology Services Gmbh Katalysator bestehend aus Silikathüllen und darin befindlichen, räumlich orientierten Nanopartikeln einer Rutheniumverbindung
CN102000583B (zh) * 2010-11-18 2012-08-15 烟台万华聚氨酯股份有限公司 一种氯化氢氧化制氯气的催化剂及其制备方法
JP2012200700A (ja) * 2011-03-28 2012-10-22 Sumitomo Chemical Co Ltd 臭素の製造方法
US9352270B2 (en) 2011-04-11 2016-05-31 ADA-ES, Inc. Fluidized bed and method and system for gas component capture
DE102011081074A1 (de) 2011-08-17 2013-02-21 Areva Np Gmbh Verfahren zur Herstellung eines Uranoxid als aktive Komponente enthaltenden Katalysators
RU2485046C1 (ru) * 2012-01-10 2013-06-20 Учреждение Российской академии наук Институт химии и химической технологии Сибирского отделения РАН (ИХХТ СО РАН) Способ получения хлора из хлороводорода с помощью вольфрамсодержащих соединений
CN104812467B (zh) 2012-09-20 2017-05-17 Ada-Es股份有限公司 用于恢复被热稳定盐污染的吸附剂上的功能位置的方法和系统
CN105268448B (zh) * 2014-07-21 2017-12-22 上海氯碱化工股份有限公司 以副产氯化氢为原料制备氯气的催化剂及制备方法和应用
CN107684927B (zh) * 2016-08-03 2020-07-28 万华化学集团股份有限公司 一种用于氯化氢氧化制备氯气的催化剂及其制备方法和用途
KR102230978B1 (ko) 2018-02-23 2021-03-23 주식회사 엘지화학 탄화수소의 옥시클로로화 공정용 촉매, 이의 제조방법 및 이를 이용한 탄화수소의 옥시클로로화 화합물의 제조방법
CN111167468B (zh) * 2020-01-03 2022-09-16 万华化学集团股份有限公司 一种氯化氢氧化制氯的催化剂及其制备方法和应用
CN112675834B (zh) * 2021-01-12 2022-09-02 万华化学集团股份有限公司 一种铀基催化剂的制备方法、由其制备的催化剂和在氯化氢氧化制备氯气中的应用
CN113258089A (zh) * 2021-05-21 2021-08-13 西安交通大学 一种含二氧化铀的铂基催化剂及其制备方法

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WO2009010167A1 (fr) 2009-01-22
EP2178636A1 (fr) 2010-04-28
CN101687178A (zh) 2010-03-31
RU2010104937A (ru) 2011-08-20
JP5225377B2 (ja) 2013-07-03
US20100202959A1 (en) 2010-08-12
US7985395B2 (en) 2011-07-26
JP2010533058A (ja) 2010-10-21
CN101743059A (zh) 2010-06-16
RU2010104936A (ru) 2011-08-20
WO2009010182A1 (fr) 2009-01-22
RU2469790C2 (ru) 2012-12-20
US20100183498A1 (en) 2010-07-22
JP5269075B2 (ja) 2013-08-21
RU2486006C2 (ru) 2013-06-27

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