EP2178636A1 - Catalyseur thermiquement stable pour l'oxydation de chlorure d'hydrogene en phase gazeuse - Google Patents

Catalyseur thermiquement stable pour l'oxydation de chlorure d'hydrogene en phase gazeuse

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Publication number
EP2178636A1
EP2178636A1 EP08773671A EP08773671A EP2178636A1 EP 2178636 A1 EP2178636 A1 EP 2178636A1 EP 08773671 A EP08773671 A EP 08773671A EP 08773671 A EP08773671 A EP 08773671A EP 2178636 A1 EP2178636 A1 EP 2178636A1
Authority
EP
European Patent Office
Prior art keywords
catalyst
uranium
carrier
catalyst according
active ingredient
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Withdrawn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
EP08773671A
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 EP2178636A1 publication Critical patent/EP2178636A1/fr
Withdrawn legal-status Critical Current

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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 for oxidation reactions comprising at least one active ingredient in the oxidation reaction catalysis and a carrier therefor, characterized in that the carrier comprises uranium oxides.
  • the catalyst is characterized by higher stability and activity compared to prior art catalysts.
  • uranium oxides are suitable as oxidation catalysts for a number of complete or selective oxidations.
  • a typical example of the use of uranium-based catalysts is CO oxidation to CO 2, as described, for example, by Campbell et al in J. Molec. Cat. A: Chem., (2006), 245 (1-2), 62-68.
  • Further oxidations catalysed by uranium-containing mixed oxides are, for example, those of isobutene to acrolein (Corberan et al., Ind. Eng. Chem. Prod. Res. Dev., (1984), 24, 546, and 1985, 24, 62) and that of propylene to acrolein and acrylonitrile (US Pat.
  • Ruthenium is, as is well known, in particular as a reduction catalyst or as an oxidation catalyst application (Handbook of Heterogeneous Catalysis, 1997, S2160 and S2181).
  • Oxidation under more severe conditions in terms of temperature and oxygen partial pressure is the method of catalytic hydrogen chloride oxidation with oxygen developed by Deacon in 1868:
  • 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 ingredient ruthenium were described as early as 1965 in DE 1 567 788, in this case starting from RuCl 3 .
  • As supports Al 2 O 3 and SiO 2 were claimed.
  • the activity of this combination is relatively low, as these carriers can not provide lattice oxygen atoms for the oxidation process.
  • Ru-based catalysts with ruthenium oxide or ruthenium mixed oxide as the active ingredient were claimed 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.
  • Ru catalysts Other supported on titanium oxide or zirconium Ru catalysts are known from DE-A 197 34 412.
  • ruthenium chloride catalysts described therein which contain at least one compound titanium dioxide and zirconium dioxide
  • 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.
  • Ru catalysts have a fairly high activity, they tend to sinter and thus deactivate at higher temperatures. To increase the economy, however, a further increase in activity with good long-term stability is necessary.
  • the previously developed supported ruthenium oxidation catalyst systems have insufficient activity or stability for the hydrogen chloride oxidation. Although the activity can be increased by increasing the reaction temperature, this leads to sintering / deactivation or to the loss of the catalytically active ingredient.
  • 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. In addition, it is not disclosed that the carrier alone may have a catalytic activity and may consist of uranium oxide. There is always disclosed a composition which detects the presence of silver and salts or oxides of rare earths. Accordingly, in the absence of further disclosure, it can be assumed that the technical teaching aims at a co-catalytic effect, which enables the conversion of the individual catalytically active constituents only a conversion.
  • the object of the present invention was thus to provide a catalyst which accomplishes the oxidation of hydrogen chloride with high activity and / or stability and thereby can be obtained economically advantageous over the prior art.
  • the present invention thus relates to a catalyst for oxidation reactions which comprises at least one active ingredient in the catalysis of oxidation reactions and a carrier therefor, characterized in that the carrier is based on a uranium-containing compound, in particular uranium oxide.
  • a catalyst in which the carrier comprises a uranium oxide is preferred.
  • uranium oxides such as UO 3 , UO 2 , UO or from mixtures of these Species resulting non-stoichiometric phases such as U 3 O 5 , U 2 O 5> U 3 O 7 , U 3 Og, U 4 ⁇ 9 , U] 3 O 34 .
  • Particularly preferred are uranium oxides or mixtures of these with a stoichiometric composition of UO 2 ] to UO 2.9 .
  • Suitable carrier materials which can be combined with uranium oxide are silicon dioxide, rutile or anatase titanium dioxide, zirconium dioxide, aluminum oxide or mixtures thereof, preferably titanium dioxide, zirconium dioxide, aluminum oxide or mixtures thereof, particularly preferably ⁇ - or ⁇ -aluminum oxide or mixtures thereof.
  • the catalyst consists only of a carrier comprising uranium oxide.
  • the at least one active ingredient in the oxidation reaction catalysis is identical to at least one constituent of the carrier and is a uranium oxide or a mixture of uranium oxides.
  • a support as catalyst comprising uranium oxides or mixtures thereof with a stoichiometric composition of U ⁇ 2, i to UO 2i9 .
  • these stoichiometries show a particularly high activity and stability.
  • the uranium oxides can also be combined with the other support materials just described.
  • the catalyst consists only of a carrier comprising uranium oxide and subjected to pretreatment.
  • the pretreatment is usually a pretreatment under the process conditions of use of the catalyst. Since the catalysts disclosed herein are preferred in the Oxidation of HCl with oxygen is used, pretreatment with a stoichiometric mixture of oxygen and HCl is preferred. Preference is given to pretreating with a stoichiometric mixture of HCl and oxygen at at least 400 ° C., preferably at least 500 ° C.
  • the pretreatment is usually at least for 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. There are also shorter and colder pretreatments conceivable. It is a question of weighing how much additional work in pretreatment, which is reflected in increased activity, can be compensated for by this gain in activity. Therefore, the temperature ranges and periods just given are to be understood as meaningful recommendations, but not as technical limitations.
  • the supports / catalysts of this invention and in particular the catalysts of the preferred further development, in which the catalyst consists only of a support comprising uranium oxide, under high temperature loading under process conditions Gaining activity as a pretreatment. All known catalysts behave this essentially opposite.
  • a catalyst is preferred in which the catalytically active constituent is applied to the support in the form of an aqueous solution or suspension and the solvent is then removed.
  • a catalyst which is characterized in that the further catalytically active ingredient is applied as an aqueous solution or suspension of ruthenium halides, oxides, hydroxides or oxyhalides each alone or in any mixture on the support and the solvent then Will get removed.
  • catalytically active ingredients in question are all components that catalyze the hydrogen chloride oxidation.
  • the following elements are suitable or compounds thereof: ruthenium, osmium, rhodium, iridium, palladium, platinum, copper, silver, gold, rhenium, bismuth, cobalt, iron, chromium or mixtures thereof.
  • ruthenium and its compounds are used.
  • ruthenium is used in oxidic form or as a chloride compound or as an oxychloride compound.
  • the further catalytically active ingredient is applied to the carrier in a non-oxidic form and converted into the oxidized form in the course of the reaction.
  • the loading with the catalytically active ingredient is in the range of 0.1 to 80 wt .-%, preferably in the range of 1 to 50 wt .-%, particularly preferably in the range of 1 to 25 wt .-% based on the total mass from catalyst and carrier.
  • the further catalytically active ingredient can be applied by various methods. For example, and without limitation, wet and wet impregnation of a support with suitable starting or starting compounds in liquid or collodial form, up and co-impingement methods, as well as ion exchange and gas phase coating (CVD, PVD) may be employed. Preference is given to a combination of impregnation and subsequent precipitation with reducing (preferably hydrogen, hydrides or hydrazine compounds) or alkaline substances (preferably NaOH, KOH or ammonia).
  • reducing preferably hydrogen, hydrides or hydrazine compounds
  • alkaline substances preferably NaOH, KOH or ammonia
  • 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 and Ba and the rare earth metal Ce.
  • alkali metals in particular Na and Cs
  • alkaline earth metals particularly preferably alkaline earth metals, in particular Sr and Ba and the rare earth metal Ce.
  • the promoters optionally present in addition to the further active constituent may, but are not limited thereto, be applied to the catalyst by impregnation and CVD processes, preferably an impregnation, particularly preferably after application of the further catalytically active constituent.
  • various dispersion stabilizers such as scandium compounds, manganese oxides and lanthanum oxides are used.
  • the stabilizers are preferably applied together with the further catalytic constituent by impregnation and / or precipitation.
  • the catalysts can be dried under atmospheric pressure or preferably under reduced pressure under a nitrogen, argon or air atmosphere at 40 to 200 ° C.
  • the drying time is preferably 10 minutes to 24 hours.
  • the catalysts can be used uncalcined or calcined.
  • the calcination can be carried out in reducing, oxidizing or inert phase, preference being given to calcination in an air or in nitrogen stream.
  • This calcination may be applied to the catalyst of the invention comprising a catalytically active ingredient on one based on a uranium containing compound, in particular uranium oxide, but also the catalyst according to the preferred development in which the at least one is active in the oxidation reaction oxidation Constituent at the same time also the carrier is.
  • the calcining is carried out in the case of a catalyst according to the preferred development of the invention, in the form of carriers comprising uranium oxide or mixtures of uranium oxide as catalysts, in the presence of or in the absence of oxygen in a temperature range of 500 to 1200 0 C, preferably in the range 700 up to 1000 ° C.
  • the calcination is carried out in the case of a catalyst comprising carrier and further catalytically active ingredient in the presence of oxidizing gases in a temperature range of 150 to 500 0 C, preferably in the range of 150 0 C to 300 0 C.
  • the catalytic process known as the Deacon process is preferably used as described above.
  • hydrogen chloride is oxidized with oxygen in an exothermic equilibrium reaction to chlorine, whereby water vapor is obtained.
  • the reaction temperature is usually 150 to 450 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.
  • oxygen in superstoichiometric amounts of hydrogen chloride use. 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.
  • Suitable preferred catalysts for the Deacon process include ruthenium oxide, ruthenium chloride or other ruthenium compounds. Suitable catalysts can be obtained, for example, by applying ruthenium chloride to the support and then drying or drying and calcining. In addition to or instead of a ruthenium compound, suitable catalysts may also contain compounds of other metals, for example gold, palladium, platinum, osmium, iridium, silver, copper, chromium, uranium or rhenium. Suitable catalysts may further contain chromium (III) oxide.
  • the catalytic hydrogen chloride oxidation may be adiabatic or preferably isothermal or approximately isothermal, batchwise, but preferably continuously or as a fixed bed process, preferably as a fixed bed process, more preferably in tube bundle reactors to heterogeneous catalysts at a reactor temperature of 180 to 450 ° C, preferably 200 to 400 ° C, more preferably 220 to 350 ° 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 are 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 plurality of reactors with intermediate cooling that is to say 2 to 10, preferably 2 to 6, particularly preferably 2 to 5, in particular 2 to 3, connected in series.
  • the hydrogen chloride can be added either completely together with the oxygen before the first reactor or distributed over the various reactors.
  • This series connection of individual reactors can also be combined in one apparatus.
  • 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 done by different impregnation of the catalyst support with active material 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 starting from uranium oxide are shaped bodies of any desired shape, 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 1: 1 and 20: 1, preferably 2: 1 and 8: 1, more preferably 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 hydrogen chloride oxidation catalyst of the present invention is characterized by high activity at a low temperature. Without wishing to be bound by theory, it is believed that the uranium oxide can positively contribute to the catalytic cycle via the ability to provide lattice oxygen. Examples
  • a uranium (VI) oxide (from Strem Chemicals) precalcined at 500 ° C. for 4 hours was suspended in 2.8 ml of water in a solution of 0.053 g of Ru (III) chloride hydrate and the mixture was stirred for 60 minutes Room temperature stirred. Subsequently, the water was separated in an air stream at 60 ° C / 4 h. The calcining was carried out at 250 ° C for 16 h in the air stream, whereby a ruthenium catalyst with theoretically calculated (2 wt .-%) Ru supported on uranium (VI) oxide was obtained.
  • VI uranium
  • a 2 wt .-% Ru catalyst on uranium (FV) -Oxid carrier was prepared analogously to Example 1, with the only difference that at 500 ° C for 4 h precalcined U (IV) oxide (Strem Chemicals) was used.
  • a 2 wt .-% Ru catalyst on uranium (V / VI) -Oxid carrier was prepared analogously to Example 1, with the only difference that at 500 0 C for 4 h precalcined U (V / VI) oxide (Strem Chemicals) was used.
  • Example 6 Pure Uranium (VI) Oxide Carrier 2 g of powdered uranium (VI) oxide (Strem Chemicals) were dried overnight at 150 ° C in a drying oven at ambient pressure and then calcined for 2 h under air at 500 ° C.
  • Example 7 Mixed uranium (V / VI) oxide carrier
  • Example 8 Mixed uranium (V / VI) oxide carrier with pretreatment
  • Example 7 The catalyst obtained from Example 7 was subjected to pretreatment for 100 hours at 540 ° C under 80 ml / min HCl and 80 ml / min O 2 . The result is a pretreated catalyst according to Example 8.
  • the moldings were then calcined for four hours at 800 ° C in an air stream.
  • Example 11-14 Using the catalysts of Examples 1-4 in the HCl oxidation at 300 0 C 0.2 g of the catalysts obtained according to Example 1-4 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 300 0 C and operated in the following 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.

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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 pour réactions d'oxydation, comprenant au moins un composant actif catalysant l'oxydation du chlorure d'hydrogène et un support de catalyseur, et caractérisé en ce que le support est à base d'oxyde d'uranium. Ce catalyseur se distingue par une stabilité et une activité élevées.
EP08773671A 2007-07-13 2008-06-26 Catalyseur thermiquement stable pour l'oxydation de chlorure d'hydrogene en phase gazeuse Withdrawn EP2178636A1 (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/EP2008/005183 WO2009010167A1 (fr) 2007-07-13 2008-06-26 Catalyseur thermiquement stable pour l'oxydation de chlorure d'hydrogène en phase gazeuse

Publications (1)

Publication Number Publication Date
EP2178636A1 true EP2178636A1 (fr) 2010-04-28

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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

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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

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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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DE102008050978A1 (de) * 2008-10-09 2010-04-15 Bayer Technology Services Gmbh Urankatalysator und Verfahren zu dessen Herstellung sowie dessen Verwendung
DE102008050975A1 (de) * 2008-10-09 2010-04-15 Bayer Technology Services Gmbh Mehrstufiges Verfahren zur Herstellung von Chlor
DE102009005320A1 (de) * 2009-01-16 2010-07-22 Bayer Technology Services Gmbh Verfahren und Vorrichtung zur Herstellung von Chlor
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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
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US20100183498A1 (en) 2010-07-22
EP2178637A1 (fr) 2010-04-28
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RU2010104936A (ru) 2011-08-20
JP5225377B2 (ja) 2013-07-03
US7985395B2 (en) 2011-07-26
WO2009010182A1 (fr) 2009-01-22
JP2010533059A (ja) 2010-10-21
US20100202959A1 (en) 2010-08-12
CN101743059A (zh) 2010-06-16
RU2469790C2 (ru) 2012-12-20
JP5269075B2 (ja) 2013-08-21
RU2010104937A (ru) 2011-08-20
RU2486006C2 (ru) 2013-06-27
WO2009010167A1 (fr) 2009-01-22

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