EP2054340A2 - Procédé de production de chlore par oxydation en phase gazeuse - Google Patents

Procédé de production de chlore par oxydation en phase gazeuse

Info

Publication number
EP2054340A2
EP2054340A2 EP07725055A EP07725055A EP2054340A2 EP 2054340 A2 EP2054340 A2 EP 2054340A2 EP 07725055 A EP07725055 A EP 07725055A EP 07725055 A EP07725055 A EP 07725055A EP 2054340 A2 EP2054340 A2 EP 2054340A2
Authority
EP
European Patent Office
Prior art keywords
catalyst
metal sulfide
oxide
hydrogen chloride
catalyst metal
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Withdrawn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
EP07725055A
Other languages
German (de)
English (en)
Inventor
Aurel Wolf
Oliver Felix-Karl SCHLÜTER
Leslaw Mleczko
Stephan Schubert
Jürgen KINTRUP
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.)
Covestro Deutschland AG
Original Assignee
Bayer MaterialScience AG
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
Application filed by Bayer MaterialScience AG filed Critical Bayer MaterialScience AG
Publication of EP2054340A2 publication Critical patent/EP2054340A2/fr
Withdrawn legal-status Critical Current

Links

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
    • B01J27/00—Catalysts comprising the elements or compounds of halogens, sulfur, selenium, tellurium, phosphorus or nitrogen; Catalysts comprising carbon compounds
    • B01J27/02—Sulfur, selenium or tellurium; Compounds thereof
    • B01J27/04—Sulfides
    • 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
    • B01J27/02—Sulfur, selenium or tellurium; Compounds thereof
    • B01J27/04—Sulfides
    • B01J27/043—Sulfides with iron group metals or platinum group metals
    • B01J27/045—Platinum group metals

Definitions

  • the invention relates to a process for the production of chlorine by catalytic gas phase oxidation of hydrogen chloride with oxygen, wherein the catalyst comprises at least one carrier substance and at least one catalyst metal sulfide, and novel catalysts comprising at least one carrier substance and at least one catalyst metal sulfide.
  • 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 contained as active component copper chloride or oxide and were already described in 1868 by Deacon. However, these showed low activity at low temperature ( ⁇ 400 0 C). Although the activity could be increased by increasing the reaction temperature, it was disadvantageous that the volatility of the active components at high temperatures led to a rapid decrease in the catalyst activity.
  • EP 0 184 413 describes the oxidation of hydrogen chloride with catalysts based on chromium oxides. However, the process realized thereby had insufficient activity and high reaction temperatures.
  • the first catalysts for the hydrogen chloride oxidation with the catalytically active component ruthenium were already described in 1965 in DE 1 567 788. In this case starting from RuC13 eg supported on silica and alumina. However, the activity of these RuC13 / SiO2 catalysts was very low. Further Ru-based catalysts with the active material ruthenium oxide or ruthenium mixed oxide and as carrier material various oxides, such as, for example, titanium oxide, zirconium dioxide, etc., have been 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 supported on titanium oxide or zirconium oxide are known from DE-A 197 34 412 known.
  • ruthenium chloride and ruthenium oxide catalysts described therein which contain at least one compound titanium oxide and zirconium oxide
  • Ru starting compounds 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.
  • TiO 2 was used as a carrier in the form of rutile.
  • the ruthenium oxide catalysts have quite high activity, but their preparation is complicated and requires a series of operations such as precipitation, impregnation followed by precipitation, etc., whose scale-up is technically difficult. In addition, ruthenium oxide catalysts also tend to sinter at high temperatures and thus to deactivate.
  • WO 2004/031074 describes supported catalysts based on gold. As an advantage of their higher compared to Ru catalysts activity at low temperatures ( ⁇ 250 0 C) is given; however, this is not supported by information or examples.
  • the previously developed catalysts for the Deacon process have a number of shortcomings. At low temperatures their activity is insufficient. Although the activity could be increased by increasing the reaction temperature, this led to sintering / deactivation or loss of the catalytic component. Furthermore, the conventional catalysts can be sensitive to traces of sulfur in the feed gas stream.
  • the object of the present invention was to provide a catalytic system which effects the oxidation of hydrogen chloride at low temperatures and with high activities and exhibits a low sensitivity to sulfur in the feed gas stream.
  • the task is solved by the development of a very specific combination of catalytically active components and carrier materials.
  • the carrier substance is preferably selected from the group consisting of oxides and mixed oxides of metals or semimetals, such as titanium oxides, tin oxides, aluminum oxides, zirconium oxides, silicon oxides, magnesium oxide, titanium mixed oxides, zirconium mixed oxides, mixed aluminum oxides and mixed silicon oxides and Soot and carbon nanotubes.
  • Oxidide (IV) dioxide, carbon black or carbon nanotubes are used as carriers of the catalytically active component.
  • the metal of the catalyst metal sulfide is preferably selected from the group consisting of: Ru, Os, Cu, Au, Bi, Pd, Pt, Rh, Ir, Re and Ag and mixtures thereof.
  • Suitable catalytically active metal of the catalyst metal sulfide are, in particular, the following elements: ruthenium, iridium and platinum, preferably ruthenium in combination with iridium or platinum.
  • the loading of the catalytically active component in the range of 0.1- 80 wt .-%, preferably in the range of 1-50 wt .-%, particularly preferably in the range of 1- 20 wt .-% based on the amount of Metal in the catalyst.
  • the catalytic component can be applied by various methods. For example, but not limited to, 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 sulfidic (preferably sodium sulfide or hydrogen sulfide) substances.
  • sulfidic preferably sodium sulfide or hydrogen sulfide
  • Suitable promoters are basic 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, 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 methods, preferably an impregnation, particularly preferably after application of the main catalytic component.
  • various dispersion stabilizers such as scandium oxides, manganese oxides and lanthanum oxides, etc. are used.
  • the stabilizers are preferably applied together with the main catalytic component by impregnation and / or precipitation.
  • the stabilizers mentioned generally also stabilize the specific surface area of the carriers used at high temperatures.
  • the catalysts can be dried under normal pressure or preferably at reduced pressure at 40 to 200 0 C.
  • the drying time is preferably 10 minutes to 6 hours.
  • catalysts comprising at least one carrier substance selected from carbon nanorubes, tin dioxide, titanium dioxide and carbon black, and at least one catalyst metal sulfide selected from ruthenium, iridium, platinum and rhodium and mixtures thereof.
  • catalysts wherein the catalyst metal sulfide is selected from mixtures of Ru and Pt sulfides, as well as Ru and Ir sulfides.
  • the catalysts can be used uncalcined or calcined.
  • the calcination can be carried out in reducing, oxidizing or inert phase, preferred is the calcination in an air, oxygen or nitrogen stream, more preferably under nitrogen.
  • the calcination is carried out in a temperature range of 150 to 600 0 C 1 preferably in the range 200 to 300 0 C.
  • the calcining time is preferably 1- 24 h.
  • the catalyst is preferably used as described above in the catalytic process known as the Deacon process.
  • 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 500 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 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 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 500 0 C, preferably 200 to 400 0th 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 several 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 done by different impregnation of the catalyst support with active material 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 external dimensions.
  • Suitable shaped catalyst bodies are shaped bodies with any desired shapes, preference being given to tablets, rings, cylinders, stars, carriage wheels or spheres, particular preference being given to rings, cylinders or star strands as molds.
  • 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 chlorine formed is separated off.
  • the separation step usually comprises several stages, namely the separation and optionally recycling of unreacted hydrogen chloride from the product gas stream of the catalytic hydrogen chloride oxidation, the drying of the obtained, substantially chlorine and oxygen-containing stream and the separation of chlorine from the dried stream.
  • the separation of unreacted hydrogen chloride and water vapor formed can be carried out by condensation of aqueous hydrochloric acid from the product gas stream of hydrogen chloride oxidation by cooling. Hydrogen chloride can also be absorbed in dilute hydrochloric acid or water.
  • the catalysts according to the invention for the hydrogen chloride oxidation are characterized by a high activity at low temperatures.
  • Example 1 Supporting ruthenium sulfide on carbon black
  • the catalyst from Example 1 was in a solid bed in a quartz reaction tube (diameter 10 mm) at 300 0 C with a gas mixture of 80 ml / min (STP) of hydrogen chloride and 80 ml / min (STP) oxygen flowed through.
  • the quartz reaction tube was heated by an electrically heated sand fluid bed. After 30 minutes, the product gas stream was passed for 10 minutes into 16% potassium iodide solution. The resulting iodine was then back titrated with 0.1 N thiosulfate standard solution to determine the amount of chlorine introduced.
  • the other sulfides shown in Table 1 were tested analogously. The quantities of chlorine listed in Table 1 were obtained.

Abstract

Procédé de production de chlore par oxydation catalytique en phase gazeuse de gaz chlorhydrique avec de l'oxygène, le catalyseur contenant au moins une substance de support et au moins un sulfure métallique catalyseur. La présente invention concerne en outre de nouveaux catalyseurs qui contiennent au moins une substance de support et au moins un sulfure métallique catalyseur.
EP07725055A 2006-05-23 2007-05-10 Procédé de production de chlore par oxydation en phase gazeuse Withdrawn EP2054340A2 (fr)

Applications Claiming Priority (2)

Application Number Priority Date Filing Date Title
DE102006024546A DE102006024546A1 (de) 2006-05-23 2006-05-23 Verfahren zur Herstellung von Chlor durch Gasphasenoxidation
PCT/EP2007/004133 WO2007134723A2 (fr) 2006-05-23 2007-05-10 Procédé de production de chlore par oxydation en phase gazeuse

Publications (1)

Publication Number Publication Date
EP2054340A2 true EP2054340A2 (fr) 2009-05-06

Family

ID=38622213

Family Applications (1)

Application Number Title Priority Date Filing Date
EP07725055A Withdrawn EP2054340A2 (fr) 2006-05-23 2007-05-10 Procédé de production de chlore par oxydation en phase gazeuse

Country Status (9)

Country Link
US (1) US20080003173A1 (fr)
EP (1) EP2054340A2 (fr)
JP (1) JP2009537313A (fr)
KR (1) KR20090015981A (fr)
CN (1) CN101489919A (fr)
DE (1) DE102006024546A1 (fr)
RU (1) RU2008150597A (fr)
TW (1) TW200827299A (fr)
WO (1) WO2007134723A2 (fr)

Families Citing this family (3)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
DE102007020096A1 (de) * 2007-04-26 2008-10-30 Bayer Materialscience Ag Verfahren zur Oxidation von Kohlenmonoxid in einem HCI enthaltenden Gasstrom
US20130004396A1 (en) * 2011-06-30 2013-01-03 Uop Llc Processes and apparatuses for eliminating elemental mercury from flue gas using deacon reaction catalysts at low temperatures
EP3673992B1 (fr) * 2017-08-22 2024-02-07 Mitsui Mining & Smelting Co., Ltd. Catalyseur d'oxydation du méthane

Family Cites Families (5)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
CN1003504B (zh) * 1984-12-03 1989-03-08 三井东圧化学有限公司 氯气制备方法
FR2678179B1 (fr) * 1991-06-26 1995-01-13 Elf Antar France Catalyseur d'hydroraffinage renfermant des sulfures de ruthenium et d'au moins un autre metal sur un support d'oxydes refractaires et procede d'hydroraffinage mettant en óoeuvre ledit catalyseur.
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
DE10244996A1 (de) * 2002-09-26 2004-04-01 Basf Ag Katalysator für die katalytische Chlorwasserstoff-Oxidation

Non-Patent Citations (1)

* Cited by examiner, † Cited by third party
Title
See references of WO2007134723A2 *

Also Published As

Publication number Publication date
US20080003173A1 (en) 2008-01-03
JP2009537313A (ja) 2009-10-29
WO2007134723A2 (fr) 2007-11-29
WO2007134723A3 (fr) 2008-03-27
KR20090015981A (ko) 2009-02-12
CN101489919A (zh) 2009-07-22
TW200827299A (en) 2008-07-01
RU2008150597A (ru) 2010-06-27
DE102006024546A1 (de) 2007-11-29

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