WO1991006505A1 - Efficient production of chlorine from hydrogen chloride - Google Patents
Efficient production of chlorine from hydrogen chloride Download PDFInfo
- Publication number
- WO1991006505A1 WO1991006505A1 PCT/US1990/006184 US9006184W WO9106505A1 WO 1991006505 A1 WO1991006505 A1 WO 1991006505A1 US 9006184 W US9006184 W US 9006184W WO 9106505 A1 WO9106505 A1 WO 9106505A1
- Authority
- WO
- WIPO (PCT)
- Prior art keywords
- catalyst
- transition metal
- temperature
- hcl
- metal oxide
- Prior art date
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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
- 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
- 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
-
- 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
Definitions
- This application relates to improved processes for the chemical production of chlorine from gaseous HC1.
- the gaseous HCl can be part of a complex mixture.
- Deacon developed a process by which chlorine is produced by direct oxidation of gaseous HCl with 0 2 in the presence of a CuCl 2 catalyst. This process is described by the overall chemical equation
- Reaction (1) in the presence of a CuCl 2 catalyst is a fast overall exothermic process which is expected to reach equilibrium under normal industrial operating conditions of 700°K to 750°K.
- a number of engineering problems are associated with the Deacon process.
- the temperatures of the process reduce the equilibrium constant for the conversion, resulting in incomplete conversion of the HCl and thereby reducing yield. This is especially a problem when the Deacon process is carried out at a single temperature in a single vessel, furthermore, at elevated temperatures above 675°K, the catalyst's activity rapidly decreases, mainly because of volatilization of the CuCl.
- U.S. Patent No. 2,206,399 to Grosvenor et al. discloses the chlorination and oxidation of a variety of chlorine-carrying multivalent metals, including chromium, cobalt, copper, manganese, nickel, magnesium, and iron.
- the metal is preferably iron.
- U.S. Patent No. 2,577,808 to Pye et al. discloses the use of iron as a chlorine carrier in a fluidized bed reaction where a granular contact mass including ferric oxide falls by gravity through a heating or cooling zone, and then through a chloridizing zone which has a temperature of 300°C at the top and 500°C at the bottom.
- the chlorine carrier now in the form of ferric chloride, falls into an oxidizing zone which has a temperature of 500°C at the top and 550°C at the bottom to oxidize the particles to ferric oxide. These particles are then returned to the top, cooled, and recycled.
- the Chemical Engineer article by J. Th. Quant et al. describes a variation of the Deacon process using a Cu catalyst adsorbed on a porous carrier containing alkali metal chlorides and/or lanthanide chlorides, the so-called “Shell catalyst.”
- the reaction is optimally carried out in a fluidized bed.
- the Kel-Chlor Process involves the reaction of HCl wit nitrosylsulfuric acid (HNS0 5 ) contained in a stream of H 2 S0 4 to produce nitrosyl chloride (NOC1) with eventual production of Cl 2 b oxidation of N0C1.
- UBSTITUTESHEET (3) Direct Oxidation with an Inorganic Oxidizing Agent.
- Oxidizing agents include nitrogen dioxide, sulfur trioxide, or a nitric/sulfuric acid mixture. The reaction is carried out in the liquid phase.
- a process according to the present invention is operable at moderate temperatures and uses a catalyst that does not volatilize and has a relatively long lifetime under the actual reaction conditions of the process. It gives a high yield of Cl 2 and efficient conversion of the HCl to Cl 2 , and can be practiced using a simple apparatus. It requires only limited input of extrinsic energy, making it economical to operate.
- the process comprises the steps of:
- An alkali metal chloride selected from the group consisting of LiCl, NaCl, KCl, and combinations thereof;
- (c) optimally, a promoter selected from the group consisting of LaCl 3 , PrCl 3 , and Pr 2 0 3 , and combinations thereof, the elevated temperature being sufficiently high, in the range of from about 100"C to about 300°C, that the transition metal oxide is converted to transition metal chloride by the HCl with elimination of water; and
- step (2) (2) contacting the transition metal chloride generated in step (1) with a source of oxygen at a temperature increased over the temperature of step (1) , the temperature being sufficient high, at least about 300°C up to about 400°C, that Cl 2 is evolved and the transition metal chloride in the catalyst is reconverted to the transition metal oxide for reuse in step (a) .
- the components are present in the catalyst in a ratio of about 1 mole of alkali metal chloride and up to about 0.2 mole of promoter, if present, per mole of transition metal oxide.
- the elevated temperature in the first step of the reaction is in the range of from about 100"C to about 250"C.
- the transition metal oxide is Mn0 2 , Co 2 0 3 , or Co 3 0 4 , or a combination thereof, most preferably Mn0 2 .
- the Mn0 2 is converted to MnCl 2 by the HCl and water and Cl 2 are evolved in the first step, which preferably occurs at a temperature of from about 100°C to about 250°C.
- the MnCl 2 is contacted with the source of oxygen in the second step at a temperature of from about 350°C to about 375°C.
- Cl 2 is evolved in both steps of the reaction.
- the transition metal oxide is Cr 2 0 3 , NiO, Ni 2 0 3 , or M0 2 0 3 , or a combination thereof.
- the HCl is preferably contacted with the catalyst containing the transition metal oxide at a temperature of from about 100°C to about 225°C.
- the resulting transition metal chloride is preferably contacted with the source of oxygen at a temperature of from about 310°C to about 375°C.
- the transition metal oxide is CuO.
- the temperature range in the first set is from about 100°C to about 300°C.
- the temperature range in the second step is from about 310°C to about 375°C 5 preferably from about 310°C to about 330°C, to prevent volatilization of the copper-containing catalyst.
- the catalyst is preferably supported on an inert support.
- the weight of the catalyst preferably comprises about 10 to about 20 percent of the total weight of the catalyst and the inert support.
- the inert support is preferably gamma-alumina, pumice, silica, or molecular sieve material.
- the source of oxygen for these processes can be 0 2 ; the 0 2 can be diluted with N 2 .
- the source of oxygen can be preheated to provide at least some of the necessary heat for the evolution of Cl 2 and the reconversion of the transition metal chloride in the catalyst to the transition metal oxide.
- the first step of the process can occur in a first reaction zone and the second step in a second reaction zone.
- the process comprises the additional step of recycling reconverted transition metal oxide from the second reaction zone to the first reaction zone.
- the catalysts for the process of the present invention can be contained in a fluidized bed or a stationary bed. When the process occurs in two separate reaction zones, the catalyst can be contained in a fluidized bed in both reaction zones. In particular, the catalyst can be contained in a first fluidized bed in the first reaction zone and a second fluidized bed in the second reaction zone.
- the single figure is a schematic diagram of a single-state reaction vessel usable for the process of the present invention.
- This improvement functionally separates the Deacon process into two steps: Step 1, a chloridizing step; and Step 2, an oxidizing step.
- This functional separation can be performed either by physically moving the catalyst from one reaction vessel to another, or by cycling the temperature between the optima for each step in a single vessel. In the first of these alternatives, each step of the process is actually performed in a separate reaction vessel whose temperature is controlled independently.
- Equations (4) and (5) can be reformulated as follows:
- thermochemistry of the Deacon process Based on our knowledge of the thermochemical properties of these intermediate reactive species and after testing thermochemically the validity of a number of alternative mechanistic routes we have proposed the following reaction mechanism for the Deacon process, using a Cu catalyst:
- the reaction mechanism of the Deacon process consists of both exothermic and endothermic steps, one expects an optimal temperature range for the process, which has been found experimentally.
- the true catalyst for the process is a mixture of the oxide and chloride forms of Cu, the oxide form being necessary for HCl adsorption and the chloride form participating in the Cl 2 release step, opens new avenues for further engineering optimization in terms of feed composition, pressure and temperature cycling, and adaptive control.
- the optimal catalyst in the Deacon process is a variation of the so-called "Shell Catalyst.”
- This catalyst comprises a transition metal oxide, an alkali metal chloride and, optimally, a trivalent rare earth metal chloride or rare earth metal oxide.
- the trivalent rare earth metal chloride or oxide serves as a promoter and is subsequently referred to by this term.
- the transition metal oxide is one of Mn0 2 , Co 2 0 3 , Co 3 0 4 , Cr 2 0 3 , Mo 2 0 3 , CuO, NiO, or Ni 2 0 3 , or mixtures and combinations thereof.
- the alkali metal chloride is preferably LiCl
- the promoter is preferably LaCl 3 or PrCl 3 , but other similar rare earth chlorides, such as NdCl 3 , or a mixture of NdCl 3 and PrCl 3 , as well as trivalent rare earth metal oxides, such as Pr 2 0 3 , can also be used as the promoter.
- the alkali metal chloride is typically present in the catalyst at a ratio of about 1 mole of alkali metal chloride per mole of transition metal oxide.
- the promoter if present, is at a ratio of up to 0.2 mole per mole of transition metal oxide.
- the catalyst is typically supported on an inert support.
- the inert support is preferably gamma-alumina, pumice, silica or molecular sieve material.
- the weight of the catalyst is preferably about 10 percent to about 20 percent of the total weight of the catalyst and the inert support taken together.
- the catalyst is incorporated in high-surface-area material, with a surface area of 100-500 m 2 /g «
- step 1 The reaction with a catalyst using Mn0 2 is exceptional in that Cl 2 is released in both steps of the reaction: step 1, the chloridizing step; and step 2, the oxidizing step.
- step 1 the chloridizing step, the catalyst is contacted with a gas containing HCl at a temperature of from about 25°C to about 250°C, preferably from about 100°C to about 250°C, more preferably no higher than 225°C.
- a gas containing HCl at a temperature of from about 25°C to about 250°C, preferably from about 100°C to about 250°C, more preferably no higher than 225°C.
- the Mn0 2 is converted into MnCl 2 , being reduced from a (+4) oxidation state to a (+2) oxidation state.
- the exit stream of the reaction contains steam and Cl 2 according to the equation
- step 2 the oxidizing step, the chloridized catalyst is then contacted with a source of oxygen at a temperature of at least 300°C but less than about 400°C but sufficiently high that Cl 2 is evolved and the MnCl 2 is reconverted to the original catalytic Mn0 2 for reuse in the first step.
- the temperature of step 2 is increased over that of step 1.
- the temperature is preferably from about 350°C to about 375°C at this step.
- This step is also exothermic with a H of -8 kcal, and takes place according to the equation
- the source of oxygen in this step can be 0 2 gas, pure or diluted with N 2 , or air.
- the source of oxygen is preheated to provide at least some of the necessary heat not provided by the reaction itself for the evolution of Cl 2 and the reconversion of MnCl 2 to Mn0 2 . Additional heat is required because of the considerable rise in temperature in going from the first step to the second step. Any 0 2 not consumed can be recycled.
- the pressure of the reaction is close to about 1 atmosphere, but there is no theoretical limit on the pressure, and use of a supra-atmospheric pressure, such as about 10 atmospheres, might be beneficial for the production of chlorine.
- SUBSTITUTE SHEET Co 2 0 3 or Co 3 0 4 can be substituted for Mn0 2 in this version of this invention.
- the temperature limits in the first step are preferably from about 100°C to about 225°C if a catalyst containing metal oxides other than CuO is used. If a catalyst containing CuO is used, the optimum temperature for the first step can range from about 100°C to about 300°C.
- the temperature of the second step is at least about 300°C but less than about 400°C, sufficiently high that Cl 2 is evolved and the metal chloride is reconverted to a metal oxide for reuse in the first step.
- the temperature of the second step is increased over that of the first step. More preferably, the temperature in the second step is to be from about 310°C to about 375°C.
- the temperature of the second step should be from about 310°C to 375°C. If the catalyst does contain CuO, the temperature of the second step should be from about 310°C to 375°C, more preferably from about 310°C to about 330°C.
- the maximum temperature should be limited when the catalyst contains CuO to avoid volatilization of the catalyst.
- FIG. 1 shows a reaction vessel suitable for carrying out the two-step process using a catalyst continuing Mn0 2 .
- the catalyst 10 is contained in the body 12 of the reaction vessel 14.
- a first inlet 16, controlled by valve 18 admits the HCl-containing gas for the performance of the first, chloridizing, step.
- a second inlet 10, controlled by valve 22, admits the source of oxygen, such as 0 2 gas, for the performance of the second, oxidizing step.
- An outlet 24, controlled by valve 26, allows escape of the effluent gas in each step for further processing.
- the vessel is surrounded by a temperature control mechanism (not shown) that can supply or remove heat as needed to keep the temperature within the required limits.
- reaction can be carried out in a fixed bed or fluidized bed reactor.
- the reaction can be carried out in an apparatus in which the first, chloridizing, step occurs in a first reaction zone and the second, oxidizing, step occurs in a second reaction zone.
- the reaction further comprises the step of recycling reconverted transition metal catalyst from the second reaction zone to the first reaction zone.
- a separate fluidized bed can be used to contain the catalyst in each reaction zone.
- a quartz tube of 15 mm I.D. was packed with glass wool and about 10-12 g of alumina- or silica-supported metal oxide catalyst.
- the metal oxide content varied between 10 and 20 weight percent of the total weight of the catalyst, including the support. the tube was located in an electrically heated furnace whose temperature was adjustable.
- the HCl-saturated catalyst was preheated to the desired temperature, usually about 350°C, and 0 2 circulated over the catalyst until no further Cl 2 was deposited in the dry ice trap. Measurements of Cl 2 were done by titration and 0 2 consumption was measured by pressure drop. No products other than Cl 2 were ever found in the oxygen experiments.
- Example 3 MnO, At 100-250°C, HCl was completely absorbed and both H 2 0 and Cl 2 , both condensed, were liberated. The resulting MnCl 2 evolved Cl 2 slowly from 350° to 400° and then rapidly at about 400°C.
- Example 4 - V ? 0. At 190°C, absorption was complete with only H 2 0 liberation. On heating the catalyst above 250"C , both Cl 2 and a volatile chloride, probably V0 2 C1 or V0C1 3 , were evolved.
- alkali metal oxides and alkaline earth metal oxides such as Na 2 0, CaO, or MgO, whose chlorides do not react with 0 2 below 900°C, and metal oxides such as A1 2 0 3 that do not react above 100°C with HCl to form chlorides;
- Oxides from classes (1) and (2) are not suitable for commercial processes.
- Oxides from classes (3) and (4) are suitable for such processes. All of them can be benefitted by mixtures with other oxides from these same categories and/or from mixtures with alkali metal halides which tend to lower the melting points of the chlorides formed in the reaction with HCl and then facilitate the rate of the later reaction with 0 2 .
- a process according to the present invention has many advantages. Such a process is commercially useful for the preparation of chlorine from HCl and operates more efficiently than currently used processes by functionally separating the Deacon process into two steps: a chloridizing step and an oxidizing step.
- the process gives a nearly quantitative conversion of HCl to chlorine and operates under conditions in which the catalyst does not volatilize, and under which the activity of the catalyst remains stable.
- the process also requires only limited input of extrinsic energy and operates at relatively moderate temperatures and without corrosion of its surroundings.
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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)
- Organic Low-Molecular-Weight Compounds And Preparation Thereof (AREA)
Abstract
Description
Claims
Priority Applications (3)
Application Number | Priority Date | Filing Date | Title |
---|---|---|---|
EP90917325A EP0500728B1 (en) | 1989-11-02 | 1990-10-26 | Efficient production of chlorine from hydrogen chloride |
DE69019981T DE69019981T2 (en) | 1989-11-02 | 1990-10-26 | EFFICIENT METHOD FOR PRODUCING CHLORINE FROM HYDROCHLORINE. |
CA002072109A CA2072109C (en) | 1989-11-02 | 1990-10-26 | Efficient production of chlorine from hydrogen chloride |
Applications Claiming Priority (2)
Application Number | Priority Date | Filing Date | Title |
---|---|---|---|
US43080589A | 1989-11-02 | 1989-11-02 | |
US430,805 | 1989-11-02 |
Publications (1)
Publication Number | Publication Date |
---|---|
WO1991006505A1 true WO1991006505A1 (en) | 1991-05-16 |
Family
ID=23709110
Family Applications (1)
Application Number | Title | Priority Date | Filing Date |
---|---|---|---|
PCT/US1990/006184 WO1991006505A1 (en) | 1989-11-02 | 1990-10-26 | Efficient production of chlorine from hydrogen chloride |
Country Status (8)
Country | Link |
---|---|
EP (1) | EP0500728B1 (en) |
AT (1) | ATE123476T1 (en) |
AU (1) | AU6747890A (en) |
CA (1) | CA2072109C (en) |
DE (1) | DE69019981T2 (en) |
ES (1) | ES2073041T3 (en) |
PT (1) | PT95777A (en) |
WO (1) | WO1991006505A1 (en) |
Cited By (7)
Publication number | Priority date | Publication date | Assignee | Title |
---|---|---|---|---|
EP0743277A1 (en) * | 1995-05-18 | 1996-11-20 | Sumitomo Chemical Company Limited | Process for producing chlorine |
EP0761594A1 (en) * | 1995-09-12 | 1997-03-12 | Basf Aktiengesellschaft | Process for the production of chlorine from hydrogen chloride |
EP0761593A1 (en) * | 1995-09-12 | 1997-03-12 | Basf Aktiengesellschaft | Process for the production of chlorine |
EP0826417A1 (en) * | 1996-08-23 | 1998-03-04 | Basf Aktiengesellschaft | Bismuth containing catalysts |
WO2010112385A1 (en) * | 2009-03-30 | 2010-10-07 | Basf Se | Process for preparing chlorine |
CN112044440A (en) * | 2019-06-06 | 2020-12-08 | 中南大学 | Catalyst for preparing chlorine gas by catalytic oxidation of hydrogen chloride and preparation method and application thereof |
CN113135552A (en) * | 2020-01-19 | 2021-07-20 | 中南大学 | Method for preparing chlorine by catalytic oxidation of hydrogen chloride |
Citations (8)
Publication number | Priority date | Publication date | Assignee | Title |
---|---|---|---|---|
US2451870A (en) * | 1942-09-04 | 1948-10-19 | Standard Oil Dev Co | Chlorine manufacture |
US2577808A (en) * | 1947-02-12 | 1951-12-11 | Dow Chemical Co | Production of chlorine |
US3210158A (en) * | 1960-01-20 | 1965-10-05 | Shell Oil Co | Process for the production of chlorine |
US3260678A (en) * | 1961-01-17 | 1966-07-12 | Shell Oil Co | Catalyst composition, particularly for catalyzing oxidation of hydrogen chloride to chlorine |
US3542520A (en) * | 1967-12-27 | 1970-11-24 | Sun Oil Co | Modified "deacon" process |
US3561923A (en) * | 1963-06-26 | 1971-02-09 | Asahi Glass Co Ltd | Process for the production of chlorine |
US4803065A (en) * | 1986-06-30 | 1989-02-07 | Mitsui Toatsu Chemicals, Incorporated | Production process of chlorine |
US4959202A (en) * | 1989-05-31 | 1990-09-25 | Medalert Incorporated | Recovery of chlorine from hydrogen chloride by carrier catalyst process |
Family Cites Families (2)
Publication number | Priority date | Publication date | Assignee | Title |
---|---|---|---|---|
GB584790A (en) * | 1942-09-04 | 1947-01-23 | Standard Oil Dev Co | Improved process for the production of chlorine |
ES2010473A6 (en) * | 1989-03-06 | 1989-11-01 | Espan Carburos Metal | Recovery of chlorine from hydrogen chloride by means of a transport catalyst process |
-
1990
- 1990-10-26 AU AU67478/90A patent/AU6747890A/en not_active Abandoned
- 1990-10-26 AT AT90917325T patent/ATE123476T1/en active
- 1990-10-26 ES ES90917325T patent/ES2073041T3/en not_active Expired - Lifetime
- 1990-10-26 EP EP90917325A patent/EP0500728B1/en not_active Expired - Lifetime
- 1990-10-26 CA CA002072109A patent/CA2072109C/en not_active Expired - Fee Related
- 1990-10-26 WO PCT/US1990/006184 patent/WO1991006505A1/en active IP Right Grant
- 1990-10-26 DE DE69019981T patent/DE69019981T2/en not_active Expired - Fee Related
- 1990-11-02 PT PT95777A patent/PT95777A/en not_active Application Discontinuation
Patent Citations (8)
Publication number | Priority date | Publication date | Assignee | Title |
---|---|---|---|---|
US2451870A (en) * | 1942-09-04 | 1948-10-19 | Standard Oil Dev Co | Chlorine manufacture |
US2577808A (en) * | 1947-02-12 | 1951-12-11 | Dow Chemical Co | Production of chlorine |
US3210158A (en) * | 1960-01-20 | 1965-10-05 | Shell Oil Co | Process for the production of chlorine |
US3260678A (en) * | 1961-01-17 | 1966-07-12 | Shell Oil Co | Catalyst composition, particularly for catalyzing oxidation of hydrogen chloride to chlorine |
US3561923A (en) * | 1963-06-26 | 1971-02-09 | Asahi Glass Co Ltd | Process for the production of chlorine |
US3542520A (en) * | 1967-12-27 | 1970-11-24 | Sun Oil Co | Modified "deacon" process |
US4803065A (en) * | 1986-06-30 | 1989-02-07 | Mitsui Toatsu Chemicals, Incorporated | Production process of chlorine |
US4959202A (en) * | 1989-05-31 | 1990-09-25 | Medalert Incorporated | Recovery of chlorine from hydrogen chloride by carrier catalyst process |
Cited By (12)
Publication number | Priority date | Publication date | Assignee | Title |
---|---|---|---|---|
EP0743277A1 (en) * | 1995-05-18 | 1996-11-20 | Sumitomo Chemical Company Limited | Process for producing chlorine |
US5871707A (en) * | 1995-05-18 | 1999-02-16 | Sumitomo Chemical Company, Limited | Process for producing chlorine |
CN1077085C (en) * | 1995-05-18 | 2002-01-02 | 住友化学工业株式会社 | Process for producing chlorine |
EP0761594A1 (en) * | 1995-09-12 | 1997-03-12 | Basf Aktiengesellschaft | Process for the production of chlorine from hydrogen chloride |
EP0761593A1 (en) * | 1995-09-12 | 1997-03-12 | Basf Aktiengesellschaft | Process for the production of chlorine |
CN1075039C (en) * | 1995-09-12 | 2001-11-21 | 巴斯福股份公司 | Preparation of chlorine from hydrogen chloride |
EP0826417A1 (en) * | 1996-08-23 | 1998-03-04 | Basf Aktiengesellschaft | Bismuth containing catalysts |
US6197275B1 (en) | 1996-08-23 | 2001-03-06 | Basf Aktiengesellschaft | Bismuth-containing catalysts |
WO2010112385A1 (en) * | 2009-03-30 | 2010-10-07 | Basf Se | Process for preparing chlorine |
CN112044440A (en) * | 2019-06-06 | 2020-12-08 | 中南大学 | Catalyst for preparing chlorine gas by catalytic oxidation of hydrogen chloride and preparation method and application thereof |
CN112044440B (en) * | 2019-06-06 | 2021-09-10 | 中南大学 | Catalyst for preparing chlorine gas by catalytic oxidation of hydrogen chloride and preparation method and application thereof |
CN113135552A (en) * | 2020-01-19 | 2021-07-20 | 中南大学 | Method for preparing chlorine by catalytic oxidation of hydrogen chloride |
Also Published As
Publication number | Publication date |
---|---|
CA2072109C (en) | 2000-08-22 |
DE69019981D1 (en) | 1995-07-13 |
ES2073041T3 (en) | 1995-08-01 |
DE69019981T2 (en) | 1995-11-02 |
EP0500728A4 (en) | 1992-09-30 |
EP0500728B1 (en) | 1995-06-07 |
PT95777A (en) | 1991-09-13 |
AU6747890A (en) | 1991-05-31 |
EP0500728A1 (en) | 1992-09-02 |
ATE123476T1 (en) | 1995-06-15 |
CA2072109A1 (en) | 1991-05-03 |
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