EP0546152A1 - Catalysts for the production of carbon monoxide - Google Patents

Catalysts for the production of carbon monoxide

Info

Publication number
EP0546152A1
EP0546152A1 EP92914450A EP92914450A EP0546152A1 EP 0546152 A1 EP0546152 A1 EP 0546152A1 EP 92914450 A EP92914450 A EP 92914450A EP 92914450 A EP92914450 A EP 92914450A EP 0546152 A1 EP0546152 A1 EP 0546152A1
Authority
EP
European Patent Office
Prior art keywords
oxide
metal
group
catalyst
methane
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Withdrawn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
EP92914450A
Other languages
German (de)
French (fr)
Inventor
Ashok Kumar Depart. Of Engineering Bhattacharya
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.)
University of Warwick
Original Assignee
University of Warwick
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 GB919114323A external-priority patent/GB9114323D0/en
Priority claimed from GB919118163A external-priority patent/GB9118163D0/en
Application filed by University of Warwick filed Critical University of Warwick
Publication of EP0546152A1 publication Critical patent/EP0546152A1/en
Withdrawn legal-status Critical Current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
    • C01B3/00—Hydrogen; Gaseous mixtures containing hydrogen; Separation of hydrogen from mixtures containing it; Purification of hydrogen
    • C01B3/02—Production of hydrogen or of gaseous mixtures containing a substantial proportion of hydrogen
    • C01B3/32—Production of hydrogen or of gaseous mixtures containing a substantial proportion of hydrogen by reaction of gaseous or liquid organic compounds with gasifying agents, e.g. water, carbon dioxide, air
    • C01B3/34—Production of hydrogen or of gaseous mixtures containing a substantial proportion of hydrogen by reaction of gaseous or liquid organic compounds with gasifying agents, e.g. water, carbon dioxide, air by reaction of hydrocarbons with gasifying agents
    • C01B3/38—Production of hydrogen or of gaseous mixtures containing a substantial proportion of hydrogen by reaction of gaseous or liquid organic compounds with gasifying agents, e.g. water, carbon dioxide, air by reaction of hydrocarbons with gasifying agents using catalysts
    • C01B3/386—Catalytic partial combustion
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
    • C01B3/00—Hydrogen; Gaseous mixtures containing hydrogen; Separation of hydrogen from mixtures containing it; Purification of hydrogen
    • C01B3/02—Production of hydrogen or of gaseous mixtures containing a substantial proportion of hydrogen
    • C01B3/32—Production of hydrogen or of gaseous mixtures containing a substantial proportion of hydrogen by reaction of gaseous or liquid organic compounds with gasifying agents, e.g. water, carbon dioxide, air
    • C01B3/34—Production of hydrogen or of gaseous mixtures containing a substantial proportion of hydrogen by reaction of gaseous or liquid organic compounds with gasifying agents, e.g. water, carbon dioxide, air by reaction of hydrocarbons with gasifying agents
    • C01B3/38—Production of hydrogen or of gaseous mixtures containing a substantial proportion of hydrogen by reaction of gaseous or liquid organic compounds with gasifying agents, e.g. water, carbon dioxide, air by reaction of hydrocarbons with gasifying agents using catalysts
    • C01B3/40—Production of hydrogen or of gaseous mixtures containing a substantial proportion of hydrogen by reaction of gaseous or liquid organic compounds with gasifying agents, e.g. water, carbon dioxide, air by reaction of hydrocarbons with gasifying agents using catalysts characterised by the catalyst
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
    • C01B32/00—Carbon; Compounds thereof
    • C01B32/40—Carbon monoxide
    • C—CHEMISTRY; METALLURGY
    • C07—ORGANIC CHEMISTRY
    • C07C—ACYCLIC OR CARBOCYCLIC COMPOUNDS
    • C07C29/00—Preparation of compounds having hydroxy or O-metal groups bound to a carbon atom not belonging to a six-membered aromatic ring
    • C07C29/15—Preparation of compounds having hydroxy or O-metal groups bound to a carbon atom not belonging to a six-membered aromatic ring by reduction of oxides of carbon exclusively
    • C07C29/151—Preparation of compounds having hydroxy or O-metal groups bound to a carbon atom not belonging to a six-membered aromatic ring by reduction of oxides of carbon exclusively with hydrogen or hydrogen-containing gases
    • C07C29/1516—Multisteps
    • C07C29/1518—Multisteps one step being the formation of initial mixture of carbon oxides and hydrogen for synthesis
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
    • C01B2203/00—Integrated processes for the production of hydrogen or synthesis gas
    • C01B2203/10—Catalysts for performing the hydrogen forming reactions
    • C01B2203/1041—Composition of the catalyst
    • C01B2203/1047—Group VIII metal catalysts
    • C01B2203/1064—Platinum group metal catalysts
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
    • C01B2203/00—Integrated processes for the production of hydrogen or synthesis gas
    • C01B2203/10—Catalysts for performing the hydrogen forming reactions
    • C01B2203/1041—Composition of the catalyst
    • C01B2203/1082—Composition of support materials

Definitions

  • This invention concerns a process for the partial catalytic oxidation of methane to carbon monoxide and either hydrogen or steam or a mixture of hydrogen and steam.
  • Carbon monoxide is a very useful material for organic synthesis. Methane is widely available from natural gas deposits, but until now no practical
  • a method of oxidising methane to carbon monoxide and either hydrogen or steam or a mixture of hydrogen and steam comprises contacting oxygen and excess methane with a catalyst comprising a platinum group metal and/or metal oxide supported on a lanthanide oxide, and/or an oxide of a metal from group IIIA and/or an oxide from a metal from group IVA of the Periodic Table and/or alumina.
  • the platinum-group metal is preferably palladium, others are platinum, rhodium and iridium.
  • One preferred lanthanide oxide is cerium oxide
  • one preferred oxide of a metal from group IIIA of the Periodic Table is yttrium oxide
  • one preferred oxide of a metal from group IVA of the Periodic Table is zirconium oxide.
  • ABO3 where A is an alkaline earth metal and B is another metal such as Ti, Zr, Hf or Ce e.g. Ba may also be used, e.g. BaCeO 3 , SrCeO 3 , BaZrO 3 , SrZrO 3 and SrTiO 3 .
  • the reaction is preferably carried out at around 750°C. At temperatures of around 500-600°C a mixture of CO and CO 2 is obtained . At higher temperatures the proportion of CO increases and at lower temperatures the proportion of CO 2 increases. In the case of CeO 2 almost no CO 2 is produced at a temperature of 750°C. The proportion of hydrogen to steam produced increases with increasing temperature.
  • the palladium or other platinum group metal may preferably be deposited on an oxide as specified above and that metal oxide may, in turn, be coated onto any high surface area thermally-stable support, such as a ceramic material.
  • Fig.1 is a graph showing the amounts of CO and CO 2 obtained from the oxidation of CH 4 using Pd/CeO 2 and CeO 2 catalysts and various temperatures;
  • Fig.2 is a graph showing the percentages of CO and CO 2 at different space velocities using a Pd/CeO 2
  • a thin layer of palladium metal was deposited on a number of catalyst supports. This was done by treating the supports with palladium nitrate and decomposing it by heating to 550°C. The initial decomposition produces a mixture of palladium metal and oxide. This may be used as it is or may be reduced e.g. with hydrogen, to convert some or all of the oxide to the metal.
  • the Ceo 2 , Y 2 O 3 and Zr ⁇ 2 supports used were obtained commercially from
  • TiO 2 was purchased from Tioxide Ltd.
  • Al 2 O 3 was obtained commercially or prepared by standard preparative ceramic techniques or by the known hydroxide precipitation method.
  • the BaCeO 3 and SrCeO 3 were obtained by standard ceramic methods from commercially-available oxides (e.g. those supplied by Johnson Matthey pic) or from nitrates (also available from Johnson Matthey pic).
  • the resulting supported catalysts were then utilised to catalyse the reaction between excess methane and oxygen at 750°C.
  • SiO 2 was particularly unsatisfactory. The use of SiO 2 is outside the scope of this invention.
  • Fig. 1 is a graph comparing the yields of CO 2 and CO obtained by utilising a variety of supports at different temperatures.
  • Fig. 1 shows clearly that as the temperature approaches 750°C, the amounts of CO 2 and CO produced fall and rise respectively, for a supported Pd catalyst as specified in this invention (i.e. Pd/CeO 2 ).
  • Pd/CeO 2 a supported Pd catalyst as specified in this invention
  • the use of the CeO 2 support alone as catalyst is shown by way of comparison only.
  • a mixture of CO, CO 2 , H 2 O and H 2 is useful as such in the synthesis of methanol and other alcohols.
  • a process for the production of methanol comprises passing methane and oxygen over a catalyst as defined above at a temperature such that a mixture of CO, CO 2 , H 2 O, H 2 , and possibly unreacted CH 4 is obtained in
  • the oxygen may be supplied as air and the methane synthesis catalyst may be a commercially available one e.g. a copper oxide/zinc oxide/alumina catalyst, such as that available from ICI.
  • Fig. 2 shows that the conversion to CO rather than CO 2 is favoured by carrying out the reaction at higher space velocities.
  • the catalyst layer was obtained by the decomposition of palladium nitrate.
  • Other known methods can also be used (e.g. decomposition of palladium acetate or chloramines) involving different preparative techniques, and supports from different sources can also be employed having different physical properties.
  • the method of deposition and the exact nature of the support affect both the conversion and the selectivity of the catalyst.
  • Other factors which affect the performance of the catalyst are the space velocity (see Fig. 2),
  • methane:oxygen ratio the partial pressures of methane and oxygen in the gas being treated.

Landscapes

  • Chemical & Material Sciences (AREA)
  • Organic Chemistry (AREA)
  • Chemical Kinetics & Catalysis (AREA)
  • Engineering & Computer Science (AREA)
  • Combustion & Propulsion (AREA)
  • Inorganic Chemistry (AREA)
  • Health & Medical Sciences (AREA)
  • General Health & Medical Sciences (AREA)
  • Catalysts (AREA)

Abstract

Procédé d'oxydation partielle de méthane en monoxyde de carbone comprenant la mise en contact de l'oxygène et du métal en surplus avec un catalyseur comprenant un métal du groupe platine et/ou un oxyde de métal supporté sur un oxyde de lanthanide et/ou un oxyde d'un métal du groupe IIIA et/ou un oxyde d'un métal du groupe IVA du tableau périodique et/ou de l'oxyde d'aluminium. Le métal du groupe platine est, de préférence, du palladium, les autres sont du platine, du rhodium et de l'iridium. Un oxyde de lanthanide préféré est l'oxyde de cérium, un oxyde préféré d'un métal du groupe IIIA du tableau périodique est l'oxyde d'yttrium et un oxyde préféré d'un métal du groupe IVA du tableau périodique est l'oxyde de zirconium.Process for the partial oxidation of methane to carbon monoxide comprising bringing oxygen and excess metal into contact with a catalyst comprising a metal of the platinum group and / or a metal oxide supported on a lanthanide oxide and / or an oxide of a metal from group IIIA and / or an oxide of a metal from group IVA of the periodic table and / or aluminum oxide. The platinum group metal is preferably palladium, the others are platinum, rhodium and iridium. A preferred lanthanide oxide is cerium oxide, a preferred oxide of a metal from group IIIA of the periodic table is yttrium oxide and a preferred oxide of a metal from group IVA of the periodic table is oxide of zirconium.

Description

CATALYSTS FOR THE PRODUCTION OF CARBON MONOXIDE
This invention concerns a process for the partial catalytic oxidation of methane to carbon monoxide and either hydrogen or steam or a mixture of hydrogen and steam.
Carbon monoxide is a very useful material for organic synthesis. Methane is widely available from natural gas deposits, but until now no practical
catalytic method has been known for the partial oxidation of methane to carbon monoxide. Complete oxidation of methane of course yields carbon dioxide.
According to this invention, a method of oxidising methane to carbon monoxide and either hydrogen or steam or a mixture of hydrogen and steam comprises contacting oxygen and excess methane with a catalyst comprising a platinum group metal and/or metal oxide supported on a lanthanide oxide, and/or an oxide of a metal from group IIIA and/or an oxide from a metal from group IVA of the Periodic Table and/or alumina. The platinum-group metal is preferably palladium, others are platinum, rhodium and iridium. One preferred lanthanide oxide is cerium oxide, one preferred oxide of a metal from group IIIA of the Periodic Table is yttrium oxide and one preferred oxide of a metal from group IVA of the Periodic Table is zirconium oxide.
Mixed oxides of general formula ABO3 where A is an alkaline earth metal and B is another metal such as Ti, Zr, Hf or Ce e.g. Ba may also be used, e.g. BaCeO3, SrCeO3, BaZrO3, SrZrO3 and SrTiO3.
The reaction is preferably carried out at around 750°C. At temperatures of around 500-600°C a mixture of CO and CO2 is obtained . At higher temperatures the proportion of CO increases and at lower temperatures the proportion of CO2 increases. In the case of CeO2 almost no CO2 is produced at a temperature of 750°C. The proportion of hydrogen to steam produced increases with increasing temperature.
The palladium or other platinum group metal may preferably be deposited on an oxide as specified above and that metal oxide may, in turn, be coated onto any high surface area thermally-stable support, such as a ceramic material.
The invention will now be described in more detail by way of non-limiting example and with reference to the drawings, in which:
Fig.1 is a graph showing the amounts of CO and CO2 obtained from the oxidation of CH4 using Pd/CeO2 and CeO2 catalysts and various temperatures; and
Fig.2 is a graph showing the percentages of CO and CO2 at different space velocities using a Pd/CeO2
catalyst.
A thin layer of palladium metal was deposited on a number of catalyst supports. This was done by treating the supports with palladium nitrate and decomposing it by heating to 550°C. The initial decomposition produces a mixture of palladium metal and oxide. This may be used as it is or may be reduced e.g. with hydrogen, to convert some or all of the oxide to the metal. The Ceo2, Y2O3 and Zrθ2 supports used were obtained commercially from
Johnson Matthey pic. The TiO2was purchased from Tioxide Ltd. Al2O3 was obtained commercially or prepared by standard preparative ceramic techniques or by the known hydroxide precipitation method.
The BaCeO3 and SrCeO3 were obtained by standard ceramic methods from commercially-available oxides (e.g. those supplied by Johnson Matthey pic) or from nitrates (also available from Johnson Matthey pic).
The resulting supported catalysts were then utilised to catalyse the reaction between excess methane and oxygen at 750°C.
The following Table shows the percentage of methane converted in the reaction, when carried out at a
temperature of 750°C and a space velocity (GHSV) of 5000 hr using a feed gas comprising 45% CH4, 5% O2, 55% Av. The Table shows the percentage of both carbon monoxide and carbon dioxide in the converted proportion of
methane. Carbon dioxide is generally an undesired by-product of the reaction. The results show that cerium oxide, yttrium oxide and zirconium oxide were
particularly effective as catalyst supports in the production of carbon monoxide, giving both a reasonable percentage conversion, and very high selectively for CO vis-a-vis CO2. SiO2 on the other hand, was particularly unsatisfactory. The use of SiO2 is outside the scope of this invention.
Fig. 1 is a graph comparing the yields of CO2 and CO obtained by utilising a variety of supports at different temperatures.
Fig. 1 shows clearly that as the temperature approaches 750°C, the amounts of CO2 and CO produced fall and rise respectively, for a supported Pd catalyst as specified in this invention (i.e. Pd/CeO2). The use of the CeO2 support alone as catalyst is shown by way of comparison only.
A mixture of CO, CO2, H2O and H2 is useful as such in the synthesis of methanol and other alcohols.
Therefore, by careful selection of the catalyst and the temperature, a mixture of these four components can be obtained in such proportions that it may be used directly in alcohol synthesis.
Thus, according to another feature of the invention a process for the production of methanol comprises passing methane and oxygen over a catalyst as defined above at a temperature such that a mixture of CO, CO2, H2O, H2, and possibly unreacted CH4 is obtained in
appropriate proportions, and then passing said mixture over a methane synthesis catalyst.
The oxygen may be supplied as air and the methane synthesis catalyst may be a commercially available one e.g. a copper oxide/zinc oxide/alumina catalyst, such as that available from ICI.
Fig. 2 shows that the conversion to CO rather than CO2 is favoured by carrying out the reaction at higher space velocities.
As mentioned above, the catalyst layer was obtained by the decomposition of palladium nitrate. Other known methods can also be used (e.g. decomposition of palladium acetate or chloramines) involving different preparative techniques, and supports from different sources can also be employed having different physical properties. The method of deposition and the exact nature of the support affect both the conversion and the selectivity of the catalyst. Other factors which affect the performance of the catalyst are the space velocity (see Fig. 2),
methane:oxygen ratio, and the partial pressures of methane and oxygen in the gas being treated.

Claims

1. A method of oxidising methane to carbon monoxide and either hydrogen or steam or a mixture thereof
characterised in that it comprises contacting oxygen and excess methane with a catalyst comprising a platinum-group metal and/or metal oxide supported on a lanthanide oxide and/or an oxide of a metal from group IIIA and/or an oxide of a metal from group IVA of the Periodic Table and/or alumina.
2. A method as claimed in claim 1, wherein the platinum-group metal is selected from palladium, platinum, rhodium and iridium.
3. A method as claimed in claim 2, wherein the platinum-group metal is palladium.
4. A method as claimed in any one of claims 1 to 3, wherein the lanthanide oxide is cerium oxide.
5. A method as claimed in any one of claims 1 to 4, wherein the oxide of a metal from group IIIA of the
Periodic Table is yttrium oxide.
6. A method as claimed in any one of claims 1 to 5, wherein the metal from group IVA of the Periodic Table is zirconium oxide.
7. A method as claimed in claim 1, wherein the catalyst comprises a mixed oxide of general formula ABO3 where A is an alkaline earth metal and B is another metal.
8. A method as claimed in claim 7, wherein B is selected from titanium (Ti), zirconium (Zr), Hafnium (Hf) or cerium (Ce).
9. A method as claimed in any preceding claim, wherein the oxygen and methane is contacted with the catalyst at a temperature of 750ºC.
10. A catalyst for oxidising methane to carbon monoxide comprising the catalyst defined in any one of claims 1 to 8.
EP92914450A 1991-07-02 1992-07-02 Catalysts for the production of carbon monoxide Withdrawn EP0546152A1 (en)

Applications Claiming Priority (4)

Application Number Priority Date Filing Date Title
GB9114323 1991-07-02
GB919114323A GB9114323D0 (en) 1991-07-02 1991-07-02 Palladium catalyst for methane oxidation
GB9118163 1991-08-22
GB919118163A GB9118163D0 (en) 1991-08-22 1991-08-22 Palladium catalyst for methane oxidation

Publications (1)

Publication Number Publication Date
EP0546152A1 true EP0546152A1 (en) 1993-06-16

Family

ID=26299176

Family Applications (1)

Application Number Title Priority Date Filing Date
EP92914450A Withdrawn EP0546152A1 (en) 1991-07-02 1992-07-02 Catalysts for the production of carbon monoxide

Country Status (2)

Country Link
EP (1) EP0546152A1 (en)
WO (1) WO1993001130A1 (en)

Families Citing this family (17)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
IT1256227B (en) * 1992-12-23 1995-11-29 Snam Progetti CATALYTIC PROCEDURE FOR THE PRODUCTION OF SYNTHESIS GAS
EP0640561B1 (en) * 1993-08-24 1998-11-11 Shell Internationale Researchmaatschappij B.V. Process for the catalytic partial oxidation of hydrocarbons
MY131526A (en) * 1993-12-27 2007-08-30 Shell Int Research A process for the preparation of carbon monoxide and/or hydrogen
US5720901A (en) * 1993-12-27 1998-02-24 Shell Oil Company Process for the catalytic partial oxidation of hydrocarbons
US5753385A (en) * 1995-12-12 1998-05-19 Regents Of The University Of California Hybrid deposition of thin film solid oxide fuel cells and electrolyzers
US5753143A (en) * 1996-03-25 1998-05-19 Northwestern University Process for the CO2 reforming of methane in the presence of rhodium zeolites
ZA99313B (en) 1998-01-20 1999-07-19 Shell Int Research Catalyst suitable for the preparation of hydrogen and carbon monoxide from a hydrocarbonaceous feedstock
CA2368048A1 (en) * 1999-03-24 2000-09-28 Israel E. Wachs Production of formaldehyde from ch4 and h2s
US6458334B1 (en) * 2000-03-02 2002-10-01 The Boc Group, Inc. Catalytic partial oxidation of hydrocarbons
EP1134188A3 (en) * 2000-03-02 2004-06-09 The Boc Group, Inc. Catalytic partial oxidation of hydrocarbons
US20030007926A1 (en) * 2000-03-02 2003-01-09 Weibin Jiang Metal catalyst and method of preparation and use
WO2002020395A2 (en) 2000-09-05 2002-03-14 Conoco Inc. Lanthanide-promoted rhodium catalysts and process for producing synthesis gas
US7090826B2 (en) 2002-12-23 2006-08-15 The Boc Group, Inc. Monolith based catalytic partial oxidation process for syngas production
US7230035B2 (en) 2002-12-30 2007-06-12 Conocophillips Company Catalysts for the conversion of methane to synthesis gas
US7066984B2 (en) 2003-09-25 2006-06-27 The Boc Group, Inc. High recovery carbon monoxide production process
US7214331B2 (en) 2004-02-26 2007-05-08 The Boc Group, Inc. Catalyst configuration and methods for syngas production
US7351275B2 (en) 2004-12-21 2008-04-01 The Boc Group, Inc. Carbon monoxide production process

Family Cites Families (1)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
EP0291857A3 (en) * 1987-05-18 1990-07-18 Air Products And Chemicals, Inc. Method of carbon monoxide production

Non-Patent Citations (1)

* Cited by examiner, † Cited by third party
Title
See references of WO9301130A1 *

Also Published As

Publication number Publication date
WO1993001130A1 (en) 1993-01-21

Similar Documents

Publication Publication Date Title
EP0546152A1 (en) Catalysts for the production of carbon monoxide
US4743576A (en) Catalyst for the production of synthesis gas or hydrogen and process for the production of the catalyst
EP1222024B1 (en) Process for preparing synthesis gas employing a nickel-rhodium based catalysts
RU2115617C1 (en) Method of catalytic partial oxidation of hydrocarbon raw material
CA1294268C (en) Method of catalytic combustion using heat-resistant catalyst
US6702960B1 (en) Catalytic partial oxidation with a rhodium-iridium alloy catalyst
RU2123471C1 (en) Method of catalytic partial oxidation of hydrocarbons
US6312660B1 (en) Process for preparing synthesis gas
EP0640561B1 (en) Process for the catalytic partial oxidation of hydrocarbons
CA2048748A1 (en) Catalysts
JPH07196301A (en) Catalytic partial oxidation of hydrocarbon
CA2034674A1 (en) Catalytic system and process for producing synthesis gas by reforming light hydrocarbons with co2
JP2009297715A (en) Catalytic reduction and oxidation method
JP2001080907A (en) Method for preliminarily reforming oxygen-containing gas
Liu et al. Partial oxidation of ethane to syngas over nickel‐based catalysts modified by alkali metal oxide and rare earth metal oxide
JP2002500952A (en) Catalyst suitable for producing hydrogen and carbon monoxide from hydrocarbon feedstocks
JPH09196306A (en) Catalytic combustion by stepwise injection of fuel
CA2050143A1 (en) Catalytic process for the production of synthetic gas by means of hydrocarbon reforming and combustion reactions
AU671232B2 (en) Process for the catalytic partial oxidation of hydrocarbons
EP0537862A1 (en) Catalyst and process for the catalytic partial oxidation of hydrocarbons
JP4143352B2 (en) Catalyst for oxidizing methane in exhaust gas and method for oxidizing and removing methane in exhaust gas
EP0629146B1 (en) Oxidation catalysts
JP2664997B2 (en) Methanol reforming method
JP2001232198A (en) Catalyst and manufacturing method of catalyst
US5567667A (en) Oxidation catalysts

Legal Events

Date Code Title Description
PUAI Public reference made under article 153(3) epc to a published international application that has entered the european phase

Free format text: ORIGINAL CODE: 0009012

17P Request for examination filed

Effective date: 19930327

AK Designated contracting states

Kind code of ref document: A1

Designated state(s): BE DE DK FR GB NL SE

STAA Information on the status of an ep patent application or granted ep patent

Free format text: STATUS: THE APPLICATION HAS BEEN WITHDRAWN

18W Application withdrawn

Withdrawal date: 19940618