EP1257497A2 - Catalyseur a base de chrome et procedes de conversion d'hydrocarbures en gaz de synthese - Google Patents

Catalyseur a base de chrome et procedes de conversion d'hydrocarbures en gaz de synthese

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Publication number
EP1257497A2
EP1257497A2 EP01910791A EP01910791A EP1257497A2 EP 1257497 A2 EP1257497 A2 EP 1257497A2 EP 01910791 A EP01910791 A EP 01910791A EP 01910791 A EP01910791 A EP 01910791A EP 1257497 A2 EP1257497 A2 EP 1257497A2
Authority
EP
European Patent Office
Prior art keywords
metal
composition
chromium
gas mixture
catalyst
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Withdrawn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
EP01910791A
Other languages
German (de)
English (en)
Inventor
Kostantinos Kourtakis
Anne M. Gaffney
Lin Wang
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.)
ConocoPhillips Co
Original Assignee
Conoco Inc
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 Conoco Inc filed Critical Conoco Inc
Publication of EP1257497A2 publication Critical patent/EP1257497A2/fr
Withdrawn legal-status Critical Current

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    • 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
    • B01J37/03—Precipitation; Co-precipitation
    • B01J37/031—Precipitation
    • B01J37/033—Using Hydrolysis
    • 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
    • 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
    • B01J23/26—Chromium
    • 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
    • B01J23/34—Manganese
    • 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
    • B01J23/68—Silver or gold with arsenic, antimony, bismuth, vanadium, niobium, tantalum, polonium, chromium, molybdenum, tungsten, manganese, technetium or rhenium
    • B01J23/683—Silver or gold with arsenic, antimony, bismuth, vanadium, niobium, tantalum, polonium, chromium, molybdenum, tungsten, manganese, technetium or rhenium with chromium, molybdenum or tungsten
    • B01J23/685—Silver or gold with arsenic, antimony, bismuth, vanadium, niobium, tantalum, polonium, chromium, molybdenum, tungsten, manganese, technetium or rhenium with chromium, molybdenum or tungsten with chromium
    • 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
    • B01J23/84—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 arsenic, antimony, bismuth, vanadium, niobium, tantalum, polonium, chromium, molybdenum, tungsten, manganese, technetium or rhenium
    • B01J23/85—Chromium, molybdenum or tungsten
    • B01J23/86—Chromium
    • 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
    • B01J23/84—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 arsenic, antimony, bismuth, vanadium, niobium, tantalum, polonium, chromium, molybdenum, tungsten, manganese, technetium or rhenium
    • B01J23/85—Chromium, molybdenum or tungsten
    • B01J23/86—Chromium
    • B01J23/864—Cobalt and chromium
    • 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
    • B01J23/84—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 arsenic, antimony, bismuth, vanadium, niobium, tantalum, polonium, chromium, molybdenum, tungsten, manganese, technetium or rhenium
    • B01J23/85—Chromium, molybdenum or tungsten
    • B01J23/86—Chromium
    • B01J23/866—Nickel and chromium
    • 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
    • B01J37/32—Freeze drying, i.e. lyophilisation
    • 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
    • C01B2203/00—Integrated processes for the production of hydrogen or synthesis gas
    • C01B2203/02—Processes for making hydrogen or synthesis gas
    • C01B2203/025—Processes for making hydrogen or synthesis gas containing a partial oxidation step
    • C01B2203/0261—Processes for making hydrogen or synthesis gas containing a partial oxidation step containing a catalytic partial oxidation step [CPO]
    • 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
    • C01B2203/1005—Arrangement or shape of catalyst
    • C01B2203/1023—Catalysts in the form of a monolith or honeycomb
    • 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
    • C01B2203/1005—Arrangement or shape of catalyst
    • C01B2203/1029—Catalysts in the form of a foam
    • 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
    • C—CHEMISTRY; METALLURGY
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    • 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
    • C01B2203/1052—Nickel or cobalt catalysts
    • C—CHEMISTRY; METALLURGY
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    • 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
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    • 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
    • C01B2203/1076—Copper or zinc-based catalysts
    • C—CHEMISTRY; METALLURGY
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    • 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
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    • 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
    • C01B2203/1094—Promotors or activators
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    • C01B2203/00—Integrated processes for the production of hydrogen or synthesis gas
    • C01B2203/12—Feeding the process for making hydrogen or synthesis gas
    • C01B2203/1205—Composition of the feed
    • C01B2203/1211—Organic compounds or organic mixtures used in the process for making hydrogen or synthesis gas
    • C01B2203/1235—Hydrocarbons
    • C01B2203/1241—Natural gas or methane
    • Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
    • Y02—TECHNOLOGIES OR APPLICATIONS FOR MITIGATION OR ADAPTATION AGAINST CLIMATE CHANGE
    • Y02P—CLIMATE CHANGE MITIGATION TECHNOLOGIES IN THE PRODUCTION OR PROCESSING OF GOODS
    • Y02P20/00—Technologies relating to chemical industry
    • Y02P20/50—Improvements relating to the production of bulk chemicals
    • Y02P20/52—Improvements relating to the production of bulk chemicals using catalysts, e.g. selective catalysts

Definitions

  • the present invention relates to catalysts and processes for the catalytic conversion of hydrocarbons (e.g., natural gas) using chromium-based catalysts to produce carbon monoxide and hydrogen. More particularly, the invention relates to such catalysts and their manner of making, and to processes employing the catalysts. Description of Related Art
  • methane as a starting material for the production of higher hydrocarbons and hydrocarbon liquids.
  • the conversion of methane to hydrocarbons is typically carried out in two steps. In the first step, methane is reformed with water to produce carbon monoxide and hydrogen (i.e., synthesis gas or "syngas"). In a second step, the syngas is converted to hydrocarbons, for example, using the Fischer-Tropsch process to provide fuels that boil in the middle distillate range, such as kerosene and diesel fuel, and hydrocarbon waxes.
  • the syngas in turn may be converted to hydrocarbon products, for example, fuels boiling in the middle distillate range, such as kerosene and diesel fuel, and hydrocarbon waxes by processes such as the Fischer-Tropsch Synthesis.
  • hydrocarbon products for example, fuels boiling in the middle distillate range, such as kerosene and diesel fuel, and hydrocarbon waxes by processes such as the Fischer-Tropsch Synthesis.
  • the selectivities of catalytic partial oxidation to the desired products, carbon monoxide and hydrogen, are controlled by several factors, but one of the most important of these factors is the choice of catalyst composition. Difficulties have arisen in the prior art in making such a choice economical. Typically, catalyst compositions have included precious metals and/or rare earths. The large volumes of expensive catalysts needed by prior art catalytic partial oxidation processes have placed these processes generally outside the limits of economic justification. For successful operation at commercial scale, the catalytic partial oxidation process must be able to achieve a high conversion of the methane feedstock at high gas hourly space velocities, and the selectivity of the process to the desired products of carbon monoxide and hydrogen must be high.
  • U.S. Pat. No. 5,149.516 discloses a process for the partial oxidation of methane comprising contacting methane and a source of oxygen with a perovskite of the formula ABO 3 , where B can be a variety of metals including Cr.
  • the perovskite that was used is LaCoO 3 .
  • U.S. Pat. No. 5,447.705 also discloses a process for the partial oxidation of methane to syngas by contacting the starting materials with a catalyst having a perovskite crystalline structure and having the composition Ln x A ⁇ .
  • y B y O 3 in which x is a number such that 0 ⁇ x ⁇ 10, y is a number such that 0 ⁇ y ⁇ l, Ln is at least one of a rare earth, strontium or bismuth, A is a metal of groups IVb, Vb, VIb, Vllb or VIII, A is a metal of groups IVb, Vb, VIb, Vllb or VIII and A and B are two different metals.
  • Various combinations of La, Ni and Fe were exemplified.
  • U.S. Pat. No. 5,149,464 discloses a method for selectively converting methane to syngas at 650°C to 950°C by contacting the methane/oxygen mixture with a solid catalyst, which is either: (a) a catalyst of the formula M x M' y O z where: M is at least one element selected from Mg, B.
  • Ln is at least one member of lanthanum and the lanthanide series of elements
  • M' is a d-block transition metal, and each of the ratios x/z and y/z and (x+y)/z is independently from 0.1 to 8; or (b) an oxide of a d- block transition metal; or (c) a d-block transition metal on a refractory support ; or (d) a catalyst formed by heating a) or b) under the conditions of the reaction or under non- oxidizing conditions.
  • the d-block transition metals are selected from those having atomic number 21 to 29, 40 to 47 and 72 to 79, the metals Sc, Ti, Va, Cr, Mn, Fe, Co, Ni, Cu, Zr, Nb, Mo, Tc, Ru, Rh, Pa, Ag, Hf, Ta, W, Re, Os, Ir, Pt and Au.
  • M' is selected from Fe, Os, Co, Rh, Ir, Pd, Pt and particularly Ni and Ru.
  • U.S. Pat. No. 5,431,855 describes a catalyst which catalyzes the combined partial oxidation-dry reforming reaction of a reactant gas mixture comprising CO 2 , O 2 and CH to for a product gas mixture comprising CO and H 2 .
  • Related patent U.S. Pat. No. 5,500,149 describes similar catalysts and methods for production of product gas mixtures comprising
  • U.S. Pat. No. 2,942,958 discloses an improved method for converting methane to carbon monoxide and hydrogen employing a reforming catalyst for the steam-methane reaction. Although it is stated that any reforming catalyst is suitable for the process, the preferred catalysts are nickel, chromium and cobalt, or their oxides.
  • U.S. Pat. No. 4,843,181 discloses a process for preparing Cr 2 ⁇ 3 that includes pyrolysis of ammonium dichromate.
  • the chromium oxide is employed in a process for manufacturing 1,1,1-trifluorodichloroethane and 1,1,1,2-tetrafluorochloroethane.
  • U.S. Pat. No. 5,036,036 discloses an improved Cr 2 O 3 catalyst composition, prepared by pyrolysis of ammonium dichromate, which is useful in hydrofluorination reactions.
  • EP303438 entitled "Production of Methanol from Hydrocarbonaceous Feedstock.”
  • the asserted advantages of EP303438 are relatively independent of catalyst composition, i.e., "partial oxidation reactions will be mass transfer controlled. Consequently, the reaction rate is relatively independent of catalyst activity, but dependent on surface area-to-volume ratio of the catalyst.”
  • a monolith catalyst is used with or without metal addition to the surface of the monolith at space velocities of 20,000-500,000 hr " l.
  • the suggested metal coatings of the monolith are selected from the exemplary list of palladium, platinum, rhodium, iridium, osmium, ruthenium, nickel, chromium, cobalt, cerium, lanthanum, and mixtures thereof in addition to metals of the groups IA, IIA, III, IV, VB, VIB, or VIIB.
  • An exemplary catalyst comprises alumina on cordierite, with a coating comprising platinum and palladium. Steam is required in the feed mixture to suppress coke formation on the catalyst. Products from the partial oxidation of methane employing these catalysts results in the production of significant quantities of carbon dioxide, steam, and C 2 + hydrocarbons.
  • the preferred chromium-based catalysts provide higher levels of activity (i.e., conversion of CH ) and high selectivity to CO and H 2 reaction products than is typically available with conventional catalytic systems designed for commercial-scale use.
  • Another advantage of the catalytic compositions and syngas production processes of the invention is that no appreciable coking occurs with use of many of the chromium-containing catalyst compositions.
  • Still another advantage of the new catalysts and processes is that they are more economically feasible for use in commercial-scale conditions than conventional catalysts now used for producing syngas.
  • a process for the catalytic conversion of a hydrocarbon feedstock to syngas is provided. Conversion of the hydrocarbon is achieved by contacting a feed stream comprising the hydrocarbon feedstock and an oxygen-containing gas with a chromium-based catalyst in a reaction zone maintained at conversion-promoting conditions effective to produce an effluent stream comprising carbon monoxide and hydrogen.
  • catalyst compositions comprising a chromium-containing compound optionally combined with at least one metal selected from the group consisting of Group 1 , Group 2, Group 11 and Group 12 of the periodic table of the elements; a metal with an atomic number of 57 through 71; Co, Ru, Rh, Pd, Ir, Pt, Al, Ti, Y and Zr, and optionally Si.
  • the preferred compositions do not have a perovskite structure.
  • Yet another aspect of the present invention includes methods of making the new chromium-based catalytic compositions.
  • chromium-based catalysts exhibit high methane oxidation activities and selectivities to syngas (CO and H 2 ) in a millisecond contact time reactor.
  • the low light-off temperatures of these materials i.e., less than 650°C
  • superior performance are indicative of the more preferred catalytic compositions.
  • Pure chromium oxide catalysts, and chromium catalysts containing rare earth oxides show little or no carbon or coke build-up after reaction with CHVO . Trends in light-off temperature appear to correlate with the basicity or ionicity of the rare earth components, which may, in turn, relate to trends in C-H activation.
  • Chromium oxide- based catalysts containing cobalt show carbon deposition on the reduced cobalt metal particles which are formed in situ.
  • a chromium- based composition for catalyzing the conversion of a C 1 -C 5 hydrocarbon to form a product gas mixture containing CO and H 2 is provided.
  • the composition comprises about 0.1- 100 mole % of chromium or chromium-containing compound per total moles of metal or metal ion in the composition.
  • the composition also includes at least one other elemental metal or metal-containing compound, the metal of which is Li, Na, K, Rb, Cs, Mg, Ca, Sr, Ba, Cu, Ag, Au, Zn, Cd, La, Ce, Pr, Nd, Sm, Eu, Gd, Tb, Dy, Ho, Er, Tm, Yb, Lu, Co, Ni, Ru or Rh.
  • the composition may also contain an oxidatively and thermally stable porous support.
  • the chromium-based composition does not have a perovskite structure.
  • the porous material may include at least one oxide or oxyhydroxide of a metal such as magnesium, silicon, titanium, tantalum, zirconium or aluminum.
  • the chromium or chromium- containing compound comprises about 10-100 mole % of the total moles of metal or metal ion in said composition.
  • the catalyst composition initially comprises a catalyst precursor comprising a mixed metal oxide, and after reaction in a syngas reactor, the catalyst finally comprises reduced metal and metal oxide.
  • the catalyst precursor comprises CoCr 2 O 4
  • the reduced metal is zero valent cobalt metal
  • the metal oxide is Cr 2 O 3 .
  • the composition comprises a matrix structure which is a xerogel or an aerogel.
  • the matrix structure comprises at least one oxide or oxyhydroxide of a metal such as magnesium, silicon, titanium, tantalum, zirconium or aluminum.
  • Certain chromium-based compositions of the invention have a matrix structure comprising at least 30 wt %, preferably about 30-99.9 mole %, and more preferably about 50-97.5 mole % of the total moles (of metal) of the composition.
  • the matrix structure comprises titanium oxide/oxyhydroxide, or magnesium oxide/oxyhydroxide and silicon oxide/oxyhydroxide.
  • the chromium-based composition also contains cobalt or a cobalt-containing compound.
  • the composition also includes lanthanum or a lanthanum- containing compound.
  • Certain catalytic chromium-based compositions contain magnesium or a magnesium-containing compound and silicon oxide/oxyhydroxide.
  • the chromium-based composition contains cerium or samarium, or compounds containing those metals.
  • gold and aluminum oxide/oxyhydroxide in addition to chromium or a chromium- containing compound.
  • the chromium-based catalytic composition comprises gold or a gold-containing compound and magnesium oxide/oxyhydroxide.
  • Still other embodiments contain lanthanum and lithium, or compounds containing those elements, and ⁇ -Al 2 O 3 , in addition to chromium or a chromium-containing compound.
  • chromium-based catalytic compositions comprise a catalyst support, which may be oxidatively and thermally stable.
  • the catalyst support may also be in the form of a porous three-dimensional monolith or it could be a reticulated ceramic or ceramic foam.
  • a process in provided for preparing a chromium-based composition for catalyzing the partial oxidation of a C 1 -C 5 hydrocarbon to form a product gas mixture comprising CO and H 2 comprises combining about 0.1-100 mole % elemental chromium or chromium-containing compound per total moles of metal in the composition, together with, optionally, at least one other metal or metal oxide the metal component of which is Li, Na, K, Rb, Cs, Mg, Ca, Sr, Ba, Cu, Ag, Au, Zn, Cd, La, Ce, Pr, Nd, Sm, Eu, Gd, Tb, Dy, Ho, Er.
  • the composition also contains at least one matrix-forming material such as an alkoxide of magnesium, silicon, titanium, tantalum, zirconium or aluminum.
  • the process also includes forming the combination into a porous solid.
  • the matrix-forming material may be at least 30 wt % of the total weight of said composition with said chromium compound and said at least one other metal compound.
  • the matrix-forming material comprises titanium or titanium oxide, or a combination of oxides or alkoxides of magnesium and silicon.
  • the process also includes preparing an intermediate composition containing the chromium or chromium-containing compound and at least one other metal or metal-containing compound.
  • the process includes applying the intermediate composition to a porous matrix material comprising at least 30 wt % of the total weight of the composition.
  • the porous matrix material may comprise a porous monolith support and the intermediate composition may be in the form of a liquid which is applied to the porous matrix material by impregnation.
  • the intermediate composition is dried, or calcined. Certain embodiments of the process provide for calcining the composition in situ under reaction conditions.
  • the composition is formed by freeze-drying, spray drying or spray roasting the intermediate composition.
  • a powder is formed, which may be compressed into a pellet.
  • Other embodiments of the process for making a chromium- based catalyst composition include forming an extrudate, or a gel such as a xerogel or aerogel.
  • the process of making a chromium-based catalytic composition employs a matrix-forming material comprising at least one metal alkoxide.
  • the metal alkoxide may contain 1 to 20 carbon atoms, and in some embodiments contains 1 to 5 carbon atoms.
  • Some embodiments combine with the chromium or chromium- containing compound at least one metal alkoxide that is a C ] -C 4 alkoxide such as tantalum n-butoxide, titanium isopropoxide or zirconium isopropoxide.
  • the process includes dissolving at least one of the metal alkoxides in a non-aqueous medium to form a metal alkoxide solution.
  • the metal alkoxide solution is mixed with a protic solvent, such as water, whereby the alkoxide(s) react(s) with the protic solvent to form a gel.
  • a protic solvent such as water
  • the process may include dissolving or suspending the matrix material in the non-aqueous liquid medium to form a non-aqueous matrix solution or colloidal suspension.
  • the process may include dissolving at least one other elemental metal or metal-containing compound and one or more matrix-forming component in a non-aqueous medium.
  • Certain embodiments of the process for making a chromium-based catalytic composition provide for combining a protic solvent and an alkoxide in a molar ratio of about 5:1 to 53.1 or about 26.5:1.
  • the process may include the gradual addition and mixing of sufficient protic solution to induce hydrolysis and condensation of the metal alkoxide(s).
  • the mixing comprises combining water and the alkoxide in a molar ratio of about 0.1 :1 to 10:1 water:alkoxide.
  • Some embodiments include combining water and zirconium alkoxide or titanium alkoxide in a molar ratio of about 4: 1.
  • processes are provided for converting a C ⁇ -C 5 hydrocarbon to form a product gas mixture containing CO and H .
  • the process comprises mixing a C 1 -C 5 hydrocarbon- containing feedstock and an oxygen-containing feedstock to provide a reactant gas mixture.
  • the process includes contacting said reactant gas mixture with a catalytically effective amount of one of the above-described chromium-based catalyst compositions.
  • the composition and the reactant gas mixture are maintained at a temperature of about 600-l,100°C or about 700-l,000°C.
  • the catalyst composition/reactant gas system is also maintained at a pressure of about 100- 12,500 kPa, preferably about 130-10,000 kPa, and the reactant gas mixture is passed over the catalyst composition at a continuous flow rate of about 20,000 to about 100,000,000 NL/kg/h, preferably about 50,000 - 50,000,000 NL/kg/h.
  • the reactant gas/catalyst composition contact time is 10 milliseconds or less.
  • Some embodiments of the syngas manufacturing process include mixing a methane- containing gas feedstock and an oxygen-containing gas feedstock to provide a reactant gas mixture having a carbo oxygen ratio of about 1.25:1 to about 3.3:1, or about 1.3:1 to about 2.2:1, or about 1.5:1 to about 2.2:1, preferably about 2:1.
  • the oxygen- containing gas further comprises steam, CO 2 , or a combination thereof.
  • the process comprises mixing a hydrocarbon feedstock and a gas comprising steam and/or CO 2 to provide a reactant gas mixture.
  • the C 1 -C 5 hydrocarbon comprises at least about 50 % methane by volume of the reactant gas mixture, preferably at least about 75 %, and more preferably at least about 80 % methane by volume of the reactant gas mixture.
  • Certain embodiments of the processes of making syngas provide for preheating the hydrocarbon feedstock and/or the oxygen-containing feedstock before contacting the catalyst composition.
  • the reactant gases are preheated to temperatures up to about 700°C.
  • the catalyst composition is in a fixed bed reaction zone.
  • One embodiment of the process of converting a hydrocarbon to methane and hydrogen employs a particularly highly active and selective catalyst system.
  • This process includes mixing a C]-C hydrocarbon-containing feedstock and an oxygen-containing feedstock to provide a reactant gas mixture.
  • the reactant gas mixture is contacted with a catalytically effective amount of a CoCr 2 O 4 cubic spinel precursor dispersed in a chromium oxide matrix.
  • the catalyst composition and the reactant gas mixture are maintained at a temperature of about 600-l,100°C. and at a pressure of about 100-12,500 kPa.
  • the reactant gas mixture is passed over the catalyst composition at a continuous flow rate of about 20,000 to about 100,000,000 NL/kg/h.
  • At least a portion of the catalyst precursor is reduced to cobalt metal (in a chromium oxide matrix) by the heated gases of the reactant stream.
  • Certain embodiments provide a process for converting a C 1 -C 5 hydrocarbon that contains at least about 80 vol% methane to form a product gas mixture comprising CO and
  • This process may include mixing a methane-containing gaseous feedstock and an oxygen-containing gaseous feedstock to provide a reactant gas mixture having a carbomoxygen ratio of about 1.25:1 to about 3.3:1.
  • the gaseous feedstocks are preheated and combined, and the reactant gas mixture is then contacted with a catalytically effective amount of a chromium-based composition containing about 10-100 mole % (as the metal) chromium or chromium-containing compound per total moles of metal or metal ion in the catalyst composition.
  • the catalyst composition also contains 0-90% cobalt or cobalt- containing compound, and optionally, an oxidatively and thermally stable porous support supporting the chromium or chromium-containing compound and the cobalt or cobalt- containing compound.
  • the catalyst composition comprises a structure other than a perovskite structure.
  • the reactant gas mixture is passed over the catalytic composition at a continuous flow rate of about 20,000 to 100,000,000 NL/kg/h, preferably ensuring a reactant gas/catalyst composition contact time of no more than about 10 milliseconds.
  • the catalytic composition is nominally 0.8 mole % in elemental chromium or chromium ion and 0.2 mole % in elemental cobalt or cobalt ion.
  • the composition is nominally 0.2 mole % in elemental chromium or chromium ion and 0.8 mole % in elemental cobalt or cobalt ion.
  • the composition is nominally 0.5 mole % in elemental chromium or chromium ion and 0.5 mole % in elemental cobalt or cobalt ion.
  • Certain embodiments of the processes for converting a hydrocarbon to yield CO and H 2 employ a catalytic composition that is nominally 2-10 mole % chromium or chromium ion, 1 mole % in lithium or lithium ion and 27 mole % lanthanum or lanthanum ion and also includes an alpha-alumina support. Such processes preferably provide at least 90% conversion of CH and at least 90% selectivities for CO and H 2 products.
  • Other embodiments, features and advantages of the present invention will become apparent with reference to the following figures and description.
  • Fig. 1 is a bar graph comparing the catalyst performance of three pure chromium oxide systems. The black bars indicate the % CH 4 conversion and the cross-hatched bars indicate the % CO selectivity.
  • Fig. 2A is a transmission electron microscopy photomicrograph showing the crystal structure of a representative freeze-dried chromium oxide catalyst as prepared.
  • Fig. 2B is similar to Fig. 2A but was taken after the catalyst was employed 6 hours on stream.
  • Fig. 3 is a graph showing trends in light-off temperature and basicity/ionicity of representative "support' " matrix compositions.
  • Fig. 4 is a graph showing the results of thermal gravimetric analysis (TGA) studies of a representative rare earth oxide based chromium catalyst.
  • Fig. 5 is a graph showing the reaction chemistry for several representative ternary freeze dried chromium oxides containing chromium and cobalt.
  • Fig. 6A is X-ray diffraction data for the catalyst precursor CoQ ⁇ CrQ gOx following reaction in situ (i.e., on stream).
  • Fig. 6B is like Fig. 6A, except the catalyst specimen was taken before reactor evaluation.
  • Fig. 7 A shows the X-ray diffraction data for COQ 2C ⁇ Q ⁇ Ox after reactor evaluation.
  • Fig. 7 B shows the X-ray diffraction data for COQ.5 Cro.8 ⁇ x after reactor evaluation
  • Fig. 7 C shows the X-ray diffraction data for COQ.8 after reactor evaluation.
  • the chromium-containing catalysts useful for catalyzing the partial oxidation of methane to CO and H 2 are prepared by employing a variety of known art techniques such as impregnation, xerogel or aerogel formation, freeze-drying, spray drying, and spray roasting.
  • monoliths can be used as supports provided that they have sufficient porosity for reactor use.
  • the supports used with some of the catalyst compositions may be in the form of monolithic supports or other configurations having longitudinal channels or passageways permitting high space velocities with a minimal pressure drop. Such configurations are known in the art and described in, for example, Structured Catalysts and Reactors, A. Cybulski and J.A.
  • the impregnation techniques preferably comprise contacting the support with a solution of a compound of the catalytically active material, or a solution of compounds of the catalytically active materials or their precursors. The contacting is followed by drying and calcining, or transforming or thermally treating the supported materials under reaction conditions; in some cases this thermal treatment can be accomplished in situ under reaction conditions.
  • a key component of the most preferred catalysts is chromium, and optionally at least one other metal selected from the group consisting of Group 1 (i.e., Li, Na, K, Rb and Cs); Group 2 (i.e., Mg, Ca, Sr and Ba); Group 11 (i.e., Cu, Ag and Au); Group 12 (i.e., Zn and Cd); metals with atomic numbers of 57 through 71 (i.e., La, Ce, Pr, Nd, Sm, Eu, Gd, Tb, Dy, Ho, Er, Tm, Yb and Lu), Co, Ni, Ru and Rh.
  • the catalyst, or catalytic composition must contain a catalytically effective amount of the metal component(s).
  • the amount of catalytic metal present in the composition may vary widely.
  • the catalyst comprises from about 0.1 mole % to about 100 mole % (as the metal) of chromium per total moles of catalytic metal and matrix metal, and more preferably from about 10 mole % to about 100 mole %.
  • a matrix is a skeletal framework of oxides and oxyhydroxides.
  • One or more of the catalytic components may also serve as a matrix material in which another catalytic metal or metal-containing compound is dispersed.
  • a catalyst composition may include a CoCr 2 O 4 cubic spinel catalyst precursor dispersed in a chromium oxide matrix.
  • This catalyst precursor is then reduced to cobalt metal in a chromium oxide matrix by the hot gases of the reactant stream.
  • a suitable matrix can also be obtained from the hydrolysis and condensation of alkoxides and/or other reagents.
  • an oxidatively and thermally stable material may serve as a matrix or a support for the catalyst composition.
  • a composition containing (in wt%) 10% Cr, 1% Li, 27% La and -Al 2 O 3 may be used.
  • Xerogels and Aerogels from Metal Alkoxides For the purposes of this disclosure, the term "gel” refers to a coherent, rigid three- dimensional polymeric network.
  • the present gels are formed in a liquid medium, usually water, alcohol, or a mixture thereof.
  • a liquid medium usually water, alcohol, or a mixture thereof.
  • alcogel refers to gels in which the pores are filled with predominantly alcohol. Gels whose pores are filled primarily with water may be referred to as aquagels or hydrogels.
  • a "xerogel” is a gel from which the liquid medium has been removed and replaced by a gas. In general, the structure is compressed and the porosity reduced significantly by the surface tension forces that occur as the liquid is removed. As soon as liquid begins to evaporate from a gel at temperatures below the critical temperature, surface tension creates concave menisci in the gel's pores.
  • an "aerogel” is a gel from which the liquid has been removed in such a way as to prevent significant collapse or change in the structure as liquid is removed.
  • the new xerogels or aerogels preferably comprise a matrix material that is essentially derived from a solution of one or more matrix components and incorporate the active catalyst component(s).
  • the active catalyst components are preferably derived from one or more dissolved component.
  • the matrix is a skeletal framework of oxides and oxyhydroxides derived from the hydrolysis and condensation of alkoxides and/or other reagents. This framework preferably comprises 30% or more, by weight, of the total catalyst composition.
  • the matrix material comprises magnesium, silicon, titanium, zirconium or aluminum, oxide/hydroxide xerogels or aerogels, or mixtures thereof, totaling from 30 to 99.9 mole %, preferably 50-97.5 mole% of the catalyst composition.
  • Especially preferred are combinations where the matrix metal is Ti and combinations where the matrix metal is a combination of Mg and Si.
  • one or more metal alkoxides may be used as starting material for preparing the gels.
  • Suitable metal alkoxides are any alkoxide that contains from 1 to 20 carbon atoms, preferably 1 to 5 carbon atoms, in the alkoxide group. It is also prefe ⁇ ed that the alkoxide is soluble in the liquid reaction medium.
  • C1-C 4 alkoxides such as tantalum n-butoxide, titanium isopropoxide and zirconium isopropoxide are especially preferred.
  • Commercially available alkoxides can be used, if desired.
  • suitable alkoxides can be prepared by other routes.
  • Some examples include direct reaction of zero valent metals with alcohols in the presence of a catalyst.
  • Many alkoxides can be formed by reaction of metal halides with alcohols.
  • Alkoxy derivatives can be synthesized by the reaction of the alkoxide with alcohol in a ligand interchange reaction.
  • Direct reactions of metal dialkylamides with alcohol also form alkoxide derivatives. Additional examples are disclosed in "Metal Alkoxides '" by D.C. Bradley et al.. Academic Press, (1978).
  • the first step in the synthesis of the gels containing alcohol, or alcogels consists of first preparing non-aqueous solutions of the alkoxides and other reagents and separate solutions containing protic solvents such as water. When the alkoxide solutions are mixed with the solutions containing the protic solvents, the alkoxides will react and polymerize to form a gel.
  • the medium utilized in the process generally should be a solvent for the alkoxide or alkoxides which are utilized and the additional metal reagents and promoters which are added in the single step synthesis. Solubility of all components in their respective media (aqueous and non-aqueous) is prefe ⁇ ed to produce highly dispersed materials. By employing soluble reagents in this manner, mixing and dispersion of the active metals and promoter reagents can be near atomic, in fact mi ⁇ oring their dispersion in their respective solutions. The precursor gel thus produced by this process will contain highly dispersed active metals and promoters. High dispersion results in catalyst metal particles in the nanometer size range.
  • the catalytic metal component of the gel is dissolved in a separate protic solvent (e.g., water) and this solution of catalytic metal compound(s) is then mixed with the non-aqueous solution of the matrix component(s).
  • a separate protic solvent e.g., water
  • the catalytic metal component is dissolved in the same non-aqueous solution as the matrix component(s), and an aqueous supplement is used.
  • the concentration or amount of solvent used is linked to the alkoxide content.
  • a molar ratio of 26.5: 1 ethano total alkoxide can be used, although the molar ratio of ethanohtotal alkoxide can be from about 5:1 to 53:1, or even greater. If a large excess of alcohol is used, gelation will not generally occur immediately; some solvent evaporation will be needed. At lower solvent concentrations, it is thought by the inventors that a heavier gel will be formed having less pore volume and surface area.
  • the process continues with adding to the alcohol soluble alkoxide and other reagents, water and any aqueous solutions, in a dropwise fashion, to induce hydrolysis and condensation reaction.
  • a discernible gel point can be reached in minutes or hours.
  • the molar ratio of the total water added to total Mg, Si, Ti, Zr, and Al added varies according to the specific alkoxide being reacted.
  • a molar ratio of wate ⁇ alkoxide from about 0.1 : 1 to 10:1 is used.
  • ratios close to 4: 1 for zirconium(alkoxide) and titanium(alkoxides) 4 can also be used with success.
  • the amount of water utilized in the reaction is that calculated to hydrolyze the alkoxide in the reaction mixture.
  • a ratio lower than that needed to hydrolyze the alkoxide species will result in a partially hydrolyzed material, which in most cases will reach a gel point at a much slower rate, depending on the aging procedure and the presence of atmospheric moisture.
  • the addition of acidic or basic reagents to the alkoxide medium can have an effect on the kinetics of the hydrolysis and condensation reactions, and the micro structure of the oxide/hydroxide matrices derived from the alkoxide precursor which entraps or incorporates the soluble metal and promoter reagents. It is prefe ⁇ ed that a pH within the range of from 1 to 12 is used, with a pH range of from 1 to 6 being more prefe ⁇ ed.
  • the alcogels After reacting to form an alcogel. as described above, it may be necessary to complete the gelation process with some aging of the gel. This aging can range from one minute to several days. Generally, the alcogels are aged at room temperature in air for at least several hours.
  • Removal of solvent from the alcogels is accomplished by several methods. Removal by vacuum drying or heating in air results in the formation of a xerogel.
  • An aerogel of the material can typically be formed by charging in a pressurized system such as an autoclave. The solvent-containing gel is placed in an autoclave where it can be contacted with a fluid above its critical temperature and pressure by allowing supercritical fluid to flow through the gel material until the solvent is no longer being extracted by the supercritical fluid. In performing this extraction to produce an aerogel material, various fluids can be utilized at their critical temperature and pressure.
  • fluorochlorocarbons typified by Freon ® fluorochloromethanes (e.g., Freon ® 1 1 (CCI3F), 12 (CCI2F2) or 1 14 (CCIF2CCIF 2 ), ammonia and carbon dioxide are all suitable for this process.
  • the extraction fluids are gases at atmospheric conditions, so that pore collapse due to the capillary forces at the liquid solid interface are avoided during drying.
  • the resulting material should, in most cases, possess a higher surface area than the non- supercritically dried materials.
  • the xerogels and aerogels thus produced may be described as precursor salts dispersed in an oxide or oxyhydroxide matrix.
  • the hydroxyl content is at this point undefined; a theoretical maximum co ⁇ esponds to the valence of central metal atom.
  • the molar H 2 O:alkoxide ratio can also impact the final xerogel stoichiometry so that there will be residual -OR groups in the unaged gel.
  • reaction with atmospheric moisture will convert these to the co ⁇ esponding -OH, and -O groups upon continued polymerization and dehydration. Aging, even under inert conditions, can also effect the condensation of the -OH, eliminating H 2 O, through continuation of cross linking and polymerization, i.e., gel formation.
  • one or more inorganic metal colloids may be used as starting material for preparing the gels.
  • colloids include colloidal alumina sols, colloidal ceria sols, colloidal zirconia sols or their mixtures.
  • the colloidal sols are commercially available from well-known suppliers. There are also several methods of preparing colloids, as described in "Inorganic Colloid Chemistry", Volumes 1, 2 and 3, J. Wiley and Sons, Inc., 1935. Colloid formation involves either nucleation and growth, or subdivision or dispersion processes.
  • hydrous titanium dioxide sols can be prepared by adding ammonia hydroxide to a solution of a tetravalent titanium salt, followed by peptization (re-dispersion) by dilute alkalis.
  • Zirconium oxide sol can be prepared by dialysis of sodium oxychlorides.
  • Cerium oxide sol can be prepared by dialysis of a solution of eerie ammonium nitrate.
  • alkoxides such as tetraethylorthosilicate and Tyzor® organic titanate esters
  • alkoxides may also be prepared by various well-known routes. Examples include direct reaction of zero valent metal with alcohols in the presence of a suitable catalyst; and the reaction of metal halides with alcohols.
  • Alkoxy derivatives can be synthesized by the reaction of the alkoxide with alcohol in a ligand interchange reaction. Direct reactions of metal dialkamides with alcohol also form alkoxide derivatives. Additional examples are described in D. C. Bradley et al., "Metal Alkoxides" (Academic Press, 1978).
  • preformed colloidal sols in water, or aquasols are used.
  • the aquasols are comprised of colloidal particles ranging in size from 2 to 50 nanometers. In general, the smaller primary particle sizes (2 to 5 nm) are prefe ⁇ ed.
  • the pre-formed colloids contain from 10 to 35 weight % of colloidal oxides or other materials, depending on the method of stabilization.
  • the final de-stabilized colloids can possess from about 1 to 35 weight % solids, preferably from about 1 to 20 weight percent.
  • colloidal oxides or their mixtures are destabilized during the addition of soluble salts of the primary and promoter cation species by the addition of acids or bases or by solvent removal, both of which alter pH. These changes modify the colloidal particle's electrical double layer.
  • Each colloidal particle possesses a double layer when suspended in a liquid medium. For instance, a negatively charged colloid causes some of the positive ions to form a firmly attached layer around the surface of a colloid. Additional positive ions are still attracted by the negative colloid, but now they are repelled by the primary positive layer as well as the positive ions, and form a diffuse layer of counterions. The primary layer and the diffuse layer are refe ⁇ ed to as the double layer.
  • the tendencies of a colloid to either agglomerate (flocculate and precipitate) or polymerize when destabilized will depend on the properties of this double layer.
  • the double layer, and resulting electrostatic forces can be modified by altering the ionic environment, or pH, liquid concentration, or by adding a surface active material directly to affect the charge of the colloid.
  • surface functional groups such as surface hydroxyls.
  • the colloids which are originally stable heterogeneous dispersions of oxides and other species in solvents, are destabilized to produce colloidal gels.
  • Destabilization is induced, in some cases, by the addition of soluble salts, e.g., chlorides or nitrates, which change the pH and the ionic strength of the colloidal suspensions; by the addition of acids or bases; or by solvent removal. pH changes generally accompany the addition of soluble salts; in general, this is prefe ⁇ ed over solvent removal.
  • soluble salts e.g., chlorides or nitrates
  • pH changes generally accompany the addition of soluble salts; in general, this is prefe ⁇ ed over solvent removal.
  • a pH range of from about 0 to about 12 can be used to destabilize the colloids; however, very large extremes in pH (such as pH 12) can cause flocculation and precipitation. For this reason, a pH range of from about 2 to 8 is prefe ⁇ ed.
  • the medium utilized in this process is typically aqueous, although non-aqueous colloids can also be used.
  • the additional metal or inorganic reagents (i.e., salts of Cr or promoters) used should be soluble in the appropriate aqueous and non-aqueous media.
  • Freeze Drying to Form the Solid Catalyst Composition Removal of solvent from the gels can be accomplished by several methods as described above to prepare either an aerogel or xerogel. Freeze drying procedures can accommodate several catalyst compositions, and are useful if the catalyst precursors are soluble in water or other solvent which can be rapidly ( ⁇ 1 minute) frozen. Precursor salts are dissolved in an appropriate amount of solvent to form a solution or fine colloid.
  • the solution is then rapidly cooled and frozen by immersion in a suitable medium, such as liquid nitrogen. If the solution is rapidly frozen, the salts and other components will remain intimately mixed and will not segregate to any significant degree.
  • the frozen solid is transfe ⁇ ed to a freeze drying chamber. The solution is kept frozen while water vapor is removed by evacuation. In the present studies, a two section Virtis freeze drying unit was employed. Refrigerated shelves were used to prevent thaw-out of the frozen solids during evacuation. Spray Drying to Form the Solid Catalyst Composition
  • Spray drying procedures involve the use of solutions, colloids or slurries containing catalyst precursors or catalyst compounds.
  • the technique consists of atomization of these liquids (usually but not exclusively aqueous) into a spray, and contact between spray and drying medium (usually hot air) resulting in moisture evaporation.
  • the drying of the spray proceeds until the desired moisture content in the dried particles is obtained, and the product is recovered by suitable separation techniques (usually cyclone separation).
  • suitable separation techniques usually cyclone separation.
  • Spray roasting also involves the use of solutions or colloids, but generally involves drying and calcination (at higher temperatures) in one process step to produce catalyst powders. Suitable spray roasting techniques are described in U.S. Pat. No. 5,707,910. EXAMPLES
  • Example 1 Crg.jLaQ Ox An aqueous solution of Cr 3 (OH) 2 (CH 3 CO 2 ) 7 (Aldrich 31,810-8) (2.22 mL, 2.5603
  • a magnesium methoxide solution (68.767 mL, 0.3495 M) diluted with 50 volume % ethanol (punctilious) was added to a 150 mL petri dish with gentle swirling under an inert N 2 atmosphere.
  • aqueous Cr 3 (OH) 2 (CH 3 CO 2 )7 solution (1.233 mL, 0.5 M in Cr) was introduced to the petri dish while it was gently swirled.
  • a gel point was realized and a homogeneous gel formed which was nearly white in color.
  • the gel was allowed to age 8 days in air and then dried under vacuum at 120°C prior to use.
  • the final xerogel had a nominal composition of Cro.o25Mgo.975 Ox.
  • Example 3 Cro.2Mgo.4Sio.-l Ox
  • a magnesium methoxide solution (57.474 mL, 0.669 M) and a tetraethylorthosilicate (TEOS) solution (diluted with ethanol to 60 volume % TEOS, 40 volume % ethanol) were simultaneously added to a 150 mL petri dish with gentle swirling under a nitrogen atmosphere.
  • aqueous Cr3(OH) 2 (CH 3 CO 2 )7 solution (7.846 mL, 2.5603 M) was added.
  • a white gel formed, and was aged for 5 days, dried under vacuum at 120°C for 5 hours prior to use.
  • the final xerogel had a nominal composition of C ⁇ Q ,2 ⁇ S0 . A ⁇ 0.A C*x.
  • Example 4 Cro. ⁇ Ceo.9 Ox
  • a titanium n-butoxide solution in ethanol (2.67 mL, 60 volume %) was added to a 150 mL petri dish under an inert nitrogen atmosphere with gentle swirling.
  • an ethanolic solution of anhydrous CoCl 2 (2.342 L, 1.00 M), glacial acetic acid (0.140 mL), H 2 O (1.182 mL) and an ethanolic solution of chromium (III) acetylacetonate (93.667 mL, 0.03 M) were simultaneously added.
  • a gel point was realized following the addition of the aqueous reagents, and the red, opaque gel which formed and was aged for at least 24 hours prior to drying under vacuum at 120°C for five hours.
  • the final xerogel had a nominal composition of Cro.25Coo.25Tio.5Ox.
  • aqueous AuCl 3 solution 28.822 mL, 0.03 M was combined with an aqueous solution of Cr 3 (OH) 2 (CH 3 CO 2 )7 (4.095 mL, 1.689 M in Cr) and an aqueous Al 2 O colloid (5.742 mL, 4.668 M (as Al)) in a 150 mL petri dish with gentle swirling.
  • a NaOH solution (1.340 mL, 0.01 M) was added both for Na content and to destabilize the colloid and induce gellation by altering pH.
  • a red brown gel formed, and the material was aged for at least two days prior to drying under vacuum at 120°C for five hours.
  • the final xerogel had a nominal composition of Cro.2AuQ.25Alo.775 ⁇ x.
  • Example 8 Cr 0 .025 Au 0.025 M ⁇ 0.95 ° x
  • an aqueous solution containing Cr 3 (OH) 2 (CH 3 COO) 7 (0.871 mL, 0.5M in Cr) was added.
  • a gel formed, and the dark gel, after aging for at least three days, was dried at 120°C under vacuum for 5 hours.
  • the final xerogel had a nominal composition of Cro.025Auo.025Mgo.95 Cx-
  • Example 9 10% Cr 1% Li 27% La / ⁇ -Al 2 O 3
  • Example 10 2% Cr 1% Li 27% La / -Al 2 O 3
  • An aqueous solution of L1NO 3 (1.762 g) in distilled water was added by the incipient wetness technique to an alpha-alumina support (22.123 g. calcined at 900°C overnight before use). The solids were dried at 110°C for two hours.
  • Example 11 Freeze-Dried Cr 2 O 3 An aqueous solution of Cr 3 (OH) 2 (CH 3 CO 2 ) 7 (100 mL, 2.5603 M in Cr) was added to a 150 mL petri dish and rapidly frozen with liquid nitrogen. The frozen solid was dried under vacuum for several days (approximately 7 days) to produce a freeze dried powder. The freeze dried material was heated in air at 350°C for 5 hours and 525°C for 1 hour prior to use.
  • Example 12 Aerogel Cr 2 O 3
  • Aerogel synthesis using a sol gel chemistry (Cr O 3 derived from the reaction of CrU 3 and methanol to produce a Cr 2 O 3 gel, followed by supercritical extraction to produce a high surface area oxide (>500 m 2 /g).
  • 16 g of chromium trioxide (CrO , Aldrich 23, 265- 7) was dissolved in 24 ml of water, and added to 420 ml of methanol and 36 ml of additional water.
  • Three of these combined solutions were loaded into a 1 liter autoclave, which was sealed and heated over a four hour time period to 300°C and 3400 psig. After holding at this temperature and pressure for 120 minutes, the pressure was vented to 1000 psig over 2 hours while maintaining 300°C.
  • Example 16 COQ.5 C ⁇ Q.5 OX 30 ml of Co(NO 3 ) .6H 2 O (Aldrich, 23,037-5), 1.0826M was combined with 12.69 ml of an aqueous solution of Cr 3 (OH) (CH 3 CO ) 7 (2.5603M in Cr) to form an aqueous solution which was then frozen, freeze-dried and calcined as described in Example 11.
  • Example 17 CoOx (Comparative Example)
  • Catalysts were evaluated in a 25 cm long quartz tube reactor equipped with a co-axial, quartz thermocouple well, resulting in a 4 mm, reactor i.d.
  • the void space within the reactor was packed with quartz chips.
  • the catalyst bed was positioned with quartz wool at approximately mid-length in the reactor.
  • a three point, K type, thermocouple was used with the catalyst's "hot spot " , read-out temperature reported as the run temperature.
  • the catalyst bed was heated with a 4 inch (10.2 cm), 600 W band furnace at 90% electrical output.
  • Mass flow controllers and meters regulated the feed composition and flow rate. Prior to start-up, the flows were checked manually with a bubble meter and then the feed composition was reconfirmed by gas chromatographic. analysis.
  • the recovered (after use) Cr 2 O 3 catalyst of Example 11 showed no weight loss after thermal gravimetric analysis in air at 600°C to 700°C; no significant carbon deposition (coking) is apparent using this analytical method.
  • Example 11 comparing catalyst performance of the catalysts from Examples 11, 12 and 13, it can be appreciated that the catalyst preparation procedure has a major impact on catalyst performance. All three of these catalysts are nominally chromium oxide, yet demonstrate major differences in performance which can be seen in Table 1.
  • the catalyst of Example 11 was prepared by freeze drying chromium oxide precursors (e.g., chromium hydroxide acetate), followed by calcination at 525°C, which appears to produce a catalyst precursor with superior (best) performance (i.e., highest conversion and selectivity).
  • the catalyst of Example 12 was prepared by aerogel synthesis using a sol gel chemistry (Cr 2 O 3 derived from the reaction of CrO 3 and methanol to produce a Cr 2 O 3 gel, followed by supercritical extraction to produce a high surface area oxide (>500m ⁇ g).
  • the catalyst of Example 13 is a commercially available catalyst. "Newport Chrome,” manufactured by DuPont at the Holly Run site. It is commercially prepared by pyrolyzing ammonium dichromate, (NH 4 ) 2 Cr 2 O 7 . Chromium oxide prepared by freeze drying an aqueous solution of chromium hydroxide acetate, followed by calcination in air at 525°C, is clearly the most active and selective catalyst, as shown in Fig.
  • the conventional view is that chromium promoters or additives promote non- selective reaction pathways for alkane oxidation reactions using molecular oxygen, O 2 .
  • chromium oxide-based compositions as catalysts for the partial oxidation of methane to CO and H 2 , as disclosed herein, is unexpected and even surprising.
  • chromium promoters in vanadium phosphorus oxide catalysts increased catalyst activity at the expense of selectivity. In these cases the catalysts were compared at the same percent conversion of reactant.
  • Oganowski, W. et al. Promotional Effect of Molybdenum. Chromium and Cobalt on a V-Mg-0 catalyst in oxidative dehydrogenation of ethylbenzene to styrene.
  • the reaction chemistry is the oxidative dehydrogenation of ethylbenzene to styrene: "The molybdenum, chromium or cobalt doped V-Mg-O catalyst changes its activity and selectivity in the oxidative dehydrogenation of ethylbenzene. The specific activity decreases in the direction Cr,Co>Cr>Co>Mo while the selectivity increases in the direction: Cr»Co,Cr,Co>Mo.' " This suggests that Cr would not serve as a selective catalyst for a process involving C-H activation, such as CH partial oxidation, and is contrary to the inventors " present findings.
  • the selectivity changes may be related to the surface areas of the catalyst generated. Catalysts possessing the highest surface areas (i.e., a chromium oxide aerogel) also possess the lowest light-off temperatures and exhibit no selectivity to CO/H 2 . This suggests that an increase in the number of sites for CO adsorption results in slower desorption from the catalyst surface, allowing for oxidation of CO. In the millisecond contact time reaction regime, a lower surface area catalyst possessing a limited number of active sites may actually be prefe ⁇ ed for selective oxidation pathways.
  • Fig. 2A shows the crystal structure of the chromium oxide catalyst as prepared in Example 11.
  • the freeze dried chromium oxide is comprised of highly crystalline powder containing well-faceted chromium oxide crystallites. Powder X-ray diffraction confirms the well-crystallized nature of this material. No change in catalyst appearance is apparent after reactor evaluation during an eight hour period, indicating stability of the material on stream over short time intervals.
  • Fig. 2A shows the crystal structure of the chromium oxide catalyst as prepared in Example 11.
  • the freeze dried chromium oxide is comprised of highly crystalline powder containing well-faceted chromium oxide crystallites. Powder X-ray diffraction confirms the well-crystallized nature of this material. No change in catalyst appearance is apparent after reactor evaluation during an eight hour period, indicating stability of the material on stream over short time intervals.
  • FIG. 2B shows the crystal structure of a sample taken after 6 hours on stream, indicating that there was no apparent change in crystallite size or morphology with time on stream in a reactor. After 6 hours on stream there is little carbon build-up (coking). A carbon deposit is indicated by the a ⁇ ow in Fig. 2B.
  • the surprisingly low carbon deposition may also be related to the lower surface area of the catalyst and the highly faceted, defect-free nature of the catalyst surface. Low carbon deposition and stability on stream (i.e., lack of sintering of chromium oxide particles) are very favorable catalyst properties for syngas catalysts.
  • X-ray diffraction (XRD) analysis of the Co/Cr materials of the representative catalysts of Examples 14-16 revealed that the COQ.2 CrQ .
  • g Ox catalyst comprised, in the catalyst as calcined (heated in air), a mixture of CoCr 2 O (cubic spinel phase) and Cr O 3 (eskolaite, hexagonal/rhombohedral phase).
  • XRD analysis revealed Cr 2 ⁇ 3 and possibly Co metal or a chromium carbide phase.
  • Low carbon formation is a very unusual, unexpected, and advantageous feature of many of the Cr 2 ⁇ catalyst systems described herein.
  • Fig. 3 is a graph showing trends in light-off temperature and basicity/ionicity of representative "support" matrix compositions (i.e., CrQ.025 M ⁇ 0.975 Ox; CVQ LaQ.9 Ox; C ⁇ Q. I CeQ.9
  • TGA Thermogravimetric analysis
  • Example 11 In Fig. 4, the a ⁇ ow at about 300°C indicates a temperature region where the catalyst undergoes carbonate decomposition and appreciable weight loss occurs. Carbon deposition, as indicated by the weight loss at about rt-350°C in N is 6.548% (0.6889 mg).
  • the weight loss from about 350-600°C is 2.897% (0.3048 mg), and from about 600-700°C is 0.08311 % (0.008744 mg).
  • TGA analysis of weight loss in air (>600°C) indicates « 1 wt % carbon deposition for these catalyst systems after eight hours on stream (i.e., ⁇ 0.07 wt % upon oxidation in air from 600-700°C for LaQ.i C ⁇ Q.9 Ox).
  • Fig. 5 is a graph showing the reaction chemistry for several representative ternary freeze dried chromium oxides containing chromium and cobalt, and for chromium oxide and cobalt oxide alone.
  • the reaction conditions included 30 % methane feed, 15% O 2 feed, 55% N atmosphere, 6 hours on stream.
  • X-ray diffraction analysis indicated the presence of Cr O 3 matrix and varying proportions of cobalt in the catalyst compositions tested.
  • the low conversion and selectivity demonstrated by cobalt oxide in Fig. 5 shows the beneficial effect of including chromium in the catalyst composition.
  • This figure also indicates an optimal composition range for the specified reaction conditions (i.e., feed composition and flow rate of about 6.1 x 10 4 GHSV).
  • the cobalt chromium oxide materials consist of the cubic spinel (CoCr 2 O ) dispersed in a Cr 2 O 3 matrix (hexagonal/rhombohedral phase, eskolaite).
  • X-ray diffraction indicates a representative cobalt chromium oxide composition contains CoCr O 4 cubic spinel and Cr 2 O 3 .
  • the catalyst precursor COQ.2 C ⁇ Q.8 OX is reduced to cobalt metal and chromium oxide, as shown in Fig. 6A.
  • Figs 7A-C contain the X-ray diffraction data for "reactor evaluated" catalysts having the following compositions, respectively: COQ.2 C ⁇ Q.8 OX, COQ.5 C ⁇ Q.8 Ox, and COQ.8 C ⁇ Q.2 OX. These compositions were prepared as described in Examples 14- 16. Each of these samples show Co metal and Cr 2 O 3 , or pure Co.
  • Example 19 The same procedure was usedas described in Example 19 except that 29.864 ml of the chromium hydroxide acetate solution and 0.468 ml of the nickel nitrate solution were used.
  • Example 23 Ceo.i Crg.7 Nig.2 Ox
  • Example 20 An identical procedure as described in Example 20 was used to make Ceo.iCro.7Nio.2Ox, except that 8.00 ml of 1.00 M cerium nitrate (Ce(NO )3 aqueous solution prepared by dissolving 503.02 g of Ce(NO 3 6 H 2 O (Alfa 11329) in sufficient water to make a 1 M solution) was combined with 33.786 ml of an aqueous solution of Cr 3 (OH) 2 (CH 3 COO) 7 (1.6575 M in Cr), and 14.981 ml of Ni (NO 3 ) 2 of 1.068 M solution (prepared by dissolving Ni(NO 3 ) 2 - 6H 2 O in water; molarity determined by ICP, elemental analysis).
  • Ce(NO )3 aqueous solution prepared by dissolving 503.02 g of Ce(NO 3 6 H 2 O (Alfa 11329) in sufficient water to make a 1 M solution
  • compositions were evaluated for 6 hrs., except where noted otherwise. * Feed composition 90% CH4, 30% O and 10% N 2 ** Evaluated for 25 hrs.
  • catalyst compounds or catalyst precursor materials which provide higher melting point pure ceramic oxides instead of metals, longer-life catalysts are obtained.
  • catalyst composition As demonstrated herein, sintering phenomena, which typically result in loss of catalytic surface area and eventually activity during use, can be diminished at high temperatures, thereby extending catalyst life.
  • Example 18 evaluated for 6 hrs, was 12.8%.
  • the rare earth compounds showed markedly less carbon build-up during a 6 hr evaluation, indicating the desirable longer life of these catalyst compositions.
  • the action of the rare earth oxide may be one of moderating (i.e., lowering) the surface acidity of the oxide, which suppresses some of the acid catalyzed carbon forming reactions.
  • Example 24 Cr 0 . 0 25 (MgO,_ ⁇ (OH) X ) 0 . 9 75 (Xerogel)
  • the material was calcined in air according to the following schedule: 5°/min to 350°C, 350°C for 5 hours, 5°C/min to 525°C, 525°C 1 hour; 10°C /min to room temperature.
  • the material was pelletized and sieved prior to the reactor evaluation as described above.
  • Example 39 14.88 ml of Cu (NO3) .3H 2 O, 1.0 M aqueous solution was combined with 1 19 ml of an aqueous solution of Cr 3 (OH) 2 (CH 3 COO) 7 (0.5M in Cr), prepared as described in Example 39.
  • the mixed solution was rapidly frozen in liquid nitrogen. It was placed in a freeze dryer (Virtis Corporation, shelves refrigerated to 0°C) and evacuated to dryness over a period of 5-7 days, or until completely dry.
  • the material was calcined in air according to the following schedule: 5°C/min to 350°C, 5 hour soak at 350°C, 5°C/min to 525°C, 525°C soak for 1 hour; 10°C /min to room temperature. The material was sieved prior to the reactor evaluation.
  • Example 35 Fe ⁇ .2 ⁇ Q.8 OX
  • ammonium metavandate (NH 4 VO 3 , solution concentration determined by elemental, ICP analysis to be 0.07644 M in V) was combined with 119 ml of an aqueous solution of Cr 3 (OH) 2 (CH 3 COO) 7 (0.5M in Cr), prepared as previously described.
  • the mixed solution was rapidly frozen in liquid nitrogen. It was placed in a freeze dryer (Virtis Corporation, shelves refrigerated to 0°C) and evacuated to dryness over a period of 5-7 days, or until completely dry.
  • Example 37 M ⁇ Q.2 C ⁇ Q.8 OX
  • Mn(NO 3 ) 2 (Alfa, 87848, Mn(NO 3 ) 2 . xH 2 O, contains 22.56 wt % as Mn) was added to 200 ml of an aqueous solution of Cr 3 (OH) 2 (CH3COO) 7 (0.5M in Cr), prepared as previously described.
  • the mixed solution was rapidly frozen in liquid nitrogen. It was placed in a freeze dryer (Virtis Corporation, shelves refrigerated to 0°C) and evacuated to dryness over a period of 5-7 days, or until completely dry.
  • Example 38 COQ.2 WQ.8 ⁇ 6.0 ml Co(NO 3 ) 2 -6H O (Alfa, 11341) aqueous solution of 1.0 M solution was simultaneously combined with 109.639 ml of an aqueous solution of (NH 4 )ioW 12 O 4 r5H 2 O (Alfa, 10899) (0.2189 M in W). The mixed solution was rapidly frozen in liquid nitrogen.
  • Example 39 NiQ.2 w 0.8 O ⁇
  • Example 40 CU0.2W0.8 Ox
  • Example 41 NiQ.2 Mo 0.8 ° x 9.363 ml Ni(NO 3 ) 2 aqueous solution of 1.068 M solution (determined by ICP analysis) was simultaneously combined with 80.0 ml of an aqueous solution of (NH 4 ) Mo 7 O 4 o.4H 2 O (Alfa, 11831) (0.5M in Mo). The mixed solution was rapidly frozen in liquid nitrogen.
  • Example 42 COQ.2 MOQ.8 OX
  • Example 43 CUQ.2 MOQ .8 Ox
  • Any suitable reaction regime is applied in order to contact the reactants with the catalyst.
  • One suitable regime is a fixed bed reaction regime, in which the catalyst is retained within a reaction zone in a fixed a ⁇ angement. Supported or self-supporting catalysts may be employed in the fixed bed regime, retained using fixed bed reaction techniques well known in the art.
  • Preferably a millisecond contact time reactor is employed.
  • CPOX catalytic partial oxidation
  • a catalyst such as platinum or rhodium.
  • a feed stream comprising a hydrocarbon feedstock and an oxygen- containing gas is contacted with one of the above-described chromium-based catalysts in a reaction zone maintained at conversion-promoting conditions effective to produce an effluent stream comprising carbon monoxide and hydrogen.
  • the hydrocarbon feedstock may be any gaseous hydrocarbon having a low boiling point, such as methane, natural gas, associated gas, or other sources of light hydrocarbons having from 1 to 5 carbon atoms.
  • the hydrocarbon feedstock may be a gas arising from naturally occurring reserves of methane which contain carbon dioxide.
  • the feed comprises at least 50% by volume methane, more preferably at least 75% by volume, and most preferably at least 80% by volume methane.
  • the hydrocarbon feedstock is contacted with the catalyst as a gaseous phase mixture with an oxygen-containing gas, preferably pure oxygen.
  • the oxygen-containing gas may also comprise steam and/or CO 2 in addition to oxygen.
  • the hydrocarbon feedstock is contacted with the catalyst as a mixture with a gas comprising steam and/or CO 2 .
  • the methane-containing feed and the oxygen-containing gas are mixed in such amounts to give a carbon (i.e., carbon in methane) to oxygen (i.e., oxygen) ratio from about 1.25: 1 to about 3.3:1, more preferably, from about 1.3:1 to about 2.2:1, and most preferably from about 1.5:1 to about 2.2:1, especially the stoichiometric ratio of 2:1.
  • the process is operated at atmospheric or superatmospheric pressures, the latter being prefe ⁇ ed.
  • the pressures may be from about 100 kPa to about 12,500 kPa, preferably from about 130 kPa to about 10,000 kPa.
  • the process of the present invention may be operated at temperatures of from about 600°C to about 1,100°C, preferably from about 700°C to about 1,000°C.
  • the hydrocarbon feedstock and the oxygen-containing gas are preferably pre-heated before contact with the catalyst.
  • the hydrocarbon feedstock and the oxygen-containing gas are passed over the catalyst at any of a variety of space velocities.
  • Gas hourly space velocities (GHSV) for the process are from about 20000 to at least about 100.000,000 NL/kg/h, preferably from about 50,000 to about 50,000,000 NL/kg/h.
  • the catalyst is employed in a millisecond contact time reactor for syngas production.
  • the process preferably includes maintaining a catalyst residence time of no more than 10 milliseconds for the reactant gas mixture. Residence time is the inverse of the space velocity, and high space velocity equates to low residence time on the catalyst.
  • the effluent stream of product gases, including CO and H 2 emerges from the reactor.
  • the inventors believe that the primary reaction catalyzed by the prefe ⁇ ed catalysts described herein is the partial oxidation reaction of Equation 2, described above in the background of the invention. Additionally, other chemical reactions may also occur to a lesser extent, catalyzed by the same catalyst composition. For example, in the course of syngas generation, intermediates such as CO 2 + H O may occur as a result of the oxidation of methane, followed by a reforming step to produce CO and H 2 . Also, particularly in the presence of carbon dioxide-containing feedstock or CO 2 intermediate, the reaction CH + CO 2 — » 2 CO + 2H 2 (3) may also occur during the production of syngas.

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Abstract

L'invention concerne des procédés destinés à la conversion catalytique d'hydrocarbures en monoxyde de carbone et en hydrogène utilisant des nouveaux catalyseurs à base de chrome. Un système catalytique hautement actif et sélectif, qui permet d'obtenir une conversion de CH4 supérieure à 95 % et une sélectivité de l'ordre de 97-98 % par rapport à CO et H2, est formé par un catalyseur contenant du chrome constitué par un précurseur de spinelles cubiques CoCr2O4 dispersé dans une matrice d'oxyde de chrome. D'autre compositions catalytiques préférées comprennent des composés contenant du nickel-chrome et des composés contenant du chrome des terres rares.
EP01910791A 2000-02-18 2001-02-16 Catalyseur a base de chrome et procedes de conversion d'hydrocarbures en gaz de synthese Withdrawn EP1257497A2 (fr)

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