EP1126914A1 - Preparation of nanocrystalline and dispersible supported metal catalysts - Google Patents
Preparation of nanocrystalline and dispersible supported metal catalystsInfo
- Publication number
- EP1126914A1 EP1126914A1 EP99954150A EP99954150A EP1126914A1 EP 1126914 A1 EP1126914 A1 EP 1126914A1 EP 99954150 A EP99954150 A EP 99954150A EP 99954150 A EP99954150 A EP 99954150A EP 1126914 A1 EP1126914 A1 EP 1126914A1
- Authority
- EP
- European Patent Office
- Prior art keywords
- metal
- metal oxide
- product
- catalyst
- heated
- 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- Withdrawn
Links
- 229910052751 metal Inorganic materials 0.000 title claims abstract description 65
- 239000002184 metal Substances 0.000 title claims abstract description 65
- 239000003054 catalyst Substances 0.000 title claims description 30
- 238000002360 preparation method Methods 0.000 title claims description 6
- 229910044991 metal oxide Inorganic materials 0.000 claims abstract description 61
- 150000004706 metal oxides Chemical class 0.000 claims abstract description 61
- 238000000034 method Methods 0.000 claims abstract description 54
- 230000008569 process Effects 0.000 claims abstract description 45
- 239000002245 particle Substances 0.000 claims abstract description 22
- 239000000203 mixture Substances 0.000 claims abstract description 21
- 150000003839 salts Chemical class 0.000 claims abstract description 20
- 238000010438 heat treatment Methods 0.000 claims abstract description 18
- 239000011240 wet gel Substances 0.000 claims abstract description 14
- 229910003455 mixed metal oxide Inorganic materials 0.000 claims abstract description 11
- 238000004519 manufacturing process Methods 0.000 claims abstract description 7
- 239000002105 nanoparticle Substances 0.000 claims abstract description 6
- 238000000354 decomposition reaction Methods 0.000 claims abstract description 5
- XLYOFNOQVPJJNP-UHFFFAOYSA-N water Substances O XLYOFNOQVPJJNP-UHFFFAOYSA-N 0.000 claims description 31
- 230000009467 reduction Effects 0.000 claims description 17
- PNEYBMLMFCGWSK-UHFFFAOYSA-N aluminium oxide Inorganic materials [O-2].[O-2].[O-2].[Al+3].[Al+3] PNEYBMLMFCGWSK-UHFFFAOYSA-N 0.000 claims description 13
- 239000000758 substrate Substances 0.000 claims description 12
- 229910001510 metal chloride Inorganic materials 0.000 claims description 5
- 229910001960 metal nitrate Inorganic materials 0.000 claims description 5
- 239000011248 coating agent Substances 0.000 claims description 4
- 238000000576 coating method Methods 0.000 claims description 4
- BVKZGUZCCUSVTD-UHFFFAOYSA-L Carbonate Chemical compound [O-]C([O-])=O BVKZGUZCCUSVTD-UHFFFAOYSA-L 0.000 claims description 3
- 239000003125 aqueous solvent Substances 0.000 claims description 2
- VLTRZXGMWDSKGL-UHFFFAOYSA-N perchloric acid Chemical compound OCl(=O)(=O)=O VLTRZXGMWDSKGL-UHFFFAOYSA-N 0.000 claims description 2
- 239000013049 sediment Substances 0.000 claims description 2
- QTBSBXVTEAMEQO-UHFFFAOYSA-M Acetate Chemical compound CC([O-])=O QTBSBXVTEAMEQO-UHFFFAOYSA-M 0.000 claims 1
- VLTRZXGMWDSKGL-UHFFFAOYSA-M perchlorate Inorganic materials [O-]Cl(=O)(=O)=O VLTRZXGMWDSKGL-UHFFFAOYSA-M 0.000 claims 1
- 239000000047 product Substances 0.000 description 30
- MCMNRKCIXSYSNV-UHFFFAOYSA-N Zirconium dioxide Chemical compound O=[Zr]=O MCMNRKCIXSYSNV-UHFFFAOYSA-N 0.000 description 20
- 239000000499 gel Substances 0.000 description 17
- 239000012153 distilled water Substances 0.000 description 13
- 239000002159 nanocrystal Substances 0.000 description 13
- 238000003756 stirring Methods 0.000 description 13
- 239000001301 oxygen Substances 0.000 description 11
- 229910052760 oxygen Inorganic materials 0.000 description 11
- QVGXLLKOCUKJST-UHFFFAOYSA-N atomic oxygen Chemical compound [O] QVGXLLKOCUKJST-UHFFFAOYSA-N 0.000 description 10
- 229910000422 cerium(IV) oxide Inorganic materials 0.000 description 10
- 239000006185 dispersion Substances 0.000 description 10
- 239000000243 solution Substances 0.000 description 9
- CETPSERCERDGAM-UHFFFAOYSA-N ceric oxide Chemical compound O=[Ce]=O CETPSERCERDGAM-UHFFFAOYSA-N 0.000 description 8
- BASFCYQUMIYNBI-UHFFFAOYSA-N platinum Substances [Pt] BASFCYQUMIYNBI-UHFFFAOYSA-N 0.000 description 8
- 239000010948 rhodium Substances 0.000 description 8
- 150000002739 metals Chemical class 0.000 description 7
- 239000000843 powder Substances 0.000 description 7
- 229910052703 rhodium Inorganic materials 0.000 description 7
- 239000006104 solid solution Substances 0.000 description 7
- PXHVJJICTQNCMI-UHFFFAOYSA-N Nickel Chemical compound [Ni] PXHVJJICTQNCMI-UHFFFAOYSA-N 0.000 description 6
- QCWXUUIWCKQGHC-UHFFFAOYSA-N Zirconium Chemical compound [Zr] QCWXUUIWCKQGHC-UHFFFAOYSA-N 0.000 description 6
- 239000000463 material Substances 0.000 description 6
- 229910052726 zirconium Inorganic materials 0.000 description 6
- 238000002441 X-ray diffraction Methods 0.000 description 5
- KDLHZDBZIXYQEI-UHFFFAOYSA-N palladium Substances [Pd] KDLHZDBZIXYQEI-UHFFFAOYSA-N 0.000 description 5
- MHOVAHRLVXNVSD-UHFFFAOYSA-N rhodium atom Chemical compound [Rh] MHOVAHRLVXNVSD-UHFFFAOYSA-N 0.000 description 5
- 239000006228 supernatant Substances 0.000 description 5
- XEEYBQQBJWHFJM-UHFFFAOYSA-N Iron Chemical compound [Fe] XEEYBQQBJWHFJM-UHFFFAOYSA-N 0.000 description 4
- 239000002253 acid Substances 0.000 description 4
- 230000003197 catalytic effect Effects 0.000 description 4
- 238000006555 catalytic reaction Methods 0.000 description 4
- 238000006243 chemical reaction Methods 0.000 description 4
- 239000010949 copper Substances 0.000 description 4
- 239000010416 ion conductor Substances 0.000 description 4
- 238000007254 oxidation reaction Methods 0.000 description 4
- 229910052697 platinum Inorganic materials 0.000 description 4
- RZVAJINKPMORJF-UHFFFAOYSA-N Acetaminophen Chemical compound CC(=O)NC1=CC=C(O)C=C1 RZVAJINKPMORJF-UHFFFAOYSA-N 0.000 description 3
- 229910052684 Cerium Inorganic materials 0.000 description 3
- RYGMFSIKBFXOCR-UHFFFAOYSA-N Copper Chemical compound [Cu] RYGMFSIKBFXOCR-UHFFFAOYSA-N 0.000 description 3
- 230000008901 benefit Effects 0.000 description 3
- WUKWITHWXAAZEY-UHFFFAOYSA-L calcium difluoride Chemical compound [F-].[F-].[Ca+2] WUKWITHWXAAZEY-UHFFFAOYSA-L 0.000 description 3
- GWXLDORMOJMVQZ-UHFFFAOYSA-N cerium Chemical compound [Ce] GWXLDORMOJMVQZ-UHFFFAOYSA-N 0.000 description 3
- 229910052802 copper Inorganic materials 0.000 description 3
- 238000001035 drying Methods 0.000 description 3
- 239000010436 fluorite Substances 0.000 description 3
- 229910052759 nickel Inorganic materials 0.000 description 3
- 230000003647 oxidation Effects 0.000 description 3
- 229910052763 palladium Inorganic materials 0.000 description 3
- 239000002244 precipitate Substances 0.000 description 3
- 230000001737 promoting effect Effects 0.000 description 3
- 239000005297 pyrex Substances 0.000 description 3
- 239000007787 solid Substances 0.000 description 3
- MCSXGCZMEPXKIW-UHFFFAOYSA-N 3-hydroxy-4-[(4-methyl-2-nitrophenyl)diazenyl]-N-(3-nitrophenyl)naphthalene-2-carboxamide Chemical compound Cc1ccc(N=Nc2c(O)c(cc3ccccc23)C(=O)Nc2cccc(c2)[N+]([O-])=O)c(c1)[N+]([O-])=O MCSXGCZMEPXKIW-UHFFFAOYSA-N 0.000 description 2
- QGZKDVFQNNGYKY-UHFFFAOYSA-N Ammonia Chemical compound N QGZKDVFQNNGYKY-UHFFFAOYSA-N 0.000 description 2
- VYZAMTAEIAYCRO-UHFFFAOYSA-N Chromium Chemical compound [Cr] VYZAMTAEIAYCRO-UHFFFAOYSA-N 0.000 description 2
- RTAQQCXQSZGOHL-UHFFFAOYSA-N Titanium Chemical compound [Ti] RTAQQCXQSZGOHL-UHFFFAOYSA-N 0.000 description 2
- 150000001450 anions Chemical class 0.000 description 2
- 229910052804 chromium Inorganic materials 0.000 description 2
- 239000011651 chromium Substances 0.000 description 2
- BERDEBHAJNAUOM-UHFFFAOYSA-N copper(I) oxide Inorganic materials [Cu]O[Cu] BERDEBHAJNAUOM-UHFFFAOYSA-N 0.000 description 2
- 239000007789 gas Substances 0.000 description 2
- 229930195733 hydrocarbon Natural products 0.000 description 2
- 150000002430 hydrocarbons Chemical class 0.000 description 2
- 229910052742 iron Inorganic materials 0.000 description 2
- 239000011159 matrix material Substances 0.000 description 2
- 239000002923 metal particle Substances 0.000 description 2
- 238000002156 mixing Methods 0.000 description 2
- AHKZTVQIVOEVFO-UHFFFAOYSA-N oxide(2-) Chemical compound [O-2] AHKZTVQIVOEVFO-UHFFFAOYSA-N 0.000 description 2
- -1 oxygen ion Chemical class 0.000 description 2
- 230000005855 radiation Effects 0.000 description 2
- 239000011369 resultant mixture Substances 0.000 description 2
- 239000002002 slurry Substances 0.000 description 2
- 239000002904 solvent Substances 0.000 description 2
- 230000003019 stabilising effect Effects 0.000 description 2
- 229910052719 titanium Inorganic materials 0.000 description 2
- 239000010936 titanium Substances 0.000 description 2
- 229910052723 transition metal Inorganic materials 0.000 description 2
- 150000003624 transition metals Chemical class 0.000 description 2
- 229910052727 yttrium Inorganic materials 0.000 description 2
- VWQVUPCCIRVNHF-UHFFFAOYSA-N yttrium atom Chemical compound [Y] VWQVUPCCIRVNHF-UHFFFAOYSA-N 0.000 description 2
- RUDFQVOCFDJEEF-UHFFFAOYSA-N yttrium(III) oxide Inorganic materials [O-2].[O-2].[O-2].[Y+3].[Y+3] RUDFQVOCFDJEEF-UHFFFAOYSA-N 0.000 description 2
- NLXLAEXVIDQMFP-UHFFFAOYSA-N Ammonium chloride Substances [NH4+].[Cl-] NLXLAEXVIDQMFP-UHFFFAOYSA-N 0.000 description 1
- VHUUQVKOLVNVRT-UHFFFAOYSA-N Ammonium hydroxide Chemical compound [NH4+].[OH-] VHUUQVKOLVNVRT-UHFFFAOYSA-N 0.000 description 1
- OKTJSMMVPCPJKN-UHFFFAOYSA-N Carbon Chemical compound [C] OKTJSMMVPCPJKN-UHFFFAOYSA-N 0.000 description 1
- 229910052688 Gadolinium Inorganic materials 0.000 description 1
- 229910002621 H2PtCl6 Inorganic materials 0.000 description 1
- MHAJPDPJQMAIIY-UHFFFAOYSA-N Hydrogen peroxide Chemical compound OO MHAJPDPJQMAIIY-UHFFFAOYSA-N 0.000 description 1
- FYYHWMGAXLPEAU-UHFFFAOYSA-N Magnesium Chemical compound [Mg] FYYHWMGAXLPEAU-UHFFFAOYSA-N 0.000 description 1
- PWHULOQIROXLJO-UHFFFAOYSA-N Manganese Chemical compound [Mn] PWHULOQIROXLJO-UHFFFAOYSA-N 0.000 description 1
- 240000008790 Musa x paradisiaca Species 0.000 description 1
- 235000018290 Musa x paradisiaca Nutrition 0.000 description 1
- 229910052779 Neodymium Inorganic materials 0.000 description 1
- GRYLNZFGIOXLOG-UHFFFAOYSA-N Nitric acid Chemical compound O[N+]([O-])=O GRYLNZFGIOXLOG-UHFFFAOYSA-N 0.000 description 1
- 240000007817 Olea europaea Species 0.000 description 1
- KJTLSVCANCCWHF-UHFFFAOYSA-N Ruthenium Chemical compound [Ru] KJTLSVCANCCWHF-UHFFFAOYSA-N 0.000 description 1
- BQCADISMDOOEFD-UHFFFAOYSA-N Silver Chemical compound [Ag] BQCADISMDOOEFD-UHFFFAOYSA-N 0.000 description 1
- 229910006220 ZrO(OH)2 Inorganic materials 0.000 description 1
- 230000001133 acceleration Effects 0.000 description 1
- 150000001242 acetic acid derivatives Chemical class 0.000 description 1
- 239000004411 aluminium Substances 0.000 description 1
- 229910052782 aluminium Inorganic materials 0.000 description 1
- XAGFODPZIPBFFR-UHFFFAOYSA-N aluminium Chemical compound [Al] XAGFODPZIPBFFR-UHFFFAOYSA-N 0.000 description 1
- 229910021529 ammonia Inorganic materials 0.000 description 1
- 235000011114 ammonium hydroxide Nutrition 0.000 description 1
- 238000010420 art technique Methods 0.000 description 1
- 230000015572 biosynthetic process Effects 0.000 description 1
- 229910052799 carbon Inorganic materials 0.000 description 1
- 150000004649 carbonic acid derivatives Chemical class 0.000 description 1
- 238000005266 casting Methods 0.000 description 1
- 229910000420 cerium oxide Inorganic materials 0.000 description 1
- 238000012512 characterization method Methods 0.000 description 1
- 239000003153 chemical reaction reagent Substances 0.000 description 1
- 229910017052 cobalt Inorganic materials 0.000 description 1
- 239000010941 cobalt Substances 0.000 description 1
- GUTLYIVDDKVIGB-UHFFFAOYSA-N cobalt atom Chemical compound [Co] GUTLYIVDDKVIGB-UHFFFAOYSA-N 0.000 description 1
- 150000001875 compounds Chemical class 0.000 description 1
- 230000001143 conditioned effect Effects 0.000 description 1
- 239000000470 constituent Substances 0.000 description 1
- 238000007796 conventional method Methods 0.000 description 1
- KRFJLUBVMFXRPN-UHFFFAOYSA-N cuprous oxide Chemical compound [O-2].[Cu+].[Cu+] KRFJLUBVMFXRPN-UHFFFAOYSA-N 0.000 description 1
- 229940112669 cuprous oxide Drugs 0.000 description 1
- 230000007547 defect Effects 0.000 description 1
- 238000000151 deposition Methods 0.000 description 1
- 238000007865 diluting Methods 0.000 description 1
- 239000002019 doping agent Substances 0.000 description 1
- 238000002296 dynamic light scattering Methods 0.000 description 1
- 230000000694 effects Effects 0.000 description 1
- 238000001493 electron microscopy Methods 0.000 description 1
- 238000000921 elemental analysis Methods 0.000 description 1
- 238000002149 energy-dispersive X-ray emission spectroscopy Methods 0.000 description 1
- 230000007613 environmental effect Effects 0.000 description 1
- 238000001704 evaporation Methods 0.000 description 1
- UIWYJDYFSGRHKR-UHFFFAOYSA-N gadolinium atom Chemical compound [Gd] UIWYJDYFSGRHKR-UHFFFAOYSA-N 0.000 description 1
- PCHJSUWPFVWCPO-UHFFFAOYSA-N gold Chemical compound [Au] PCHJSUWPFVWCPO-UHFFFAOYSA-N 0.000 description 1
- 229910052737 gold Inorganic materials 0.000 description 1
- 239000010931 gold Substances 0.000 description 1
- 230000036571 hydration Effects 0.000 description 1
- 238000006703 hydration reaction Methods 0.000 description 1
- 230000037427 ion transport Effects 0.000 description 1
- 229910000311 lanthanide oxide Inorganic materials 0.000 description 1
- 229910052747 lanthanoid Inorganic materials 0.000 description 1
- 150000002602 lanthanoids Chemical class 0.000 description 1
- 229910052746 lanthanum Inorganic materials 0.000 description 1
- FZLIPJUXYLNCLC-UHFFFAOYSA-N lanthanum atom Chemical compound [La] FZLIPJUXYLNCLC-UHFFFAOYSA-N 0.000 description 1
- 239000011777 magnesium Substances 0.000 description 1
- 229910052749 magnesium Inorganic materials 0.000 description 1
- 229910052748 manganese Inorganic materials 0.000 description 1
- 239000011572 manganese Substances 0.000 description 1
- 229910021645 metal ion Inorganic materials 0.000 description 1
- QEFYFXOXNSNQGX-UHFFFAOYSA-N neodymium atom Chemical compound [Nd] QEFYFXOXNSNQGX-UHFFFAOYSA-N 0.000 description 1
- 229910017604 nitric acid Inorganic materials 0.000 description 1
- UJVRJBAUJYZFIX-UHFFFAOYSA-N nitric acid;oxozirconium Chemical compound [Zr]=O.O[N+]([O-])=O.O[N+]([O-])=O UJVRJBAUJYZFIX-UHFFFAOYSA-N 0.000 description 1
- 230000001590 oxidative effect Effects 0.000 description 1
- BMMGVYCKOGBVEV-UHFFFAOYSA-N oxo(oxoceriooxy)cerium Chemical compound [Ce]=O.O=[Ce]=O BMMGVYCKOGBVEV-UHFFFAOYSA-N 0.000 description 1
- 150000003057 platinum Chemical class 0.000 description 1
- 238000000634 powder X-ray diffraction Methods 0.000 description 1
- 230000001376 precipitating effect Effects 0.000 description 1
- 239000002243 precursor Substances 0.000 description 1
- 239000011541 reaction mixture Substances 0.000 description 1
- 238000006479 redox reaction Methods 0.000 description 1
- 230000004044 response Effects 0.000 description 1
- 229910052707 ruthenium Inorganic materials 0.000 description 1
- 239000012266 salt solution Substances 0.000 description 1
- 238000007789 sealing Methods 0.000 description 1
- 229910052709 silver Inorganic materials 0.000 description 1
- 239000004332 silver Substances 0.000 description 1
- 238000004544 sputter deposition Methods 0.000 description 1
- 239000007858 starting material Substances 0.000 description 1
- 230000007704 transition Effects 0.000 description 1
- 229910000314 transition metal oxide Inorganic materials 0.000 description 1
- 229910001233 yttria-stabilized zirconia Inorganic materials 0.000 description 1
- PDTGVTZFEAGHFZ-UHFFFAOYSA-N yttrium(3+);trinitrate;pentahydrate Chemical compound O.O.O.O.O.[Y+3].[O-][N+]([O-])=O.[O-][N+]([O-])=O.[O-][N+]([O-])=O PDTGVTZFEAGHFZ-UHFFFAOYSA-N 0.000 description 1
Classifications
-
- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01F—COMPOUNDS OF THE METALS BERYLLIUM, MAGNESIUM, ALUMINIUM, CALCIUM, STRONTIUM, BARIUM, RADIUM, THORIUM, OR OF THE RARE-EARTH METALS
- C01F17/00—Compounds of rare earth metals
- C01F17/20—Compounds containing only rare earth metals as the metal element
- C01F17/206—Compounds containing only rare earth metals as the metal element oxide or hydroxide being the only anion
- C01F17/224—Oxides or hydroxides of lanthanides
- C01F17/235—Cerium oxides or hydroxides
-
- B—PERFORMING OPERATIONS; TRANSPORTING
- B82—NANOTECHNOLOGY
- B82Y—SPECIFIC USES OR APPLICATIONS OF NANOSTRUCTURES; MEASUREMENT OR ANALYSIS OF NANOSTRUCTURES; MANUFACTURE OR TREATMENT OF NANOSTRUCTURES
- B82Y30/00—Nanotechnology for materials or surface science, e.g. nanocomposites
-
- B—PERFORMING OPERATIONS; TRANSPORTING
- B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
- B01D—SEPARATION
- B01D53/00—Separation of gases or vapours; Recovering vapours of volatile solvents from gases; Chemical or biological purification of waste gases, e.g. engine exhaust gases, smoke, fumes, flue gases, aerosols
- B01D53/34—Chemical or biological purification of waste gases
- B01D53/74—General processes for purification of waste gases; Apparatus or devices specially adapted therefor
- B01D53/86—Catalytic processes
- B01D53/88—Handling or mounting catalysts
- B01D53/885—Devices in general for catalytic purification of waste gases
-
- 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
- B01J23/40—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of noble metals of the platinum group metals
-
- B—PERFORMING OPERATIONS; TRANSPORTING
- B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
- B01J—CHEMICAL OR PHYSICAL PROCESSES, e.g. CATALYSIS OR COLLOID CHEMISTRY; THEIR RELEVANT APPARATUS
- B01J23/00—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00
- B01J23/38—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of noble metals
- B01J23/54—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of noble metals combined with metals, oxides or hydroxides provided for in groups B01J23/02 - B01J23/36
- B01J23/56—Platinum group metals
- B01J23/63—Platinum group metals with rare earths or actinides
-
- B—PERFORMING OPERATIONS; TRANSPORTING
- B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
- B01J—CHEMICAL OR PHYSICAL PROCESSES, e.g. CATALYSIS OR COLLOID CHEMISTRY; THEIR RELEVANT APPARATUS
- B01J23/00—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00
- B01J23/70—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of the iron group metals or copper
- B01J23/76—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of the iron group metals or copper combined with metals, oxides or hydroxides provided for in groups B01J23/02 - B01J23/36
- B01J23/83—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of the iron group metals or copper combined with metals, oxides or hydroxides provided for in groups B01J23/02 - B01J23/36 with rare earths or actinides
-
- 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
- B01J35/00—Catalysts, in general, characterised by their form or physical properties
- B01J35/20—Catalysts, in general, characterised by their form or physical properties characterised by their non-solid state
- B01J35/23—Catalysts, in general, characterised by their form or physical properties characterised by their non-solid state in a colloidal state
-
- 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
-
- 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
- B01J37/08—Heat treatment
- B01J37/082—Decomposition and pyrolysis
- B01J37/088—Decomposition of a metal salt
-
- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
- C01B13/00—Oxygen; Ozone; Oxides or hydroxides in general
- C01B13/14—Methods for preparing oxides or hydroxides in general
- C01B13/18—Methods for preparing oxides or hydroxides in general by thermal decomposition of compounds, e.g. of salts or hydroxides
- C01B13/185—Preparing mixtures of oxides
-
- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01G—COMPOUNDS CONTAINING METALS NOT COVERED BY SUBCLASSES C01D OR C01F
- C01G25/00—Compounds of zirconium
- C01G25/02—Oxides
-
- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
- C01P2002/00—Crystal-structural characteristics
- C01P2002/50—Solid solutions
-
- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
- C01P2002/00—Crystal-structural characteristics
- C01P2002/50—Solid solutions
- C01P2002/52—Solid solutions containing elements as dopants
- C01P2002/54—Solid solutions containing elements as dopants one element only
-
- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
- C01P2002/00—Crystal-structural characteristics
- C01P2002/60—Compounds characterised by their crystallite size
-
- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
- C01P2002/00—Crystal-structural characteristics
- C01P2002/70—Crystal-structural characteristics defined by measured X-ray, neutron or electron diffraction data
- C01P2002/72—Crystal-structural characteristics defined by measured X-ray, neutron or electron diffraction data by d-values or two theta-values, e.g. as X-ray diagram
-
- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
- C01P2004/00—Particle morphology
- C01P2004/60—Particles characterised by their size
- C01P2004/64—Nanometer sized, i.e. from 1-100 nanometer
Definitions
- the present invention relates to the field of the preparation of supported metal and metal oxide products, particularly catalysts.
- the lower or higher valent dopant for example Ln 3+ , Y 3+ or Zr 4+ (wherein Ln represents a lanthanide metal), creates oxygen ion vacancies in the fluorite lattice, thus allowing facile oxygen ion transport within the lattice to the surface.
- an "active" metal (or metal oxide) on the surface of an oxygen ion conductor catalyses redox reactions with atmospheric gases.
- An example of this is in exhaust emission control (catalytic converters), where oxygen may react with CO gas, or unbumed hydrocarbons, to form C0 2 and water (oxidation), and where NO may react with CO to produce N 2 and C0 2 (reduction/oxidation) .
- the ability of the oxide ion conductor (the "promoting" oxide ion conductor) supporting the active metal/metal oxide in such a system to release oxygen under reducing conditions (acceleration), and to take up oxygen under oxidizing conditions (deceleration), has a direct effect upon the size of the window of oxygen partial pressures over which the active metal (e.g. Pt, Rh or Pd) is effective.
- the active metal e.g. Pt, Rh or Pd
- catalytic efficiency relies on the high dispersion of active metal on the promoter alone.
- this technique may be modified by including at least one reducible salt of an active metal in the initial reaction mixture in order to produce an aqueous dispersion of individual crystalline nanoparticles cont ⁇ ining both the active metal/metal oxide and the promoter as a single phase.
- at least one reducible salt of an active metal in the initial reaction mixture in order to produce an aqueous dispersion of individual crystalline nanoparticles cont ⁇ ining both the active metal/metal oxide and the promoter as a single phase.
- simple reduction of these nanocrystals results in the active metal/metal particles being substantially dispersed on the surface of the promoter oxide. This results in a process that may be employed in the preparation of inter alia improved catalyst products.
- a process for the production of a product comprising nanocrystalline particles, which particles comprise at least one metal, or at least one metal oxide, substantially dispersed on the surface of at least one metal oxide, or mixed metal oxide, which process includes the steps of:
- process steps (a), (b) and (c) are preferably carried out in the above order.
- the process of the invention may be used to prepare particles that are substantially nanocrystalline in nature (i.e. up to 100% of the individual, unagglomerated crystallites have a particle size of less than 500 nm (e.g. less than 250 nm, preferably less than 50 nm)), as used herein, the term "nanocrystalline" particles, includes that no more than 1 % of particles produced via the process of the invention are non-crystalline, and/or that no more than 1 % of particles produced via the process of the invention exceed a particle size of 500 nm, and in which the average crystallite sizes (Z av ) are in the range 3 to 250 nm (e.g. 4 to 100 nm and preferably 10 to 30 nm).
- substantially dispersed we include that at least 40%, preferably at least 60%, and more preferably at least 80%, of the relevant metal or metal oxide (as appropriate) is presented, e.g. as particles, on the surface of the metal oxide support, as opposed to within the matrix thereof.
- wet hydrous metal oxides, and mixed metal oxides includes systems comprising a hydrous metal oxide and water, wherein the combined lattice water and/or free water content, is present in excess of 10% w/w, and preferably between 10 and 200% w/w, of the metal oxide system, whether coordinated to the metal ions of the metal oxide system or otherwise.
- the term "wet gel” as used herein includes a gel system containing a metal oxide, lattice water and, optionally, depending upon the oxide system that is employed, excess free water, wherein any excess free water that is present, is present in an excess of between 0 and 95 % , preferably 0 and 70% , and especially 0 and 60% , w/w of the total weight of the gel.
- step (b) of the process of the invention results in the production of deaggregated material.
- the heating step (b) may preferably be carried out until the reducible metal salt is decomposed and/or the product is deaggregated.
- the product of step (b) may preferably be dispersed onto a suitable substrate (e.g. a high surface area support) before or after carrying out the reduction step (c).
- a suitable substrate e.g. a high surface area support
- This dispersion may be achieved by dispersing the product of step (b) into a suitable medium (e.g. an aqueous solvent, such as distilled water), casting the resultant mixture onto the relevant substrate and drying as necessary.
- a suitable medium e.g. an aqueous solvent, such as distilled water
- non-dispersible product which may be formed following step (b) may be removed using conventional techniques.
- non-dispersible product we include product, which is of a particle size which is too great to allow it to enter the colloidal state.
- non-dispersible product may be removed by dispersing the product of step (b) as described above to form a sol. In such an instance, dispersion may take place with stirring over an appropriate period (e.g. approximately 1 hour) followed by standing over 2 hours. Any non-dispersible sediment may then be removed by an appropriate means (e.g. decanting the supernatant).
- the resultant sol which may or may not be dialysed using techniques known to those skilled in the art in order to remove any excess anions, may comprise a single phase nanocrystalline solid solution (i.e. it does not comprise particles of a size of greater than 500 nm, preferably greater than 250 nm, once the non-dispersible product is removed).
- the nanocrystals may then be dispersed onto an appropriate substrate (e.g. ⁇ -Al 2 0 3 ) before carrying out the reduction step (c).
- an appropriate substrate e.g. ⁇ -Al 2 0 3
- the reduction step (c) may be performed directly after step (b), and any non-dispersible product may then be removed by dispersing the product of step (c) into a solvent to form a sol in the above-described manner.
- the resultant nanocrystals comprising reduced metal, or metal oxide may then be dispersed onto an appropriate substrate (e.g. ⁇ - A1 2 0 3 ).
- reduction step (c) results in reduced metal migrating to, and being presented on, the surface of the metal oxide particles.
- Such metals may or may not re-oxidise (or partially re-oxidise), if subjected to an oxygen-containing atmosphere (such as air), once they have migrated to the surface such that a metal oxide (and/or mixed metal/metal oxide) is presented on the surface of the metal oxide particles (though this surface re-oxidation may be prevented if the product of step (c) is kept in a reducing environment).
- the process of the invention finds particular utility in the production of products (e.g. catalysts) in which an active metal, or active metal oxide, is supported on (i.e. dispersed, or presented, on the surface of) a metal oxide (e.g. a promoter or stabilising oxide, or a solid solution of metal oxides).
- the process of the invention may be used to form products comprising a wide variety of metals or metal oxides, which are supported on metal oxide systems, mixed metal oxide systems, and/or metal oxide hydrate systems.
- any "active" metal (e.g. transition metal) or “active” metal (e.g. transition metal) oxide that is capable of catalysing a chemical reaction to a experimentally determinable degree may be employed in the process of the invention.
- Suitable active metals include palladium, platinum, rhodium, copper, iron, chromium, silver, cobalt, ruthenium and nickel and suitable active metal oxides include those of copper.
- Suitable supporting metal oxide systems include any single or multicomponent oxide system, especially those that are capable of promoting the reaction of a given active metal, and/or metal oxide, for a specific catalytic reaction.
- Suitable supporting metal oxides thus include lanthanide oxide systems (including, but not limited to, those of lanthanum, cerium, gadolinium, neodymium and praeseodymium), transition metal oxides (including, but not limited to, those of yttrium, zirconium, iron, palladium, nickel, titanium and chromium) and even oxides of main group metals (including, but not limited to, magnesium and aluminium).
- the process according to the invention may be used to prepare mixed oxides and solid solutions of two or more of the abovementioned metals.
- Particularly preferred metal oxide systems include those which are promoters (e.g. promotors of redox rections), for example those of cerium, zirconium, yttrium and mixtures of such oxide systems.
- the process of the invention may be used to prepare, at low temperatures, supported metal/metal oxide systems in which the supporting metal oxide system possesses a high degree of accuracy in the desired compositional stoichiometry and a minimal point defect concentration.
- the wet gel comprising the hydrous metal oxide may be formed (step (a)) by heating a mixture of wet hydrous oxide system and reducible metal salt, in the desired proportions. It is preferred that the heating is performed under atmospheric pressure (i.e. in an open atmosphere, rather than in a sealed vessel).
- the mixture may be heated such that it is dried up to a specific, or critical, oxide:free water ratio, which ratio depends upon the hydrous metal oxide(s) that is/are employed.
- critical ( ⁇ iinimum) amount of water that must be present in the wet gel depends upon the oxide system that is used, it can be determined non- inventively by the skilled person as the minimum amount of free water that must be present in the resultant gel that will enable deaggregation during the course of carrying out the next step in the process of the invention (step (b)).
- the mixture may be heated until it is sufficiently dried such that it forms a gel which, depending upon the metal oxide system that is employed in the first instance, may include drying until the gel so formed is of a soft and/or crumbly consistency or drying to a constant weight (i.e. no free water).
- a constant weight i.e. no free water.
- systems comprising cerium oxide and aluminium oxide may be dried to a constant weight (though this is not critical).
- Systems comprising other oxides e.g. those of zirconium and titanium
- may be dried to form a gel with a soft and/or crumbly consistency which may comprise e.g. 60 to 70% water (lattice and combined) based on the total weight of the gel).
- the temperature at, and length of time over, which the mixture should be heated will depend upon factors such as the composition of the mixture and the degree of hydration (i.e. "wetness") of the hydrous metal oxide.
- suitable temperatures are in the range room temperature to 120°C, preferably 40 to 110°C and more preferably 55 to 110°C (e.g. 105°C)
- suitable time periods are in the range 1 to 24, preferably 1 to 6, more preferably 1.5 to 5 and especially 1.75 to 4.5 hours.
- reducible metal salts that may be employed in the process of the invention include any salt of a metal in which the oxidation state of that metal may be lowered using conventional reducing techniques.
- suitable salts include metal nitrates, metal chlorides, metal perchlorates, metal acetates, metal carbonates and higher metal oxides.
- the reducible metal salt is a metal nitrate or a metal chloride.
- wet hydrous metal oxides and reducible metal salts are commercially available, are well known in the literature or are readily available using techniques which are well known to those skilled in the art, such as those described hereinafter.
- Appropriate vessels which may be used to heat the mixtare to form the wet gel (step (a)) will be well known to those skilled in the art and include standard evaporating dishes made from an appropriate material (e.g. pyrex).
- the product of step (a) may be heated (step (b)) in a suitable atmosphere e.g. a furnace or a controlled pressure/water atmosphere by, for example, sealing in an appropriate reaction vessel (e.g. a pressure reactor vessel (e.g. an autoclave) or a hydrothermal reactor).
- a suitable atmosphere e.g. a furnace or a controlled pressure/water atmosphere by, for example, sealing in an appropriate reaction vessel (e.g. a pressure reactor vessel (e.g. an autoclave) or a hydrothermal reactor).
- a reaction vessel e.g. a pressure reactor vessel (e.g. an autoclave) or a hydrothermal reactor).
- the reaction vessel may be composed of appropriate materials, which may depend upon the constituents of the we
- the wet gel may, for example, be heated to the decomposition temperature of the salt. This is typically in the region of 220 to 330°C, for example 305 to 320°C, for metal nitrates and metal chlorides. Suitable heating rates are in the region 10 to 500 °C per hour, for example 200 °C per hour.
- the wet gel may be heated for between 1 and 60 minutes, preferably 10 to 30 minutes at the appropriate temperature, depending on the hydrous metal oxide system that is used and the total mass.
- the decomposition of the reducible salt as appropriate may be monitored via an appropriate means (e.g., in the case of an autoclave, by observing the presence of an endotherm by means of a temperature gauge, and/or an increase in pressure on a pressure gauge).
- the heating step (b) may also be carried out in a furnace (e.g. a muffle furnace), or in an open atmosphere. Suitable heating rates are in the region 10 to 500°C per hour, for example 200°C per hour, and a heating time of between 1 and 180 minutes, preferably 30 to 120 minutes, depending on the hydrous metal oxide system that is used and the total mass.
- a furnace e.g. a muffle furnace
- Suitable heating rates are in the region 10 to 500°C per hour, for example 200°C per hour, and a heating time of between 1 and 180 minutes, preferably 30 to 120 minutes, depending on the hydrous metal oxide system that is used and the total mass.
- step (b) the reducible metal salt is decomposed and is substantially in the form of a reducible metal oxide that is present within the supporting metal oxide matrix. Further, the product of step (b) is preferably deaggregated, and in the form of nanocrystals.
- the reduction step (c) may be performed using standard reduction techniques, which are known to those skilled in the art, for example reduction in a suitable reducing atmosphere (e.g. H 2 in N 2 ; such as 5% H 2 /N 2 ) at an appropriate pressure (e.g. atmospheric pressure) and temperature (e.g. 800°C to 1000°C).
- a suitable reducing atmosphere e.g. H 2 in N 2 ; such as 5% H 2 /N 2
- an appropriate pressure e.g. atmospheric pressure
- temperature e.g. 800°C to 1000°C
- Products obtainable by the process of the invention may be dispersed into an appropriate solvent to form a sol, which may then be used to coat or impregnate a variety of substrates in order to yield a coating which is nanocrystalline in nature.
- products may be dispersed onto a catalyst support to form a catalyst.
- Other layered materials comprising coated substrates may be readily produced in a similar fashion. It will be appreciated by the skilled person that the process of the invention offers the flexibility that the reduction step (c) may be performed before or after dispersion on a substrate.
- Products obtainable by the process of the invention have the advantage that, following the reduction step (c), metals/metal oxides may be dispersed substantially to entirely on the surface of a metal oxide system (e.g. a promoter or stabilising oxide).
- a metal oxide system e.g. a promoter or stabilising oxide.
- the process of the invention has advantages over standard active metal/metal oxide deposition techniques described hereinbefore, which prior art techniques result in a lower proportion of active metal/metal oxide being dispersed on the promoting oxide system (see Figure 1).
- the process of the invention may result in catalyst products in which less than 1 % (e.g. none) of the metal/metal oxide is presented on the catalyst support, and thus catalyst products possessing a higher surface area of active metal/metal oxide. This may greatly increase the catalyst efficiency and lifetime of the resultant catalyst.
- the process of the invention also has the advantage that a wide variety of cheap, readily available inorganic precursors may be used.
- Figure 1 illustrates the structural differences between a catalyst produced using the process of the invention, and according to the prior art.
- Figure 2 shows an x-ray diffraction pattern for (a) Ce 075 Zr 0 2 Pto 05 O 2- ⁇ sol dried at 100°C, and (b) the same gel following reduction at 850 °C for 3 hours in 5% H 2 /N 2 .
- Figure 3 shows an x-ray diffraction pattern for (a) sol dried at 100°C, and (b) the same gel following reduction at 850°C for 3 hours in 5% H 2 /N 2 .
- Figure 4 shows an x-ray diffraction pattern for (a) s °l dried at 100°C, and (b) the same gel following reduction at 850°C for 3 hours in 5% H 2 /N 2 . Characterisation
- Ce(N0 3 ) 3 .6H 2 0 50 g was added to 250 mL of distilled water and dissolved at room temperature. Separately, cone, ammonia solution (880 s.g.; 30 g) and hydrogen peroxide solution (27.5% wt.; 17.5 g) were dissolved in 150 mL of distilled water and were added rapidly to the cerium solution with stirring. Stirring was continued for 5 minutes to give a deep red/orange precipitate. The mixtare was diluted to 750 mL with distilled water and centrifuged at 2000 rpm for 5 minutes, removing the supernatant.
- the resultant solid was washed with 4 x 750 mL of distilled water, with centrifuging in between to remove all anions and excess precipitating reagents. Finally, the precipitate was slurried to a 250 mL total volume, and 2M HN0 3 was added drop wise with stirring until a pH value of 6 was attained. Heating of the resultant mixture to 50 °C with stirring resulted in a banana yellow precipitate. Centrifuging at 3000 rpm for 5 rninutes, and removal of the supernatant, yielded a crystalline ceria hydrate with a primary crystallite size of 20 A.
- a zirconium oxynitrate solution was prepared made by adding ZrO(C0 3 ) 2 .xH 2 0 powder (7.67 g) to 15 mL of distilled water and mixing to a thin slurry. Cone. HN0 3 acid (5 g) was then added and the resultant mixed until the fizzing stopped. The mixture was then heated briefly to give a clear solution. Separately, H 2 PtCl 6 .xH 2 0 (3.2 g) was added to 10 mL of distilled water containing 2 drops of cone. HN0 3 acid and dissolved. The platinum salt solution was then added drop wise with stirring to the zirconia solution to give a deep red/orange solution.
- the sol was orange, transparent and stable, and consisted of single phase crystalline fluorite structured nano- particles (see Figure 2(a)) with an average particle size of about 10 nm and a primary crystallite size of about 5 nm.
- This sol was used to impregnate a suitable high surface area and porous support ( ⁇ -Al 2 0 3 ), dried and fired to 600 °C for 30 minutes.
- the catalyst was then activated by reduction at 850 °C for 2 hours in 5% H 2 /N 2 , producing platinum metal finely dispersed on the surface of Ce 08 Zr 0.2 0 2-x ⁇ nanocrystals, which in turn were dispersed on ⁇ -Al 2 0 3 .
- Figure 2(b) which shows the X-Ray diffraction pattern of the reduced undispersed nanocrystals.
- La(N0 3 ) 3 .5H 2 0 (8.47 g) was added to 15 mL of water and dissolved. To this, Cu(N0 3 ) 2 .3H 2 0 (1.645 g) was added and dissolved. The solution was added to 25 g of ceria hydrate (75.4% Ce0 2 ; see Example l(i) above) mixed thoroughly and dried to constant weight at 60°C. The dried mixtare was lightly crushed and placed in a pyrex beaker to a bed depth of 1.5 cm. The mixture was then heated to 310°C for 40 minutes at a heating rate of 200°C/hr. The resulting gravel was ground to a dark green powder and added, with stirring, to 800 mL of distilled water.
- ceria hydrate 75.4% Ce0 2 ; see Example l(i) above
- the stirring was continued for 30 minutes. Any non-dispersible solids ( ⁇ 5%) were removed by centrifuging at 4000 rpm for 10 minutes to leave an olive green transparent sol.
- the sol consisted of single phase fluorite nanocrystals with 10 to 15 nm particle size and a primary crystallite size of 5 nm (see Figure 3(a)). This sol was then used to impregnate a suitable high surface area and porous support ( ⁇ -Al 2 0 3 ), dried and fired to 600 °C for 30 minutes.
- the catalyst was then activated by reduction at 850 °C for 2 hours in 5% H 2 /N 2 , to produce a fine dispersion of copper metal on the surface of Ce 0.75 Lao .
- zirconium basic carbonate Small quantities of zirconium basic carbonate (total quantity 60 g) were added to 6M HN0 3 (43 mL). A further portion of zirconium basic carbonate (40 g) was then slurried with water before adding to the acid mixture. The mixture was heated with stirring and after 10 to 15 minutes a clear sol developed. After diluting with distilled water (500 mL) and stirring for 20 minutes, the mixture was allowed to cool to room temperature. 880 ammonia (23 mL) was then added to water (880 mL) with stirring. The zirconium sol was added slowly to this mixtare over 10 minutes with stirring. The resultant was allowed to settle and the supernatant decanted off. The sol was washed 4 times with 2 L of distilled water.
- the resultant gel was decanted to 900 mL, and 100 mL of HN0 3 was added. The mixture was centrifuged and the supernatant discarded to leave acid conditioned ZrO(OH) 2 .xH 2 0 hydrate gel.
- the resulting slurry was dried to a soft crumbly gel at 40 °C (about 70% water by weight) and placed in a sealed reactor vessel.
- the vessel was heated to 295 to 300°C for 15 minutes and pressure was released after this time from 1020 psi to 600 psi (72 to 43 bar) quickly to remove excess nitric acid.
- the rector vessel was then cooled to room temperature quickly and the product added to 900 mL of distilled water and stirred for 1 hour to give a brown/beige translucent sol. Any non-dispersible product was again centrifuged off at 4000 m for 10 rninutes.
- the resultant sol was transparent and beige in colour, and consisted of single phase cubic stabilised zirconia nanocrystals containing rhodium within the lattice (see Figure 4(a)).
- the average particle size of the sol was about 20 nm with a primary crystallite size of about 8 to 9 nm.
- This sol was used to impregnate a suitable support ( ⁇ -Al 2 0 3 ), and dried and fired to 600°C for 30 minutes.
- the powder was then reduced at 900 °C for 3 hours in 5% H 2 /N 2 to produce highly dispersed rhodium metal entirely on the surface of yttria stabilized zirconia nanocrystals in turn dispersed on gamma alumina.
- the x-ray diffraction pattern of the undispersed material is shown in Figure 4(b).
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Abstract
There is provided a process for the production of a product comprising nanocrystalline particles, which particles comprise at least one metal, or at least one metal oxide, substantially dispersed on the surface of at least one metal oxide, or mixed metal oxide, which process includes the steps of (a) heating a mixture including at least one wet hydrous metal oxide, or wet hydrous mixed metal oxide, and at least one reducible metal salt to form a wet gel; (b) heating the wet gel to the decomposition temperature of the reducible metal salt; and (c) reducing the resultant composition.
Description
PREPARATION OF NANOCRYSTALLINE AND DISPERSIBLE SUPPORTED METAL CATALYSTS
Field of the Invention
The present invention relates to the field of the preparation of supported metal and metal oxide products, particularly catalysts.
Background
For many years, it has been known that suitably-doped ceria and zirconia solid solutions are exceptional oxygen ion conductors.
This is because the lower or higher valent dopant, for example Ln3+, Y3+ or Zr4+ (wherein Ln represents a lanthanide metal), creates oxygen ion vacancies in the fluorite lattice, thus allowing facile oxygen ion transport within the lattice to the surface.
The resultant ability of these compounds to take up and release oxygen in response to the atmospheric partial pressure of oxygen, has been put to use extensively in catalysis. Here, an "active" (i.e. catalytic) metal (or metal oxide) on the surface of an oxygen ion conductor catalyses redox reactions with atmospheric gases. An example of this is in exhaust emission control (catalytic converters), where oxygen may react with CO gas, or unbumed hydrocarbons, to form C02 and water (oxidation), and where NO may react with CO to produce N2 and C02 (reduction/oxidation) .
The ability of the oxide ion conductor (the "promoting" oxide ion conductor) supporting the active metal/metal oxide in such a system to release oxygen under reducing conditions (acceleration), and to take up oxygen under oxidizing conditions (deceleration), has a direct effect upon the size of the window of oxygen partial pressures over which the active metal (e.g. Pt, Rh or Pd) is effective.
Recently, it has been shown (see, for example, J. Catal , (1997) 169, 490, Catalysis Letts. , (1998) 50, 193, Applied Catalysis B - Environmental (1998) 16, 105 and J. Catal. , 175, 269) that ceria-zirconia solid solutions of the formula Ce1-xZrx02-x/2, in the ceria rich region (i.e. those in which x = 0.15 to 0.50), are the most effective presently known redox promoters when operating at low temperatures (engine cold start). When an appropriate active metal is dispersed on their surface, these ceria-zirconia compounds have been found to greatly reduce emissions of CO, NOx and hydrocarbons.
It follows that catalytic efficiency relies on the high dispersion of active metal on the promoter alone.
Currently available techniques for coating active metals onto metal oxide supports, namely washcoating and dispersion techniques, involve dispersing promoter oxide powders (> 1 um particle size) within high surface area supports e.g. γ-Al203, and then dispersing the active metal onto this combined washcoat. This results in the problem that a large proportion of the expensive active metal particles are dispersed on the alumina support (see Figure 1), thereby reducing the efficiency of the catalyst (in that a greater proportion is "unpromoted"), and the lifetime of
the catalytic system (a metal catalyst may sinter more readily on a support such as alumina).
In international patent application PCT/GB98/01355 (WO 98/51617), techniques for the production of metal oxide gel products as nanocrystalline aqueous dispersions (particle sizes, for example, in the range 5 to 50 nm), using cheap inorganic starting materials, are disclosed.
We have now found that this technique may be modified by including at least one reducible salt of an active metal in the initial reaction mixture in order to produce an aqueous dispersion of individual crystalline nanoparticles contøining both the active metal/metal oxide and the promoter as a single phase. We have also found, surprisingly, that simple reduction of these nanocrystals results in the active metal/metal particles being substantially dispersed on the surface of the promoter oxide. This results in a process that may be employed in the preparation of inter alia improved catalyst products.
Disclosure of the Invention
According to the invention, there is provided a process for the production of a product comprising nanocrystalline particles, which particles comprise at least one metal, or at least one metal oxide, substantially dispersed on the surface of at least one metal oxide, or mixed metal oxide, which process includes the steps of:
(a) heating a mixture including at least one wet hydrous metal oxide, or wet hydrous mixed metal oxide, and at least one reducible metal salt, to form a wet gel;
(b) heating the wet gel to the decomposition temperature of the
reducible metal salt; and (c) reducing the resultant composition, which process is referred to hereinafter as "the process of the invention".
In the process of the invention, process steps (a), (b) and (c) are preferably carried out in the above order.
Although the process of the invention may be used to prepare particles that are substantially nanocrystalline in nature (i.e. up to 100% of the individual, unagglomerated crystallites have a particle size of less than 500 nm (e.g. less than 250 nm, preferably less than 50 nm)), as used herein, the term "nanocrystalline" particles, includes that no more than 1 % of particles produced via the process of the invention are non-crystalline, and/or that no more than 1 % of particles produced via the process of the invention exceed a particle size of 500 nm, and in which the average crystallite sizes (Zav) are in the range 3 to 250 nm (e.g. 4 to 100 nm and preferably 10 to 30 nm).
By "substantially" dispersed, we include that at least 40%, preferably at least 60%, and more preferably at least 80%, of the relevant metal or metal oxide (as appropriate) is presented, e.g. as particles, on the surface of the metal oxide support, as opposed to within the matrix thereof.
The term "wet" hydrous metal oxides, and mixed metal oxides, includes systems comprising a hydrous metal oxide and water, wherein the combined lattice water and/or free water content, is present in excess of 10% w/w, and preferably between 10 and 200% w/w, of the metal oxide system, whether coordinated to the metal ions of the metal oxide system or otherwise.
The term "wet gel" as used herein includes a gel system containing a metal oxide, lattice water and, optionally, depending upon the oxide system that is employed, excess free water, wherein any excess free water that is present, is present in an excess of between 0 and 95 % , preferably 0 and 70% , and especially 0 and 60% , w/w of the total weight of the gel.
We have found that step (b) of the process of the invention results in the production of deaggregated material. Thus, the heating step (b) may preferably be carried out until the reducible metal salt is decomposed and/or the product is deaggregated.
The product of step (b) may preferably be dispersed onto a suitable substrate (e.g. a high surface area support) before or after carrying out the reduction step (c). This dispersion may be achieved by dispersing the product of step (b) into a suitable medium (e.g. an aqueous solvent, such as distilled water), casting the resultant mixture onto the relevant substrate and drying as necessary.
Any non-dispersible product which may be formed following step (b) may be removed using conventional techniques. By "non-dispersible product" we include product, which is of a particle size which is too great to allow it to enter the colloidal state. For example, non-dispersible product may be removed by dispersing the product of step (b) as described above to form a sol. In such an instance, dispersion may take place with stirring over an appropriate period (e.g. approximately 1 hour) followed by standing over 2 hours. Any non-dispersible sediment may then be removed by an appropriate means (e.g. decanting the supernatant). The resultant sol, which may or may not be dialysed using techniques known
to those skilled in the art in order to remove any excess anions, may comprise a single phase nanocrystalline solid solution (i.e. it does not comprise particles of a size of greater than 500 nm, preferably greater than 250 nm, once the non-dispersible product is removed).
The nanocrystals may then be dispersed onto an appropriate substrate (e.g. γ-Al203) before carrying out the reduction step (c).
Alternatively, the reduction step (c) may be performed directly after step (b), and any non-dispersible product may then be removed by dispersing the product of step (c) into a solvent to form a sol in the above-described manner. Again, the resultant nanocrystals comprising reduced metal, or metal oxide, may then be dispersed onto an appropriate substrate (e.g. γ- A1203).
We have found, surprisingly, that reduction step (c) results in reduced metal migrating to, and being presented on, the surface of the metal oxide particles. Such metals may or may not re-oxidise (or partially re-oxidise), if subjected to an oxygen-containing atmosphere (such as air), once they have migrated to the surface such that a metal oxide (and/or mixed metal/metal oxide) is presented on the surface of the metal oxide particles (though this surface re-oxidation may be prevented if the product of step (c) is kept in a reducing environment). In this respect, the process of the invention finds particular utility in the production of products (e.g. catalysts) in which an active metal, or active metal oxide, is supported on (i.e. dispersed, or presented, on the surface of) a metal oxide (e.g. a promoter or stabilising oxide, or a solid solution of metal oxides).
Thus, the process of the invention may be used to form products
comprising a wide variety of metals or metal oxides, which are supported on metal oxide systems, mixed metal oxide systems, and/or metal oxide hydrate systems. In particular, any "active" metal (e.g. transition metal) or "active" metal (e.g. transition metal) oxide that is capable of catalysing a chemical reaction to a experimentally determinable degree may be employed in the process of the invention. Suitable active metals, include palladium, platinum, rhodium, copper, iron, chromium, silver, cobalt, ruthenium and nickel and suitable active metal oxides include those of copper.
Suitable supporting metal oxide systems include any single or multicomponent oxide system, especially those that are capable of promoting the reaction of a given active metal, and/or metal oxide, for a specific catalytic reaction. Suitable supporting metal oxides thus include lanthanide oxide systems (including, but not limited to, those of lanthanum, cerium, gadolinium, neodymium and praeseodymium), transition metal oxides (including, but not limited to, those of yttrium, zirconium, iron, palladium, nickel, titanium and chromium) and even oxides of main group metals (including, but not limited to, magnesium and aluminium). Moreover, the process according to the invention may be used to prepare mixed oxides and solid solutions of two or more of the abovementioned metals. Particularly preferred metal oxide systems include those which are promoters (e.g. promotors of redox rections), for example those of cerium, zirconium, yttrium and mixtures of such oxide systems.
We have found that the process of the invention may be used to prepare, at low temperatures, supported metal/metal oxide systems in which the supporting metal oxide system possesses a high degree of accuracy in the
desired compositional stoichiometry and a minimal point defect concentration.
Thus, according to a further aspect of the invention, there is provided a product obtainable by the process of the invention.
In the process of invention, the wet gel comprising the hydrous metal oxide may be formed (step (a)) by heating a mixture of wet hydrous oxide system and reducible metal salt, in the desired proportions. It is preferred that the heating is performed under atmospheric pressure (i.e. in an open atmosphere, rather than in a sealed vessel).
In the formation of the wet gel, the mixture may be heated such that it is dried up to a specific, or critical, oxide:free water ratio, which ratio depends upon the hydrous metal oxide(s) that is/are employed. Although the critical (πiinimum) amount of water that must be present in the wet gel depends upon the oxide system that is used, it can be determined non- inventively by the skilled person as the minimum amount of free water that must be present in the resultant gel that will enable deaggregation during the course of carrying out the next step in the process of the invention (step (b)). For example, the mixture may be heated until it is sufficiently dried such that it forms a gel which, depending upon the metal oxide system that is employed in the first instance, may include drying until the gel so formed is of a soft and/or crumbly consistency or drying to a constant weight (i.e. no free water). For example, systems comprising cerium oxide and aluminium oxide may be dried to a constant weight (though this is not critical). Systems comprising other oxides (e.g. those of zirconium and titanium) may be dried to form a gel with a soft and/or crumbly consistency (which may comprise e.g. 60 to 70% water (lattice
and combined) based on the total weight of the gel). The temperature at, and length of time over, which the mixture should be heated will depend upon factors such as the composition of the mixture and the degree of hydration (i.e. "wetness") of the hydrous metal oxide. However, suitable temperatures are in the range room temperature to 120°C, preferably 40 to 110°C and more preferably 55 to 110°C (e.g. 105°C), and suitable time periods are in the range 1 to 24, preferably 1 to 6, more preferably 1.5 to 5 and especially 1.75 to 4.5 hours.
The skilled person will appreciate that reducible metal salts that may be employed in the process of the invention include any salt of a metal in which the oxidation state of that metal may be lowered using conventional reducing techniques. Thus, suitable salts include metal nitrates, metal chlorides, metal perchlorates, metal acetates, metal carbonates and higher metal oxides.
We prefer that the reducible metal salt is a metal nitrate or a metal chloride.
Appropriate wet hydrous metal oxides and reducible metal salts are commercially available, are well known in the literature or are readily available using techniques which are well known to those skilled in the art, such as those described hereinafter.
Appropriate vessels which may be used to heat the mixtare to form the wet gel (step (a)) will be well known to those skilled in the art and include standard evaporating dishes made from an appropriate material (e.g. pyrex).
The product of step (a) may be heated (step (b)) in a suitable atmosphere e.g. a furnace or a controlled pressure/water atmosphere by, for example, sealing in an appropriate reaction vessel (e.g. a pressure reactor vessel (e.g. an autoclave) or a hydrothermal reactor). The skilled person will appreciate that the reaction vessel may be composed of appropriate materials, which may depend upon the constituents of the wet gel.
The wet gel may, for example, be heated to the decomposition temperature of the salt. This is typically in the region of 220 to 330°C, for example 305 to 320°C, for metal nitrates and metal chlorides. Suitable heating rates are in the region 10 to 500 °C per hour, for example 200 °C per hour. The wet gel may be heated for between 1 and 60 minutes, preferably 10 to 30 minutes at the appropriate temperature, depending on the hydrous metal oxide system that is used and the total mass. The decomposition of the reducible salt as appropriate may be monitored via an appropriate means (e.g., in the case of an autoclave, by observing the presence of an endotherm by means of a temperature gauge, and/or an increase in pressure on a pressure gauge).
The heating step (b) may also be carried out in a furnace (e.g. a muffle furnace), or in an open atmosphere. Suitable heating rates are in the region 10 to 500°C per hour, for example 200°C per hour, and a heating time of between 1 and 180 minutes, preferably 30 to 120 minutes, depending on the hydrous metal oxide system that is used and the total mass.
Once step (b) has been carried out the reducible metal salt is decomposed and is substantially in the form of a reducible metal oxide that is present
within the supporting metal oxide matrix. Further, the product of step (b) is preferably deaggregated, and in the form of nanocrystals.
The reduction step (c) may be performed using standard reduction techniques, which are known to those skilled in the art, for example reduction in a suitable reducing atmosphere (e.g. H2 in N2; such as 5% H2/N2) at an appropriate pressure (e.g. atmospheric pressure) and temperature (e.g. 800°C to 1000°C).
Products obtainable by the process of the invention may be dispersed into an appropriate solvent to form a sol, which may then be used to coat or impregnate a variety of substrates in order to yield a coating which is nanocrystalline in nature. For example, products may be dispersed onto a catalyst support to form a catalyst. Other layered materials comprising coated substrates may be readily produced in a similar fashion. It will be appreciated by the skilled person that the process of the invention offers the flexibility that the reduction step (c) may be performed before or after dispersion on a substrate.
Products obtainable by the process of the invention have the advantage that, following the reduction step (c), metals/metal oxides may be dispersed substantially to entirely on the surface of a metal oxide system (e.g. a promoter or stabilising oxide). Thus, when the product to be prepared is a catalyst system, the process of the invention has advantages over standard active metal/metal oxide deposition techniques described hereinbefore, which prior art techniques result in a lower proportion of active metal/metal oxide being dispersed on the promoting oxide system (see Figure 1). Conversely, the process of the invention may result in catalyst products in which less than 1 % (e.g. none) of the metal/metal
oxide is presented on the catalyst support, and thus catalyst products possessing a higher surface area of active metal/metal oxide. This may greatly increase the catalyst efficiency and lifetime of the resultant catalyst.
The process of the invention also has the advantage that a wide variety of cheap, readily available inorganic precursors may be used.
Examples
The invention is illustrated, but in no way limited, by way of the following examples, in which:
Figure 1 illustrates the structural differences between a catalyst produced using the process of the invention, and according to the prior art.
Figure 2 shows an x-ray diffraction pattern for (a) Ce075Zr0 2Pto 05O2-δ sol dried at 100°C, and (b) the same gel following reduction at 850 °C for 3 hours in 5% H2/N2.
Figure 3 shows an x-ray diffraction pattern for (a)
sol dried at 100°C, and (b) the same gel following reduction at 850°C for 3 hours in 5% H2/N2.
Figure 4 shows an x-ray diffraction pattern for (a)
s°l dried at 100°C, and (b) the same gel following reduction at 850°C for 3 hours in 5% H2/N2.
Characterisation
Morphology and elemental analysis
This was carried out on dried gel or calcine samples using out a JEOL scanning electron microscope operating at 20 kV and equipped with an energy dispersive x-ray analyzer. Conducting samples were prepared by either carbon coating or gold sputtering finely ground powder specimens. Both broad beam and point EDX analysis of powder particles were performed using pure manganese as a reference standard.
X-ray powder diffraction patterns of the samples were recorded in the region of 2Θ = 10-80° with a scanning speed of 1/4° /min on a Philips diffractometer using CuKα radiation with a nickel filter. The average crystallite size of each composition was calculated from the broadening of a specific diffraction peak using the well-known Scherrer equation, D = kλ/hy2cosΘ, where D = average size of the crystallites, k = Scherrer constant, λ = wavelength of radiation, hV2 = peak width at half height and Θ corresponds to the peak position.
Particle Size
This was measured in solution by photon correlation spectroscopy or on solid samples by transition electron microscopy.
Example 1 Platinum Catalyst on a Ceria/Zirconia Solid Solution
(i) Ceria Hydrate
Ce(N03)3.6H20 (50 g) was added to 250 mL of distilled water and dissolved at room temperature. Separately, cone, ammonia solution (880
s.g.; 30 g) and hydrogen peroxide solution (27.5% wt.; 17.5 g) were dissolved in 150 mL of distilled water and were added rapidly to the cerium solution with stirring. Stirring was continued for 5 minutes to give a deep red/orange precipitate. The mixtare was diluted to 750 mL with distilled water and centrifuged at 2000 rpm for 5 minutes, removing the supernatant. The resultant solid was washed with 4 x 750 mL of distilled water, with centrifuging in between to remove all anions and excess precipitating reagents. Finally, the precipitate was slurried to a 250 mL total volume, and 2M HN03 was added drop wise with stirring until a pH value of 6 was attained. Heating of the resultant mixture to 50 °C with stirring resulted in a banana yellow precipitate. Centrifuging at 3000 rpm for 5 rninutes, and removal of the supernatant, yielded a crystalline ceria hydrate with a primary crystallite size of 20 A.
(ii) Platinum Catalyst on a Ceria/Zirconia Solid Solution
A zirconium oxynitrate solution was prepared made by adding ZrO(C03)2.xH20 powder (7.67 g) to 15 mL of distilled water and mixing to a thin slurry. Cone. HN03 acid (5 g) was then added and the resultant mixed until the fizzing stopped. The mixture was then heated briefly to give a clear solution. Separately, H2PtCl6.xH20 (3.2 g) was added to 10 mL of distilled water containing 2 drops of cone. HN03 acid and dissolved. The platinum salt solution was then added drop wise with stirring to the zirconia solution to give a deep red/orange solution. This was then added to 25 g of ceria hydrate (75.4% Ce02; from step (i) above), mixed thoroughly and dried to constant weight at 60°C. The mixtare was then lightly crushed and added to a pyrex beaker to a 1.5 cm bed depth. This was then heated in a muffle furnace to 260 °C for 2 minutes at a heating rate of 200°C/hr, removed from the furnace and cooled. The resultant orange powder was finely ground and added with
stirring to 850 mL of distilled water and stirred for 30 minutes. The resultant sol was then centrifuged for 10 minutes at 4000rpm to remove any non-dispersible product ( <5%). The sol was orange, transparent and stable, and consisted of single phase crystalline fluorite structured nano- particles (see Figure 2(a)) with an average particle size of about 10 nm and a primary crystallite size of about 5 nm. This sol was used to impregnate a suitable high surface area and porous support (γ-Al203), dried and fired to 600 °C for 30 minutes. The catalyst was then activated by reduction at 850 °C for 2 hours in 5% H2/N2, producing platinum metal finely dispersed on the surface of Ce08Zr0.202-x^ nanocrystals, which in turn were dispersed on γ-Al203. (See Figure 2(b), which shows the X-Ray diffraction pattern of the reduced undispersed nanocrystals.)
Example 2 A Highly Dispersed Cuprous Oxide Catalyst
La(N03)3.5H20 (8.47 g) was added to 15 mL of water and dissolved. To this, Cu(N03)2.3H20 (1.645 g) was added and dissolved. The solution was added to 25 g of ceria hydrate (75.4% Ce02; see Example l(i) above) mixed thoroughly and dried to constant weight at 60°C. The dried mixtare was lightly crushed and placed in a pyrex beaker to a bed depth of 1.5 cm. The mixture was then heated to 310°C for 40 minutes at a heating rate of 200°C/hr. The resulting gravel was ground to a dark green powder and added, with stirring, to 800 mL of distilled water. The stirring was continued for 30 minutes. Any non-dispersible solids ( <5%) were removed by centrifuging at 4000 rpm for 10 minutes to leave an olive green transparent sol. The sol consisted of single phase fluorite nanocrystals with 10 to 15 nm particle size and a primary crystallite size of 5 nm (see Figure 3(a)). This sol was then used to impregnate a suitable high surface area and porous support (γ-Al203), dried and fired to 600 °C
for 30 minutes. The catalyst was then activated by reduction at 850 °C for 2 hours in 5% H2/N2, to produce a fine dispersion of copper metal on the surface of Ce 0.75Lao.i5θ_- /2 nanocrystals which in turn were dispersed on γ -A1203. On exposure to air, the metal dispersion partially reoxidised to give a fine dispersion of Cu20 on nanocrystals of Ce0.75Lao .ι502-x/2, as can be seen in Figure 3(b) for the undispersed material.
Example 3
Rhodium Metal Catalyst on Yttria Stabilised Zirconia Nanocrystals
(i) Zirconia Hydrate Gel
Small quantities of zirconium basic carbonate (total quantity 60 g) were added to 6M HN03 (43 mL). A further portion of zirconium basic carbonate (40 g) was then slurried with water before adding to the acid mixture. The mixture was heated with stirring and after 10 to 15 minutes a clear sol developed. After diluting with distilled water (500 mL) and stirring for 20 minutes, the mixture was allowed to cool to room temperature. 880 ammonia (23 mL) was then added to water (880 mL) with stirring. The zirconium sol was added slowly to this mixtare over 10 minutes with stirring. The resultant was allowed to settle and the supernatant decanted off. The sol was washed 4 times with 2 L of distilled water. The resultant gel was decanted to 900 mL, and 100 mL of HN03 was added. The mixture was centrifuged and the supernatant discarded to leave acid conditioned ZrO(OH)2.xH20 hydrate gel.
(ii) Rhodium Metal Catalyst on Yttria Stabilised Zirconia Nanocrystals Yttrium nitrate pentahydrate (8.16 g) and Rh(N03)3.xH20 solution (13.21 % Rh; 2.07 g) were added to 15 mL of distilled water and dissolved to give an orange/red clear solution. This was added with mixing to a wet
zirconia hydrate gel (125 g; containing 10.5 g Zr02; from step (i) above) and homogenized in a high shear mixer for 2 to 3 minutes. The resulting slurry was dried to a soft crumbly gel at 40 °C (about 70% water by weight) and placed in a sealed reactor vessel. The vessel was heated to 295 to 300°C for 15 minutes and pressure was released after this time from 1020 psi to 600 psi (72 to 43 bar) quickly to remove excess nitric acid. The rector vessel was then cooled to room temperature quickly and the product added to 900 mL of distilled water and stirred for 1 hour to give a brown/beige translucent sol. Any non-dispersible product was again centrifuged off at 4000 m for 10 rninutes. The resultant sol was transparent and beige in colour, and consisted of single phase cubic stabilised zirconia nanocrystals containing rhodium within the lattice (see Figure 4(a)). The average particle size of the sol was about 20 nm with a primary crystallite size of about 8 to 9 nm. This sol was used to impregnate a suitable support (γ-Al203), and dried and fired to 600°C for 30 minutes. The powder was then reduced at 900 °C for 3 hours in 5% H2/N2 to produce highly dispersed rhodium metal entirely on the surface of yttria stabilized zirconia nanocrystals in turn dispersed on gamma alumina. The x-ray diffraction pattern of the undispersed material is shown in Figure 4(b).
Claims
1. A process for the production of a product comprising nanocrystalline particles, which particles comprise at least one metal, or at least one metal oxide, substantially dispersed on the surface of at least one metal oxide, or mixed metal oxide, which process includes the steps of: (a) heating a mixture including at least one wet hydrous metal oxide, or wet hydrous mixed metal oxide, and at least one reducible metal salt, to form a wet gel; (b) heating the wet gel to the decomposition temperature of the reducible metal salt; and (c) reducing the resultant composition.
2. A process as claimed in Claim 1, wherein- any non-dispersible product formed during steps (a) and/or (b) is removed by dispersing the product of step (b) into an aqueous solvent to form a sol, followed by removal of any non-dispersible sediment.
3. A process as claimed in Claim 1 or Claim 2, wherein the mixture of wet hydrous metal oxide, or mixed metal oxide, and reducible metal salt is heated at between room temperature and 120°C, and/or for between 1 and 24 hours.
4. A process as claimed in any one of the preceding claims, wherein the reducible metal salt is a metal nitrate, a metal chloride, a metal perchlorate, a metal acetate, a metal carbonate or a higher metal oxide.
5. A process as claimed in Claim 4, wherein the salt is a metal nitrate or a metal chloride.
6. A process as claimed in any one of the preceding claims, wherein the product of step (a) is heated in a controlled pressure/water atmosphere.
7. A process as claimed in Claim 6, wherein the product of step (a) is heated to between 220 and 330°C, and/or at a heating rate of between 10 and 500°C per hour, and/or for between 1 and 60 minutes.
8. A process as claimed in any one of Claims 1 to 5, wherein the product of step (a) is heated in a furnace or in an open atmosphere.
9. A process as claimed in Claim 8, wherein the product of step (a) is heated at a heating rate of between 10 and 500°C per hour, and/or for between 1 and 180 minutes.
10. A process as claimed in any one of the preceding claims, wherein the reduction is performed in 5% H2/N2, and/or at atmospheric pressure, and/or at 800°C to 1000°C.
11. A nanocrystalline product obtainable by a process as defined in any one of the preceding claims.
12. A process for the preparation of a coated or impregnated substrate, which comprises coating or impregnating a substrate with a product according to Claim 11.
13. A process for the preparation of a coated or impregnated substrate, which comprises a process as claimed in any one of Claims 1 to 10, but with the additional step that the product of step (b) is dispersed onto a substrate before or after carrying out step (c).
14. A process as claimed in Claim 12 or Claim 13, wherein the substrate is γ-Al203.
15. A product obtainable by a process as defined in any one of Claims 12 to 14.
16. A product as claimed in Claim 15, which is a catalyst.
17. A catalyst comprising a product as claimed in Claim 11, coated or impregnated on a catalyst support.
18. A catalyst comprising nanocrystalline particles, which particles comprise at least one active metal, or at least one active metal oxide, substantially dispersed on the surface of at least one supporting metal oxide, or supporting mixed metal oxide, and a catalyst support, wherein no more than 1 % of active metal/metal oxide is presented/dispersed on the catalyst support.
19. The use of a product according to Claim 11 in the manufacture of a catalyst.
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GBGB9824152.4A GB9824152D0 (en) | 1998-11-05 | 1998-11-05 | New product |
GB9824152 | 1998-11-05 | ||
PCT/GB1999/003657 WO2000027527A1 (en) | 1998-11-05 | 1999-11-04 | Preparation of nanocrystalline and dispersible supported metal catalysts |
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ATE357971T1 (en) | 2000-08-19 | 2007-04-15 | Umicore Ag & Co Kg | OXYGEN STORING MATERIAL BASED ON CEROXIDE, METHOD FOR ITS PRODUCTION AND USE IN EXHAUST GAS TREATMENT OF COMBUSTION ENGINES |
GB0120962D0 (en) * | 2001-08-30 | 2001-10-17 | Univ Dundee | "Sensor" |
FR2832328B1 (en) * | 2001-11-20 | 2004-10-29 | Centre Nat Rech Scient | HETEROGENIC CATALYST COMPOSED OF AN AGGREGATE OF METALLIZED NANOPARTICLES |
JP2005097642A (en) * | 2003-09-22 | 2005-04-14 | Tanaka Kikinzoku Kogyo Kk | Noble metal-metal oxide composite cluster |
GB0413771D0 (en) | 2004-06-21 | 2004-07-21 | Johnson Matthey Plc | Metal oxide sols |
GB0413767D0 (en) | 2004-06-21 | 2004-07-21 | Johnson Matthey Plc | Metal oxide sols |
WO2007052627A1 (en) | 2005-11-01 | 2007-05-10 | Nissan Motor Co., Ltd. | Catalyst for exhaust-gas purification and process for producing the same |
JP4265626B2 (en) | 2006-07-12 | 2009-05-20 | トヨタ自動車株式会社 | Catalyst carrier particles, method for producing the same, and exhaust gas purification catalyst |
EP1920830A1 (en) * | 2006-11-08 | 2008-05-14 | L'AIR LIQUIDE, Société Anonyme pour l'Etude et l'Exploitation des Procédés Georges Claude | Group VIII and ceria/zirconia containing catalysts for catalytic hydrocarbon reforming or oxidation |
DE102011108620B4 (en) * | 2011-07-22 | 2015-08-27 | Technische Universität Dresden | Method for producing a component for high-temperature applications, component produced by the method and its use |
FR2991713A1 (en) * | 2012-06-11 | 2013-12-13 | Air Liquide | EXHAUST GAS PURIFYING DEVICE OF A THERMAL MOTOR COMPRISING A FRACTIONAL NANOMETER-SCALE CERAMIC SUPPORT |
CN106470752A (en) * | 2014-03-21 | 2017-03-01 | Sdc材料公司 | For passive NOXThe compositionss of absorption (PNA) system |
CN117466251B (en) * | 2023-11-22 | 2024-04-05 | 山东科源生化有限公司 | Method for preparing yttrium perchlorate by utilizing rare earth yttrium oxide |
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GB9709449D0 (en) * | 1997-05-10 | 1997-07-02 | Univ Warwick | Low temperature production of metal oxides |
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