WO1979000233A1 - Method of catalysis,hydrogen produced by the method,and a porous electrode - Google Patents
Method of catalysis,hydrogen produced by the method,and a porous electrode Download PDFInfo
- Publication number
- WO1979000233A1 WO1979000233A1 PCT/GB1978/000027 GB7800027W WO7900233A1 WO 1979000233 A1 WO1979000233 A1 WO 1979000233A1 GB 7800027 W GB7800027 W GB 7800027W WO 7900233 A1 WO7900233 A1 WO 7900233A1
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- electrode
- compounds
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- nickel
- hydrogen
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- C—CHEMISTRY; METALLURGY
- C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
- C25B—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES FOR THE PRODUCTION OF COMPOUNDS OR NON-METALS; APPARATUS THEREFOR
- C25B11/00—Electrodes; Manufacture thereof not otherwise provided for
- C25B11/04—Electrodes; Manufacture thereof not otherwise provided for characterised by the material
- C25B11/051—Electrodes formed of electrocatalysts on a substrate or carrier
- C25B11/073—Electrodes formed of electrocatalysts on a substrate or carrier characterised by the electrocatalyst material
- C25B11/091—Electrodes formed of electrocatalysts on a substrate or carrier characterised by the electrocatalyst material consisting of at least one catalytic element and at least one catalytic compound; consisting of two or more catalytic elements or catalytic compounds
- C25B11/095—Electrodes formed of electrocatalysts on a substrate or carrier characterised by the electrocatalyst material consisting of at least one catalytic element and at least one catalytic compound; consisting of two or more catalytic elements or catalytic compounds at least one of the compounds being organic
Definitions
- POROUS ELECTRODE This invention relates to a method of catalysis, hydrogen produced by the method and to a porous electrode (intended to be suitable for evolving gas).
- the invention may be used in industrial catalysis, for example in producing hydrogen from brine or chlor-alkali solutions.
- Electrodes including a mixed cobalt/nickel oxide compound have been briefly described in UK Patent Specification No. 1461764, but it would be desirable to have electrodes with a higher activity. This invention arises from modifying that compound.
- the invention is a method of ccatalysis using, as a catalyst, particles whose surfaces (to a depth of at least 2 ⁇ X) are compounds between sulphur optionally including oxygen and at least two of cobalt, nickel, iron and manganese.
- evolution of gaseous hydrogen e.g. formed by electrolysing water
- Another aspect of the invention is operating an aqueous alkali electrolysis cell using the catalyst, preferably bonded together in porous fashion by a chemically inert polymeric binder, as a cathode, optionally permitting air to contact the cathode from time to time, in which cell hydrogen is evolved at the cathode.
- the invention in another aspect is an electrode made from particles whose surfaces (to a depth of at least 20 ⁇ ) are compounds between sulphur optionally including oxygen and at least two of cobalt, nickel, iron and manganese bonded together in porous fashion by a chemically inert polymeric binder.
- the compounds are preferably A x B 4-2x S 3.6 4 O 0.4-0 where x is from
- the binder may be polytetrafluoroethylene, and may represent from 1 to 10 parts (by weight) per 10 parts of the total compounds, preferably 2 to 6 parts.
- a most preferred electrode has 3 parts of polytetrafluoroethylene binding 10 parts of Co 2 NiS 4 .
- the compounds may be made by treating the corresponding oxides with a sulphur-bearing compound, e.g. H S.
- the oxides may themselves have been made by a method ensuring small particle size, for example freeze-drying, and are described in UK Patent Specification No. 1461764. The invention will now be described by way of example.
- Ni(NO 3 ) 2 .6H 2 O was sprayed onto liquid nitrogen.
- the frozen metallic salt solution was rapidly transferred to roundbottomed flasks containing liquid nitrogen and subjected to freeze-drying. After drying, the mixed nitrate powder was subjected to vacuum decomposition for three hours at 250oC followed by thermal treatment in hydrogen sulphide at 350oC for
- Co 2 NiS 4 which has a particle size in the region of 0.1 ⁇ m
- 3 parts of polytetrafluoroethylene in the form of a dispersion (60% PTFE content) sold by Imperial Chemical Industries of England under the trade mark ICI Fluon GPl, and with just enough de-ionised water to make into a paste-like slurry.
- the slurry was dispersed ultrasonically and then painted onto a 100 B.S. mesh nickel screen, allowed to dry in air for one hour at 100oC and then cured in air at 300oC for an hour.
- the cured assembly represents the desired electrode, and offered a Co 2 NiS 4 , loading of 15.6 mg (and 4.4mg polytetrafluoroethylene) per square centimetre.
- the electrode was held potentiostatically at -173mV with reference to a dynamic hydrogen electrode in 5M KOH at 70oC, with iR correction, an excessively large nickel screen being provided as anode.
- the electrode passed about 750mA/cm 2 .
- the electrode passed 1300mA/cm 2 . This recovery even after exposure to air, shown in both
- 150 ml of an aqueous solution contained 24.4g CoCl 2 .6H 2 O and 12.13g of NiCl 2 .6H 2 O. This solution was added with constant stirring to 100 ml of 5M KOH, and the pH was adjusted until chloride ion could not be detected in the filtrate and finally the clean precipitate was heated in an over (containing air) at 400oC for 21 hours, giving Co 2 NiO 4 .
- the Co 2 NiO 4 was heated to 500oC and exposed for 5 hours to excess hydrogen sulphide, thus giving Co 2 NiS 4 as was confirmed by analysis. In any event, it is the superficial composition (i.e. the top 20 ⁇ layer) which influences the electrode behaviour and whose composition must therefore be as defined.
- Example 1 Alternatively, and equally successfully, the freeze-drying method of Example 1 could have been used.
- the Co 2 NiS 4 was made into a slurry, painted onto a nickel screen and cured, in similar fashion to Example 1.
- the cured assembly represents the desired electrode, and in this case offered a Co 2 Nis 4 loading of 22mg (and 9.3 mg polytetrafluoroethylene) per square centimetre.
- the electrode was held potentiostatically at -300mV with reference to a dynamic hydrogen electrode in 5-M KOH at 70oC, with iR correction, an excessively large nickel screen being provided as the counter electrode (anode). As may be seen from Figure 2, the electrode was able to pass a current of 1150mA/cm 2 even after
- Example 1 was repeated with the difference that in making the paste-like slurry, methanol was used in place of the de-ionised water.
- the Co NiS, loading was also much higher, at about 40 to 60 mg/cm 2 on the electrode.
- the electrode was held potentiostatically at -75 eaV with reference to a reversible hydrogen electrode, at 70oC NaOH (but otherwise as in Example 1), and gave 250mA/cm 2 , (iR corrected) a significant improvement on mild steel cathodes.
- the electrode was held at 95oC in a typical chlor-alkali solution 15% NaOH+17%NaCl) and set to allow a steady 250mA/cm to pass.
- This current density was sustained for over 400 hours, with a reasonably steady half cell voltage (i.e. - 80mV with reference to a reversible hydrogen electrode).
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- Chemical & Material Sciences (AREA)
- Engineering & Computer Science (AREA)
- Chemical Kinetics & Catalysis (AREA)
- Electrochemistry (AREA)
- Materials Engineering (AREA)
- Metallurgy (AREA)
- Organic Chemistry (AREA)
- Electrodes For Compound Or Non-Metal Manufacture (AREA)
- Electrolytic Production Of Non-Metals, Compounds, Apparatuses Therefor (AREA)
Abstract
In chlor-alkali cells, the cathode may consist of a nickel screen carrying 15.6 mg Co2NiS4 bonded by 4.4 mg polytetrafluoroethylene per cm2.
Description
METHOD OF CATALYSIS, HYDROGEN PRODUCED BY THE METHOD, AND A
POROUS ELECTRODE This invention relates to a method of catalysis, hydrogen produced by the method and to a porous electrode (intended to be suitable for evolving gas). The invention may be used in industrial catalysis, for example in producing hydrogen from brine or chlor-alkali solutions.
Many electrolysers use planar or mesh electrodes and as such can only give low current densities. A porous electrode which could ensure that most of the electrode surfaces continue to function during gas evolution reaction would give significantly higher current densities. At present, in for example the field of alkali (including chlor-alkali) electrolysis, anodes can be such that the performance of a cell is limited by the cathode, at which hydrogen gas forms. Electrodes including a mixed cobalt/nickel oxide compound have been briefly described in UK Patent Specification No. 1461764, but it would be desirable to have electrodes with a higher activity. This invention arises from modifying that compound.
The invention is a method of ccatalysis using, as a catalyst, particles whose surfaces (to a depth of at least 2θX) are compounds between sulphur optionally including oxygen and at least two of cobalt, nickel, iron and manganese. For example, evolution of gaseous hydrogen (e.g. formed by electrolysing water) may be thus catalysed.
Another aspect of the invention is operating an aqueous alkali electrolysis cell using the catalyst, preferably bonded together in porous fashion by a chemically inert polymeric binder, as a cathode, optionally permitting air to contact the cathode from time to time, in which cell hydrogen is evolved at the cathode.
The invention in another aspect is an electrode made from particles whose surfaces (to a depth of at least 20Å) are compounds between sulphur optionally including oxygen and at least two of cobalt, nickel, iron and manganese bonded together in porous fashion by a chemically inert polymeric binder. The compounds are preferably AxB4-2xS3.6 4O0.4-0 where x is from
0.05 to 1.95 and where A and B are any different two of cobalt, nickel, iron and manganese, for example cobalt and nickel. The binder may be polytetrafluoroethylene, and may represent from 1 to 10 parts (by weight) per 10 parts of the total compounds, preferably 2 to 6 parts.
Thus, a most preferred electrode has 3 parts of polytetrafluoroethylene binding 10 parts of Co2NiS4. The compounds may be made by treating the corresponding oxides with a sulphur-bearing compound, e.g. H S. The oxides may themselves have been made by a method ensuring small particle size, for example freeze-drying, and are described in UK Patent Specification No. 1461764.
The invention will now be described by way of example.
In the accompanying drawings, Figure 1 is a graph illustrating performance obtained according to Example 1, and Figure 2 is a graph illustrating performance obtained according to Example 2. EXAMPLE 1
A 100 ml solution containing 39.49g of Co (NO3)2.6H2O and
19.79g of Ni(NO3)2.6H2O was sprayed onto liquid nitrogen. The frozen metallic salt solution was rapidly transferred to roundbottomed flasks containing liquid nitrogen and subjected to freeze-drying. After drying, the mixed nitrate powder was subjected to vacuum decomposition for three hours at 250ºC followed by thermal treatment in hydrogen sulphide at 350ºC for
8 hours, giving a compound approximating to Co2NiS4 , in practice about Co2NiS3 O0.4.
Ten parts of the Co2NiS4 , which has a particle size in the region of 0.1μm, were mixed with 3 parts of polytetrafluoroethylene, in the form of a dispersion (60% PTFE content) sold by Imperial Chemical Industries of Britain under the trade mark ICI Fluon GPl, and with just enough de-ionised water to make into a paste-like slurry. The slurry was dispersed ultrasonically and then painted onto a 100 B.S. mesh nickel screen, allowed to dry in air for one hour at 100ºC and then cured in air at 300ºC for an hour.
The cured assembly represents the desired electrode, and offered a Co2NiS4, loading of 15.6 mg (and 4.4mg polytetrafluoroethylene) per square centimetre.
The electrode was held potentiostatically at -173mV with reference to a dynamic hydrogen electrode in 5M KOH at 70ºC, with iR correction, an excessively large nickel screen being provided as anode. As may be seen from Figure 1, on the first day, the electrode passed about 750mA/cm2. After being exposed overnight to air at 250, however, the electrode passed 1300mA/cm2. This recovery even after exposure to air, shown in both
Examples, is an important advantage.
EXAMPLE 2
150 ml of an aqueous solution contained 24.4g CoCl2.6H2O and 12.13g of NiCl2.6H2O. This solution was added with constant stirring to 100 ml of 5M KOH, and the pH was adjusted until chloride ion could not be detected in the filtrate and finally the clean precipitate was heated in an over (containing air) at 400ºC for 21 hours, giving Co2NiO4.
The Co2NiO4 was heated to 500ºC and exposed for 5 hours to excess hydrogen sulphide, thus giving Co2NiS4 as was confirmed by analysis. In any event, it is the superficial composition (i.e. the top 20Å layer) which influences the electrode behaviour and whose composition must therefore be as defined.
Alternatively, and equally successfully, the freeze-drying method of Example 1 could have been used.
The Co2NiS4 was made into a slurry, painted onto a nickel screen and cured, in similar fashion to Example 1.
The cured assembly represents the desired electrode, and in this case offered a Co2Nis4 loading of 22mg (and 9.3 mg polytetrafluoroethylene) per square centimetre.
The electrode was held potentiostatically at -300mV with reference to a dynamic hydrogen electrode in 5-M KOH at 70ºC, with iR correction, an excessively large nickel screen being provided as the counter electrode (anode). As may be seen from Figure 2, the electrode was able to pass a current of 1150mA/cm2 even after
10 hours use. Initially, the current was somewhat lower, at about
1050mA/cm2; if the electrode was used and then left in air for 24 hours, the performance on resuming use was 850mA/cm2, rising to 1050mA/cm after about 6 hours. EXAMPLE 3
Example 1 was repeated with the difference that in making the paste-like slurry, methanol was used in place of the de-ionised water. The Co NiS, loading was also much higher, at about 40 to 60 mg/cm2 on the electrode. The electrode was held potentiostatically at -75 eaV with reference to a reversible hydrogen electrode, at 70ºC NaOH (but otherwise as in Example 1), and gave 250mA/cm2, (iR corrected) a significant improvement on mild steel cathodes.
In another experiment, the electrode was held at 95ºC in a typical chlor-alkali solution 15% NaOH+17%NaCl) and set to allow a steady 250mA/cm to pass. This current density was sustained
for over 400 hours, with a reasonably steady half cell voltage (i.e. - 80mV with reference to a reversible hydrogen electrode). These results suggest that the invention could be exploited in industry by, for example, providing an alternative to mild steel cathodes in chlor-alkali electrolysis.
Claims
1. A method of catalysis, using as catalyst, particles whose surfaces (to depth of at least 20A) are compounds between sulphur optionally including oxygen and at least two of cobalt, nickel, iron and manganese.
2. A method according to Claim 1, wherein what is catalysed is evolution of gaseous hydrogen.
3- A method according to Claim 2, wherein the hydrogen is formed by electrolysing water.
4. A method according to Claim 3, when performed by operating an aqueous alkali electrolysis cell, in which the hydrogen is evolved at the cathode, which comprises the catalyst.
5. A method according to Claim 4, wherein the cathode comprises said particles bonded together in porous fashion by a chemically inert polymeric binder.
6. A method according to Claim 4 or 5, wherein air is permitted to contact the cathode from time to time.
7. Hydrogen obtained by a method according to any of Claims 2 to 6.
8. An electrode made from particles whose surfaces (to a depth of at least 20A) are compounds between sulphur optionally including oxygen and at least two of cobalt, nickel, iron and manganese bonded together in porous fashion by a chemically inert polymeric binder.
9. An electrode as claimed in Claim 8, wherein the compounds are AxB4-2xS3.6 - 4O0.4 - 0 where x is from 0.05 to 1.95 and where A and B are any different two of cobalt, nickel, iron and manganese.
10. An electrode as claimed in Claim 9, wherein A is nickel, and B is cobalt.
11. An electrode as claimed in Claim 8, 9 or 10, wherein the binder is polytetrafluoroethylene.
12. An electrode as claimed in any of Claims 8 to 11, wherein the binder represents from 1 to 10 parts by weight per 10 parts of the total compounds.
13. An electrode as claimed in Claim 12, wherein the binder represents from 2 to 6 parts per 10 of the total compounds.
14. An electrode as claimed in Claim 13, wherein substantially 3 parts of polytetrafluoroethylene bind 10 parts of Co2NiS4.
15- An electrode as claimed in any of Claims 8 to 14, made by treating the corresponding oxide compounds with a sulphur-bearing compound such as H2S. l6. A method according to any of Claims 1 to 6 when performed using an electrode as claimed in any of Claims 8 to 15.
Priority Applications (2)
Application Number | Priority Date | Filing Date | Title |
---|---|---|---|
DE7878900178T DE2861417D1 (en) | 1977-10-25 | 1978-10-20 | Method of catalysing evolution of gaseous hydrogen in alkaline electrolysis of water |
JP50001978A JPS54500031A (en) | 1977-10-25 | 1978-10-20 |
Applications Claiming Priority (2)
Application Number | Priority Date | Filing Date | Title |
---|---|---|---|
GB44362/77 | 1977-10-25 | ||
GB44362/77A GB1556452A (en) | 1977-10-25 | 1977-10-25 | Catalysing hydrogen evolution |
Publications (1)
Publication Number | Publication Date |
---|---|
WO1979000233A1 true WO1979000233A1 (en) | 1979-05-03 |
Family
ID=10432927
Family Applications (1)
Application Number | Title | Priority Date | Filing Date |
---|---|---|---|
PCT/GB1978/000027 WO1979000233A1 (en) | 1977-10-25 | 1978-10-20 | Method of catalysis,hydrogen produced by the method,and a porous electrode |
Country Status (8)
Country | Link |
---|---|
US (1) | US4279713A (en) |
EP (1) | EP0006933B1 (en) |
BE (1) | BE871328A (en) |
CA (1) | CA1137921A (en) |
DE (1) | DE2861417D1 (en) |
GB (1) | GB1556452A (en) |
IT (1) | IT1108757B (en) |
WO (1) | WO1979000233A1 (en) |
Cited By (1)
Publication number | Priority date | Publication date | Assignee | Title |
---|---|---|---|---|
WO2017167373A1 (en) * | 2016-03-31 | 2017-10-05 | Siemens Aktiengesellschaft | A technique for in-situ anode activation by a cathode in an alkaline water electrolytic cell |
Families Citing this family (5)
Publication number | Priority date | Publication date | Assignee | Title |
---|---|---|---|---|
CA1113802A (en) * | 1980-09-02 | 1981-12-08 | William A. Armstrong | Mixed oxide oxygen electrode |
US4488578A (en) * | 1981-05-26 | 1984-12-18 | National Research Development Corporation | Prevention of hydrogen embrittlement of metals in corrosive environments |
US4547278A (en) * | 1984-08-10 | 1985-10-15 | Inco Alloys International, Inc. | Cathode for hydrogen evolution |
GB9405518D0 (en) * | 1994-03-21 | 1994-05-04 | Mupor Ltd | Porous metal composite body |
CN113174602B (en) * | 2021-04-30 | 2023-07-28 | 浙江大学杭州国际科创中心 | Preparation method of three-dimensional co-continuous macroporous heterostructure sulfide full-water-splitting catalyst |
Family Cites Families (3)
Publication number | Priority date | Publication date | Assignee | Title |
---|---|---|---|---|
GB1461764A (en) * | 1972-11-17 | 1977-01-19 | Nat Res Dev | Cobalt/nickel oxide catalysts |
US4035255A (en) * | 1973-05-18 | 1977-07-12 | Gerhard Gritzner | Operation of a diaphragm electrolylytic cell for producing chlorine including feeding an oxidizing gas having a regulated moisture content to the cathode |
US4035254A (en) * | 1973-05-18 | 1977-07-12 | Gerhard Gritzner | Operation of a cation exchange membrane electrolytic cell for producing chlorine including feeding an oxidizing gas having a regulated moisture content to the cathode |
-
1977
- 1977-10-25 GB GB44362/77A patent/GB1556452A/en not_active Expired
-
1978
- 1978-10-17 BE BE191174A patent/BE871328A/en not_active IP Right Cessation
- 1978-10-20 DE DE7878900178T patent/DE2861417D1/en not_active Expired
- 1978-10-20 WO PCT/GB1978/000027 patent/WO1979000233A1/en unknown
- 1978-10-24 IT IT69445/78A patent/IT1108757B/en active
- 1978-10-24 CA CA000314003A patent/CA1137921A/en not_active Expired
-
1979
- 1979-05-07 EP EP78900178A patent/EP0006933B1/en not_active Expired
- 1979-06-22 US US06/116,676 patent/US4279713A/en not_active Expired - Lifetime
Non-Patent Citations (3)
Title |
---|
CHEMICAL ABSTACTS, Vol. 82, published 16th June 1975, Columbus, Ohio, USA, BEHRET: "Electrocatalytic oxygen reduction with thiospinels and other sulfides of transition metals", Abstract No. 161804. * |
CHEMICAL ABSTRACTS, Vol. 82, published 21st April 1975, Columbus, Ohio, USA, BARESEL: "Transition metal chalcogenides as oxygen catalysts for fuel cells", Abstract No. 101137. * |
Electrochimica Acta, Vol. 23, pages 1023-1029, published October 1978, BEHRET: "Comparison of the reaction mechanisms of electrocatalytic oxygen reduction usingtransition metal thiospinels and chelates", see figure 2, page 1024. * |
Cited By (1)
Publication number | Priority date | Publication date | Assignee | Title |
---|---|---|---|---|
WO2017167373A1 (en) * | 2016-03-31 | 2017-10-05 | Siemens Aktiengesellschaft | A technique for in-situ anode activation by a cathode in an alkaline water electrolytic cell |
Also Published As
Publication number | Publication date |
---|---|
IT7869445A0 (en) | 1978-10-24 |
DE2861417D1 (en) | 1982-01-28 |
GB1556452A (en) | 1979-11-28 |
EP0006933B1 (en) | 1981-12-02 |
CA1137921A (en) | 1982-12-21 |
IT1108757B (en) | 1985-12-09 |
US4279713A (en) | 1981-07-21 |
EP0006933A1 (en) | 1980-01-23 |
BE871328A (en) | 1979-02-15 |
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