US20130256123A1 - Electrocatalyst for electrochemical conversion of carbon dioxide - Google Patents
Electrocatalyst for electrochemical conversion of carbon dioxide Download PDFInfo
- Publication number
- US20130256123A1 US20130256123A1 US13/437,766 US201213437766A US2013256123A1 US 20130256123 A1 US20130256123 A1 US 20130256123A1 US 201213437766 A US201213437766 A US 201213437766A US 2013256123 A1 US2013256123 A1 US 2013256123A1
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- electrocatalyst
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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
-
- 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
-
- 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
- C25B3/00—Electrolytic production of organic compounds
- C25B3/20—Processes
- C25B3/25—Reduction
-
- 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
Definitions
- the present invention relates to electrochemical catalysts, and particularly to an electrocatalyst for the electrochemical conversion of carbon dioxide to hydrocarbons, such as methanol and methane.
- the electrocatalyst for the electrochemical conversion of carbon dioxide includes a copper material supported on carbon nanotubes.
- the copper material may be pure copper, such that the pure copper forms 20 wt % of the electrocatalyst; or copper and ruthenium supported on the carbon nanotubes such that the copper forms 20 wt % of the electrocatalyst and the ruthenium forms 20 wt % of the electrocatalyst; or copper and iron supported on the carbon nanotubes such that the copper forms 20 wt % of the electrocatalyst and the iron forms 20 wt % of the electrocatalyst; or copper and palladium supported on the carbon nanotubes such that the copper forms 20 wt % of the electrocatalyst and the palladium forms 20 wt % of the electrocatalyst.
- the metal supported on carbon nanotubes is prepared using homogenous deposition-precipitation with urea.
- the electrocatalyst is prepared by first dissolving copper nitrate trihydrate (Cu(NO 3 ) 2 3H 2 O) in deionized water to form a salt solution. Carbon nanotubes are then added to the salt solution to form a suspension, which is then heated. A urea solution is added to the suspension to form the electrocatalyst in solution. The electrocatalyst is then removed from the solution.
- copper nitrate trihydrate Cu(NO 3 ) 2 3H 2 O
- iron nitrate monohydrate Fe(NO 3 ) 2 H 2 O
- RuCl 3 ruthenium chloride
- PdCl 2 palladium chloride
- the electrocatalyst for the electrochemical conversion of carbon dioxide to hydrocarbons, such as methanol and methane includes a copper material supported on carbon nanotubes.
- the copper material may be pure copper, such that the pure copper forms 20 wt % of the electrocatalyst; or copper and ruthenium supported on the carbon nanotubes such that the copper forms 20 wt % of the electrocatalyst and the ruthenium forms 20 wt % of the electrocatalyst; or copper and iron supported on the carbon nanotubes such that the copper forms 20 wt % of the electrocatalyst and the iron forms 20 wt % of the electrocatalyst; or copper and palladium supported on the carbon nanotubes such that the copper forms 20 wt % of the electrocatalyst and the iron forms 20 wt % of the electrocatalyst.
- the electrocatalyst is prepared by first dissolving copper nitrate trihydrate (Cu(NO 3 ) 2 3H 2 O) in deionized water to form a salt solution. Using exemplary quantities, the copper nitrate trihydrate is dissolved in about 220 mL of the deionized water and then stirred for about thirty minutes. Using the exemplary volume of deionized water given above, about one gram of carbon nanotubes (preferably single wall carbon nanotubes) are then added to the salt solution to form a suspension, which is then sonicated for about one hour and heated to a temperature of about 90° C. with stirring.
- copper nitrate trihydrate Cu(NO 3 ) 2 3H 2 O
- a urea solution is added to the suspension to form the electrocatalyst in solution.
- about 30 mL of an about 0.42 M aqueous urea solution may be added to the suspension (about 6 g of urea are added to the solution).
- the urea solution is added to the suspension in a drop-wise fashion.
- the urea solution and suspension are then maintained at a temperature of about 90° C. for about eight hours, with stirring.
- the electrocatalyst is then removed from the solution, preferably by first cooling the solution to room temperature, centrifuging the solution to separate out the electrocatalyst, and then washing and drying the catalyst at a temperature of about 110° C. overnight.
- the electrocatalyst may then be calcined at a temperature of about 450° C. for about four hours in an argon gas flow.
- the electrocatalyst is reduced at a rate of about 100 mL/min at a temperature of about 450° C. for about four hours in a gas flow of about 10% hydrogen in argon.
- the result is a solid powder having a particle size in the range of 3-60 nm.
- iron nitrate monohydrate Fe(NO 3 ) 2 H 2 O
- RuCl 3 ruthenium chloride
- PdCl 2 palladium chloride
- the carbon nanotubes preferably have diameters of about 3-60 nm, and may be prepared by a conventional deposition-precipitation method.
- each catalyst was tested in an electrochemical reactor system operated in phase mode.
- the electrochemical system was similar to a fuel cell test station.
- Humidified carbon dioxide was fed on the cathode side and 0.5M NaHCO 3 was used as an analyte on the anode side.
- Each electrocatalyst sample was dissolved in a solvent and painted or coated on one side of a solid polymer electrolyte (SPE) membrane, viz., a proton conducting Nafion® 117 membrane (manufactured by E.I. Du Pont De Nemours and Company of Delaware), with 60% Pt—Ru deposited on Vulcan® carbon (manufactured by Vulcan Engineering Ltd. of the United Kingdom) being used as an anode catalyst.
- SPE solid polymer electrolyte
- Permeation of sodium bicarbonate solution through the membrane provided the alkalinity required for the reduction reaction to occur. Feeding CO 2 in the gas phase greatly reduced the mass transfer resistance.
Abstract
Description
- 1. Field of the Invention
- The present invention relates to electrochemical catalysts, and particularly to an electrocatalyst for the electrochemical conversion of carbon dioxide to hydrocarbons, such as methanol and methane.
- 2. Description of the Related Art
- Over the past several decades, various electrode materials have been researched for the reduction of carbon dioxide (CO2) into different products, most notably formic acid, carbon monoxide (CO), methane and methanol. Conventional metals used in the research were provided in the form of high purity foils, plates, rotating discs, wires, beds of particles, tubes and mesh. These are all macroscopic materials. Thus, when compared to microscopic or nanoscopic materials, they all have relatively low surface areas and low conductivity electrical supports.
- It would be desirable to provide an electrocatalytic material formed on nanostructures, thus greatly increasing available reactive surface area and conductivity. Given the destructive nature of carbon dioxide as a greenhouse gas, increasing the efficiency of electrocatalysts to form benign hydrocarbons, such as methanol, is obviously quite important. Further, it would be desirable to not only increase the overall efficiency of the catalytic process, but also provide an electrocatalyst that operates under relatively low temperatures and in the range of atmospheric pressure.
- Thus, an electrocatalyst for the electrochemical conversion of carbon dioxide solving the aforementioned problems is desired.
- The electrocatalyst for the electrochemical conversion of carbon dioxide includes a copper material supported on carbon nanotubes. The copper material may be pure copper, such that the pure copper forms 20 wt % of the electrocatalyst; or copper and ruthenium supported on the carbon nanotubes such that the copper forms 20 wt % of the electrocatalyst and the ruthenium forms 20 wt % of the electrocatalyst; or copper and iron supported on the carbon nanotubes such that the copper forms 20 wt % of the electrocatalyst and the iron forms 20 wt % of the electrocatalyst; or copper and palladium supported on the carbon nanotubes such that the copper forms 20 wt % of the electrocatalyst and the palladium forms 20 wt % of the electrocatalyst. The metal supported on carbon nanotubes is prepared using homogenous deposition-precipitation with urea.
- The electrocatalyst is prepared by first dissolving copper nitrate trihydrate (Cu(NO3)2 3H2O) in deionized water to form a salt solution. Carbon nanotubes are then added to the salt solution to form a suspension, which is then heated. A urea solution is added to the suspension to form the electrocatalyst in solution. The electrocatalyst is then removed from the solution. In addition to dissolving the copper nitrate trihydrate (Cu(NO3)2 3H2O) in the deionized water, either iron nitrate monohydrate (Fe(NO3)2 H2O), ruthenium chloride (RuCl3), or palladium chloride (PdCl2) may also be dissolved in the deionized water to form the salt solution.
- These and other features of the present invention will become readily apparent upon further review of the following specification.
- The electrocatalyst for the electrochemical conversion of carbon dioxide to hydrocarbons, such as methanol and methane, includes a copper material supported on carbon nanotubes. The copper material may be pure copper, such that the pure copper forms 20 wt % of the electrocatalyst; or copper and ruthenium supported on the carbon nanotubes such that the copper forms 20 wt % of the electrocatalyst and the ruthenium forms 20 wt % of the electrocatalyst; or copper and iron supported on the carbon nanotubes such that the copper forms 20 wt % of the electrocatalyst and the iron forms 20 wt % of the electrocatalyst; or copper and palladium supported on the carbon nanotubes such that the copper forms 20 wt % of the electrocatalyst and the iron forms 20 wt % of the electrocatalyst.
- The electrocatalyst is prepared by first dissolving copper nitrate trihydrate (Cu(NO3)2 3H2O) in deionized water to form a salt solution. Using exemplary quantities, the copper nitrate trihydrate is dissolved in about 220 mL of the deionized water and then stirred for about thirty minutes. Using the exemplary volume of deionized water given above, about one gram of carbon nanotubes (preferably single wall carbon nanotubes) are then added to the salt solution to form a suspension, which is then sonicated for about one hour and heated to a temperature of about 90° C. with stirring.
- A urea solution is added to the suspension to form the electrocatalyst in solution. Using the exemplary quantities given above, about 30 mL of an about 0.42 M aqueous urea solution may be added to the suspension (about 6 g of urea are added to the solution). Preferably, the urea solution is added to the suspension in a drop-wise fashion. The urea solution and suspension are then maintained at a temperature of about 90° C. for about eight hours, with stirring.
- The electrocatalyst is then removed from the solution, preferably by first cooling the solution to room temperature, centrifuging the solution to separate out the electrocatalyst, and then washing and drying the catalyst at a temperature of about 110° C. overnight. The electrocatalyst may then be calcined at a temperature of about 450° C. for about four hours in an argon gas flow. Following calcination, the electrocatalyst is reduced at a rate of about 100 mL/min at a temperature of about 450° C. for about four hours in a gas flow of about 10% hydrogen in argon. The result is a solid powder having a particle size in the range of 3-60 nm.
- In addition to dissolving the copper nitrate trihydrate (Cu(NO3)2 3H2O) in the deionized water, either iron nitrate monohydrate (Fe(NO3)2 H2O), ruthenium chloride (RuCl3), or palladium chloride (PdCl2) may also be dissolved in the deionized water to form the salt solution. The carbon nanotubes preferably have diameters of about 3-60 nm, and may be prepared by a conventional deposition-precipitation method.
- In the following, each catalyst was tested in an electrochemical reactor system operated in phase mode. The electrochemical system was similar to a fuel cell test station. Humidified carbon dioxide was fed on the cathode side and 0.5M NaHCO3 was used as an analyte on the anode side. Each electrocatalyst sample was dissolved in a solvent and painted or coated on one side of a solid polymer electrolyte (SPE) membrane, viz., a proton conducting Nafion® 117 membrane (manufactured by E.I. Du Pont De Nemours and Company of Delaware), with 60% Pt—Ru deposited on Vulcan® carbon (manufactured by Vulcan Engineering Ltd. of the United Kingdom) being used as an anode catalyst. Permeation of sodium bicarbonate solution through the membrane provided the alkalinity required for the reduction reaction to occur. Feeding CO2 in the gas phase greatly reduced the mass transfer resistance.
- For the first electrocatalyst sample, using pure copper forming 20 wt % of the electrocatalyst, using the experimental reactor described above, at lower voltages (−0.5 V), no hydrocarbon was produced. Maximum faradaic efficiency for methanol was achieved at −1.5 V. Maximum faradaic efficiency for methane was achieved at −2.5 V. The overall results are given below in Table 1:
-
TABLE 1 Results of reduction of CO2 over 20% Cu/CNT Faradaic Faradaic Faradaic Faradaic Efficiency Efficiency Efficiency Efficiency Potential Current for for for for carbon vs. SCE/V density hydrogen methanol methane monoxide −0.5 0.40 0 0 0 0 −1.5 5.20 8.03 3.90 4.20 0 −2.5 14.40 68.76 1.45 6.60 9.43 −3.5 40.48 77.83 0.80 1.40 18.17 - For the second electrocatalyst sample, using copper and ruthenium supported on the carbon nanotubes such that the copper forms 20 wt % of the electrocatalyst and the ruthenium forms 20 wt % of the electrocatalyst, using the experimental reactor described above, at lower voltages (−0.5 V), no hydrocarbon apart from methanol was produced. Maximum faradaic efficiency (15.5%) for methanol was achieved at −1.5 V. The overall results are given below in Table 2:
-
TABLE 2 Results of reduction of CO2 over 20% Cu - 20% Ru/CNT Faradaic Faradaic Faradaic Efficiency Efficiency Efficiency Potential Current for for for carbon vs. SCE/V density hydrogen methanol monoxide −0.5 0.32 0 0 0 −1.5 8.40 8.00 15.50 0 −2.5 30.40 68.80 6.20 9.43 −3.5 75.20 77.80 1.30 18.17 - For the third electrocatalyst sample, using copper and iron supported on the carbon nanotubes such that the copper forms 20 wt % of the electrocatalyst and the iron forms 20 wt % of the electrocatalyst, using the experimental reactor described above, no hydrocarbon was detected in the working potential range. Instead, carbon monoxide was detected. The overall results are given below in Table 3:
-
TABLE 3 Results of reduction of CO2 over 20% Cu - 20% Fe/CNT Faradaic Faradaic Efficiency Efficiency Potential Current for for carbon vs. SCE/V density hydrogen monoxide −0.5 1.2 0 0 −1.5 14.1 13.6 0 −2.5 38.2 68.4 9.4 −3.5 78.8 89.8 8.3 - For the fourth electrocatalyst sample, using copper and palladium supported on the carbon nanotubes such that the copper forms 20 wt % of the electrocatalyst and the palladium forms 20 wt % of the electrocatalyst, using the experimental reactor described above, no hydrocarbon apart from formic acid was detected in the working potential range. At lower voltages (−0.5 V), no product was produced. Maximum faradaic efficiency (21.3%) of formic acid was achieved at −1.5 V. The overall results are given below in Table 4:
-
TABLE 4 Results of reduction of CO2 over 20% Cu - 20% Pd/CNT Faradaic Faradaic Faradaic Efficiency Efficiency Efficiency Potential Current for for formic for carbon vs. SCE/V density hydrogen acid monoxide −0.5 0.42 0 0 0 −1.5 7.6 8.0 9.5 0 −2.5 28.5 68.8 21.3 10.3 −3.5 54.2 73.8 18.2 9.8 - It is to be understood that the present invention is not limited to the embodiments described above, but encompasses any and all embodiments within the scope of the following claims.
Claims (18)
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US13/437,766 US20130256123A1 (en) | 2012-04-02 | 2012-04-02 | Electrocatalyst for electrochemical conversion of carbon dioxide |
US14/340,619 US9109293B2 (en) | 2012-04-02 | 2014-07-25 | Electrocatalyst for electrochemical conversion of carbon dioxide |
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Cited By (7)
Publication number | Priority date | Publication date | Assignee | Title |
---|---|---|---|---|
JP2015147990A (en) * | 2014-02-07 | 2015-08-20 | 日立化成株式会社 | Electrode, method of producing electrode, electrochemical reduction method and method of producing electrochemical reduction product |
WO2016054400A1 (en) * | 2014-10-01 | 2016-04-07 | Anne Co | Materials and methods for the electrochemical reduction of carbon dioxide |
EP3453062A4 (en) * | 2016-05-02 | 2020-01-01 | UT-Battelle, LLC | Electrochemical catalyst for conversion of co2 to ethanol |
US10844502B2 (en) | 2017-12-13 | 2020-11-24 | King Fahd University Of Petroleum And Minerals | Electrode and an electrochemical cell for producing propanol from carbon dioxide |
CN113943942A (en) * | 2021-11-09 | 2022-01-18 | 深圳先进技术研究院 | Carbon dioxide energy storage system driven by new energy electric energy and energy storage method |
WO2022072434A1 (en) * | 2020-09-30 | 2022-04-07 | Ut-Battelle, Llc | Alloy based electrochemical catalyst for conversion of carbon dioxide to hydrocarbons |
WO2024060687A1 (en) * | 2022-09-20 | 2024-03-28 | 中国石油化工股份有限公司 | Copper-carbon composite material, preparation method therefor and use thereof |
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US20140174916A1 (en) * | 2012-12-26 | 2014-06-26 | King Abdulaziz City For Science And Technology | Catalytic composition for the electrochemical reduction of carbon dioxide |
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US6809229B2 (en) | 1999-01-12 | 2004-10-26 | Hyperion Catalysis International, Inc. | Method of using carbide and/or oxycarbide containing compositions |
US6099963A (en) * | 1999-03-18 | 2000-08-08 | Alliedsignal Inc. | Sizeless yarn, a method of making it and a method of using it |
US7146655B2 (en) * | 2003-06-05 | 2006-12-12 | Db Industries Llc | Bariatric toilet seat support apparatus |
CA2588124A1 (en) | 2004-11-16 | 2006-06-08 | Hyperion Catalysis International, Inc. | Method for preparing supported catalysts from metal loaded carbon nanotubes |
US7923403B2 (en) | 2004-11-16 | 2011-04-12 | Hyperion Catalysis International, Inc. | Method for preparing catalysts supported on carbon nanotubes networks |
AU2006301857A1 (en) | 2005-10-13 | 2007-04-19 | Mantra Energy Alternatives Ltd. | Continuous co-current electrochemical reduction of carbon dioxide |
CN101607203B (en) | 2009-07-16 | 2011-05-18 | 浙江大学 | Catalyst for removing dioxin-type halogenated aromatic compounds and preparation method thereof |
CN101786001A (en) | 2010-03-12 | 2010-07-28 | 厦门大学 | Catalyst for hydrogenation of carbon dioxide to generate methanol and preparation method thereof |
CN102091618A (en) | 2011-01-12 | 2011-06-15 | 厦门大学 | Copper-zirconium catalyst used in process of preparing methanol by hydrogenation of carbon dioxide and preparation method thereof |
-
2012
- 2012-04-02 US US13/437,766 patent/US20130256123A1/en not_active Abandoned
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- 2014-07-25 US US14/340,619 patent/US9109293B2/en not_active Expired - Fee Related
Patent Citations (1)
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US6936565B2 (en) * | 1999-01-12 | 2005-08-30 | Hyperion Catalysis International, Inc. | Modified carbide and oxycarbide containing catalysts and methods of making and using thereof |
Cited By (8)
Publication number | Priority date | Publication date | Assignee | Title |
---|---|---|---|---|
JP2015147990A (en) * | 2014-02-07 | 2015-08-20 | 日立化成株式会社 | Electrode, method of producing electrode, electrochemical reduction method and method of producing electrochemical reduction product |
WO2016054400A1 (en) * | 2014-10-01 | 2016-04-07 | Anne Co | Materials and methods for the electrochemical reduction of carbon dioxide |
EP3453062A4 (en) * | 2016-05-02 | 2020-01-01 | UT-Battelle, LLC | Electrochemical catalyst for conversion of co2 to ethanol |
US10844502B2 (en) | 2017-12-13 | 2020-11-24 | King Fahd University Of Petroleum And Minerals | Electrode and an electrochemical cell for producing propanol from carbon dioxide |
WO2022072434A1 (en) * | 2020-09-30 | 2022-04-07 | Ut-Battelle, Llc | Alloy based electrochemical catalyst for conversion of carbon dioxide to hydrocarbons |
US11519087B2 (en) | 2020-09-30 | 2022-12-06 | Ut-Battelle, Llc | Alloy based electrochemical catalyst for conversion of carbon dioxide to hydrocarbons |
CN113943942A (en) * | 2021-11-09 | 2022-01-18 | 深圳先进技术研究院 | Carbon dioxide energy storage system driven by new energy electric energy and energy storage method |
WO2024060687A1 (en) * | 2022-09-20 | 2024-03-28 | 中国石油化工股份有限公司 | Copper-carbon composite material, preparation method therefor and use thereof |
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US20140336037A1 (en) | 2014-11-13 |
US9109293B2 (en) | 2015-08-18 |
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