US20250027220A1 - Electrolyte Membrane - Google Patents

Electrolyte Membrane Download PDF

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Publication number
US20250027220A1
US20250027220A1 US18/707,359 US202118707359A US2025027220A1 US 20250027220 A1 US20250027220 A1 US 20250027220A1 US 202118707359 A US202118707359 A US 202118707359A US 2025027220 A1 US2025027220 A1 US 2025027220A1
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Prior art keywords
reduction
electrode
carbon dioxide
oxidation
electrolyte membrane
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US18/707,359
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English (en)
Inventor
Akihiro Kono
Yuya Uzumaki
Sayumi Sato
Takeshi Komatsu
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NTT Inc USA
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Nippon Telegraph and Telephone Corp
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Assigned to NIPPON TELEGRAPH AND TELEPHONE CORPORATION reassignment NIPPON TELEGRAPH AND TELEPHONE CORPORATION ASSIGNMENT OF ASSIGNORS INTEREST (SEE DOCUMENT FOR DETAILS). Assignors: UZUMAKI, YUYA, KONO, AKIHIRO, SATO, SAYUMI, KOMATSU, TAKESHI
Publication of US20250027220A1 publication Critical patent/US20250027220A1/en
Assigned to NTT, INC. reassignment NTT, INC. CHANGE OF NAME (SEE DOCUMENT FOR DETAILS). Assignors: NIPPON TELEGRAPH AND TELEPHONE CORPORATION
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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
    • C25B13/00—Diaphragms; Spacing elements
    • C25B13/02—Diaphragms; Spacing elements characterised by shape or form
    • 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
    • C25B1/00—Electrolytic production of inorganic compounds or non-metals
    • C25B1/01—Products
    • C25B1/02—Hydrogen or oxygen
    • C25B1/04—Hydrogen or oxygen by electrolysis of water
    • 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
    • C25B1/00—Electrolytic production of inorganic compounds or non-metals
    • C25B1/01—Products
    • C25B1/23—Carbon monoxide or syngas
    • 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
    • C25B1/00—Electrolytic production of inorganic compounds or non-metals
    • C25B1/50—Processes
    • C25B1/55—Photoelectrolysis
    • 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
    • C25B13/00—Diaphragms; Spacing elements
    • C25B13/04—Diaphragms; Spacing elements characterised by the material
    • C25B13/08—Diaphragms; Spacing elements characterised by the material based on organic materials
    • 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
    • C25B3/21—Photoelectrolysis
    • 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
    • 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
    • C25B3/26—Reduction of carbon dioxide
    • 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
    • C25B9/00—Cells or assemblies of cells; Constructional parts of cells; Assemblies of constructional parts, e.g. electrode-diaphragm assemblies; Process-related cell features
    • 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
    • C25B9/00—Cells or assemblies of cells; Constructional parts of cells; Assemblies of constructional parts, e.g. electrode-diaphragm assemblies; Process-related cell features
    • C25B9/17—Cells comprising dimensionally-stable non-movable electrodes; Assemblies of constructional parts thereof
    • C25B9/19—Cells comprising dimensionally-stable non-movable electrodes; Assemblies of constructional parts thereof with diaphragms
    • C25B9/23—Cells comprising dimensionally-stable non-movable electrodes; Assemblies of constructional parts thereof with diaphragms comprising ion-exchange membranes in or on which electrode material is embedded
    • 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
    • C25B9/00—Cells or assemblies of cells; Constructional parts of cells; Assemblies of constructional parts, e.g. electrode-diaphragm assemblies; Process-related cell features
    • C25B9/50—Cells or assemblies of cells comprising photoelectrodes; Assemblies of constructional parts thereof

Definitions

  • the present invention relates to an electrolyte membrane.
  • Non Patent Literature 1 discloses a carbon dioxide reduction device by light irradiation.
  • the oxidation electrode When the oxidation electrode is irradiated with light, electron-hole pairs are generated and separated at the oxidation electrode, and oxygen and protons (H + ) are generated by the oxidation reaction of water in the electrolytic solution.
  • the protons pass through the electrolyte membrane and reach the reduction tank, and the electrons flow to the reduction electrode through the conductive wire.
  • a reduction reaction of carbon dioxide by protons, electrons, and carbon dioxide dissolved in the solution is caused at the reduction electrode in the solution. This reduction reaction generates carbon monoxide, formic acid, methane, and the like that can be used as energy resources.
  • the reduction electrode is immersed in a solution, and carbon dioxide is dissolved in the solution to supply the carbon dioxide to the reduction electrode.
  • this method for reducing carbon dioxide since the reduction electrode is immersed in the solution, there are limitations on the concentration of carbon dioxide dissolved in the solution and the diffusion coefficient of carbon dioxide in the solution, and the amount of carbon dioxide supplied to the reduction electrode is limited.
  • Non Patent Literature 2 by using a reduction tank having structure in which carbon dioxide in a gas phase is directly supplied to the reduction electrode, the amount of carbon dioxide supplied to the reduction electrode is increased, and reduction reaction of carbon dioxide is promoted.
  • the electrolyte membrane swells with the lapse of time, and the electrolytic solution in the oxidation tank gradually exudes into the reduction tank through the electrolyte membrane. Therefore, the reaction surface (reaction site) of the reduction electrode is covered with the electrolytic solution, and the reduction reaction of carbon dioxide does not proceed. Therefore, the conventional carbon dioxide reduction device has a problem in that the reduction reaction efficiency of carbon dioxide decreases in several tens of hours.
  • the present invention has been made to address the problem above, and an object of the present invention is to provide a technology capable of improving the reduction reaction efficiency of carbon dioxide.
  • An electrolyte membrane according to an aspect of the present invention is an electrolyte membrane that is disposed between an electrolytic solution in an oxidation tank and a reduction electrode in a reduction tank in contact with the electrolytic solution and reduction electrode, and is used in a carbon dioxide reduction device that performs a reduction reaction of carbon dioxide by bringing carbon dioxide into direct contact with the reduction electrode, in which fibers are woven in a network shape.
  • the reduction reaction efficiency of carbon dioxide can be improved.
  • FIG. 1 is a diagram showing a configuration example of a carbon dioxide reduction device according to a first embodiment.
  • FIG. 2 is a diagram showing a formation example of fibers.
  • FIG. 3 is a diagram showing an example of fibers.
  • FIG. 4 is a diagram showing a measurement result of the Faraday efficiency of formic acid according to the first embodiment.
  • FIG. 5 is a diagram showing a configuration example of a carbon dioxide reduction device according to a second embodiment.
  • FIG. 6 is a diagram showing a measurement result of the Faraday efficiency of formic acid according to the second embodiment.
  • FIG. 1 is a diagram showing a configuration example of a carbon dioxide reduction device 100 according to a first embodiment.
  • the carbon dioxide reduction device 100 includes an oxidation electrode 1 , an oxidation tank 2 , an electrolytic solution 3 , a reduction electrode 4 , a reduction tank 5 , an electrolyte membrane 6 , a conductive wire 7 , a light source 8 , and fibers 9 .
  • the oxidation electrode 1 is immersed in the electrolytic solution 3 in the oxidation tank 2 .
  • the oxidation electrode 1 is formed by forming a semiconductor on a substrate having a predetermined area.
  • the oxidation electrode 1 is formed, for example, by forming a film of a compound exhibiting photoactivity, redox activity, or the like such as a nitride semiconductor, titanium oxide, amorphous silicon, a ruthenium complex, or a rhenium complex, on a surface of the sapphire substrate.
  • the oxidation tank 2 holds the electrolytic solution 3 in which the oxidation electrode 1 is immersed.
  • the electrolytic solution 3 is placed in the oxidation tank 2 .
  • the electrolytic solution 3 include a potassium hydrogen carbonate aqueous solution, a sodium hydrogen carbonate aqueous solution, a potassium chloride aqueous solution, a sodium chloride aqueous solution, a potassium hydroxide aqueous solution, a rubidium hydroxide aqueous solution, and a cesium hydroxide aqueous solution.
  • the reduction electrode 4 is disposed in the reduction tank 5 .
  • the reduction electrode 4 is formed on a substrate having predetermined area similarly to the oxidation electrode 1 .
  • the reduction electrode 4 is, for example, a porous body of copper, platinum, gold, silver, indium, palladium, gallium, nickel, tin, cadmium, or an alloy thereof.
  • the reduction electrode 4 may be a compound such as silver oxide, copper oxide, copper (II) oxide, nickel oxide, indium oxide, tin oxide, tungsten oxide, tungsten (VI) oxide, or copper oxide, or a porous metal complex having a metal ion and an anionic ligand.
  • the reduction tank 5 has the reduction electrode 4 disposed inside thereof, and holds gas phase carbon dioxide supplied from the outside through a pipe.
  • the electrolyte membrane 6 is disposed between the oxidation tank 2 and the reduction tank 5 . To be precise, the electrolyte membrane 6 is disposed between the electrolytic solution 3 and the reduction electrode 4 in contact with the electrolytic solution 3 and the reduction electrode 4 .
  • the electrolyte membrane 6 is, for example, Nafion (registered trademark), FORBLUE, or Aquivion each of which is an electrolyte membrane having a carbon-fluorine skeleton, or SELEMION or NEOSEPTA that is an electrolyte membrane having a carbon-hydrogen skeleton.
  • the conductive wire 7 physically and electrically connects the oxidation electrode 1 and the reduction electrode 4 .
  • the light source 8 is disposed close to the oxidation tank 2 .
  • the light source 8 is, for example, a light source of sunlight, a xenon lamp, a pseudo sunlight source, a halogen lamp, a mercury lamp, or a combination thereof.
  • the reduction electrode 4 and the electrolyte membrane 6 may be formed of an integrated material.
  • the reduction electrode 4 and the electrolyte membrane 6 can be realized by using a gas diffusion electrode (GDE (registered trademark)) including porous equipment and a catalyst. Since the gas diffusion electrode can separate liquid and gas, and allows cations to move in the electrode, the gas diffusion electrode has an action equivalent to the action of both the reduction electrode 4 and the electrolyte membrane 6 .
  • GDE registered trademark
  • the reduction electrode 4 and the electrolyte membrane 6 are drawn so as to have a large width in the lateral direction of the paper surface, but the width in the lateral direction of the paper surface may be reduced to have a thin plate shape with a flat surface in the depth direction of the paper surface.
  • the oxidation reaction of water in the electrolytic solution 3 is performed by irradiation light (light energy) from the light source 8 using the electrolytic solution 3 and the oxidation electrode 1 of the semiconductor immersed in the electrolytic solution 3 .
  • the reduction reaction of carbon dioxide is performed using the reduction electrode 4 connected to the oxidation electrode 1 via the conductive wire 7 and carbon dioxide brought into direct contact with the reduction electrode 4 .
  • the light source 8 emits light from the bottom of the oxidation tank 2 , electron-hole pairs are generated and separated at the oxidation electrode 1 within the oxidation tank 2 that has received the emitted light, and oxygen and protons are generated by the oxidation reaction of water in the electrolytic solution 3 .
  • the protons pass through the electrolyte membrane 6 and reach the reduction electrode 4 in the reduction tank 5 from the electrolytic solution 3 in the oxidation tank 2 .
  • the electrons flow from the oxidation electrode 1 in the oxidation tank 2 to the reduction electrode 4 in the reduction tank 5 via the conductive wire 7 .
  • a reduction reaction of carbon dioxide by protons, electrons, and carbon dioxide in a gas phase brought into direct contact with the reduction electrode 4 is caused in the reduction electrode 4 .
  • This oxidation-reduction reaction generates carbon monoxide, formic acid, methane, and the like that can be used as energy resources.
  • a strong alkaline aqueous solution for example, a 1.0 mol/L aqueous solution of sodium hydroxide is used as the electrolytic solution 3 in the oxidation tank 2 .
  • the electrolyte membrane 6 swells, and the electrolytic solution 3 passes through the pores of the electrolyte membrane 6 and exudes to the surface of the reduction electrode 4 in the reduction tank 5 .
  • fibers 51 may be incorporated into the electrolyte membrane 6 so as to prevent swelling of the electrolyte membrane 6 .
  • the fibers 9 are woven in a network shape inside the electrolyte membrane 6 .
  • the fibers 9 are woven into the electrolyte membrane 6 so as to form a regular triangular, square, and regular hexagonal network shape when viewed from the side of the paper surface of FIG. 1 .
  • the lengths of the sides of a regular triangle, a square, and a regular hexagon are ⁇ cm, and the area to be filled is A cm 2
  • the length of the side of the regular triangle is ⁇ (4A/ ⁇ ( 3 )) ⁇ 3
  • the length of the side of the square is ⁇ (A) ⁇ 4
  • the length of the side of the regular hexagon is ⁇ (2A/3 ⁇ (3)) ⁇ 6. Therefore, it can be seen that the necessary lengths of the sides of the regular triangle, the square, and the regular hexagon are shortened in this order. Therefore, it is desirable that the fibers 9 are woven into the electrolyte membrane 6 so as to have structure of regular hexagonal network (regular hexagonal network structure, honeycomb structure).
  • the polymer material of the fibers 9 is preferably, for example, polytetrafluoroethylene (PTFE), polyvinylidene chloride (PVdC), acrylonitrile-butadiene-styrene (ABS), polyethylene (PE), or polypropylene (PP) which does not swell even in an acid or an alkaline solution.
  • PTFE polytetrafluoroethylene
  • PVdC polyvinylidene chloride
  • ABS acrylonitrile-butadiene-styrene
  • PE polyethylene
  • PP polypropylene
  • the fibers 9 are woven into the inside of the electrolyte membrane 6 in a network shape, it is possible to suppress the electrolytic solution 3 in the oxidation tank 2 from entering the inside of the electrolyte membrane 6 , it is possible to suppress liquid leakage of the electrolytic solution 3 to the reduction electrode 4 , and the reaction site of the reduction electrode 4 is not filled with the electrolytic solution 3 . In addition, it is possible to maintain a state in which protons can pass through the electrolyte membrane 6 . As a result, the reduction reaction of carbon dioxide can proceed, and a decrease in the reduction reaction efficiency can be suppressed.
  • GaN gallium nitride
  • AlGaN aluminum gallium nitride
  • NiO nickel oxide
  • the cocatalyst thin film was used as the oxidation electrode 1 , and the oxidation electrode 1 was immersed in the electrolytic solution 3 of a 1.0 mol/L aqueous potassium hydroxide solution in the oxidation tank 2 .
  • the reduction electrode 4 was formed using a porous body of copper, the formed reduction electrode 4 was connected to the oxidation electrode 1 by the conductive wire 7 , and the reduction electrode 4 was installed in the reduction tank 5 .
  • Nafion was used for the electrolyte membrane 6 physically separating the oxidation tank 2 and the reduction tank 5 .
  • the fibers 9 of PTFE having a fiber length and a fiber diameter shown in FIG. 3 were used.
  • Nafion having PTFE fibers having regular hexagonal network structure was used.
  • Nafion having PTFE fibers having square network structure was used.
  • Nafion having PTFE fibers having regular triangular network structure was used.
  • Nafion into which no PTFE fibers were introduced was used as it was as the electrolyte membrane 6 .
  • the light source 8 a 300 W xenon lamp was used. A wavelength of 450 nm or more was cut with a filter, and the illuminance was set to 6.6 mW/cm 2 . A light irradiation surface of the oxidation electrode 1 was set to 2.5 cm 2 .
  • the current flowing between the oxidation electrode 1 and the reduction electrode 4 by the irradiation light was measured by an electrochemical measurement apparatus (Model 1287 Potentiogalvanostat manufactured by Solartron). Gases and liquids generated in the oxidation tank 2 and the reduction tank 5 were collected, and the reaction products were analyzed using a gas chromatograph, a liquid chromatograph, and a gas chromatograph mass spectrometer.
  • the effect of the fibers 9 woven into the electrolyte membrane 6 was examined by determining the Faraday efficiency of the carbon dioxide reduction reaction.
  • a method for calculating the Faraday efficiency of the carbon dioxide reduction reaction will be described later.
  • FIG. 4 is a diagram showing a measurement result of the Faraday efficiency of formic acid according to the first embodiment.
  • Comparative Example in which the fibers 9 were not woven, the Faraday efficiency decreased after 6 hours.
  • Examples 1 to 3 in which the fibers 9 were woven the Faraday efficiency did not decrease even after 6 hours. This is because as a result of introducing PTFE fibers into the Nafion film, swelling of the Nafion film was suppressed, liquid leakage of the electrolytic solution 3 to the reduction electrode 4 was suppressed, and the reaction site of the reduction electrode 4 was not filled with the electrolytic solution 3 .
  • the Faraday efficiency is in descending order of the Faraday efficiency as Comparative Example, Example 1, Example 2, and Example 3. This is because the PTFE fibers inhibit the movement of protons, and it can be understood that the order of the introduction amount of the PTFE fibers and the order of the Faraday efficiency coincide with each other as described above.
  • the Faraday efficiency of carbon dioxide indicates the ratio of the number of electrons used in the carbon dioxide reduction reaction to the number of electrons moved between the oxidation electrode 1 and the reduction electrode 4 by light irradiation or application of a current voltage, and can be calculated by Formula (1).
  • Faraday ⁇ efficiency ⁇ number ⁇ of ⁇ electrons ⁇ in ⁇ reduction ⁇ reaction ⁇ / ( 1 ) ⁇ number ⁇ of ⁇ electrons ⁇ transferred ⁇ between ⁇ electrodes ⁇
  • the “number of electrons in reduction reaction” in Formula (1) is determined by converting the measured value of the integrated amount of the generated carbon dioxide reduction product into the number of electrons required for the production reaction.
  • the “number of electrons in the reduction reaction” when the reduction product is a gas can be calculated by Formula (2).
  • A is a concentration (ppm) of the reduction reaction product.
  • B is a flow rate (L/sec) of the carrier gas.
  • Z is the number of electrons required for the reduction reaction.
  • F is the Faraday constant (C/mol).
  • T is a light irradiation time or a current voltage application time (sec).
  • V g is a molar volume of the gas (L/mol).
  • the “number of electrons in the reduction reaction” when the reduction product is a liquid can be calculated by Formula (3).
  • C is a concentration (mol/L) of the reduction reaction product.
  • V l is a volume (L) of the liquid sample.
  • Z is the number of electrons required for the reduction reaction.
  • F is the Faraday constant (C/mol).
  • the first embodiment has been described above. According to the carbon dioxide reduction device 100 of the first embodiment, it is possible to provide the carbon dioxide reduction device 100 capable of allowing the carbon dioxide reduction reaction to proceed without reducing the Faraday efficiency.
  • the fibers 9 are woven in a network shape inside the electrolyte membrane 6 .
  • the case where the light source 8 and the oxidation electrode 1 including a semiconductor are used has been described.
  • an oxidation/reduction reaction is allowed to proceed using an external power supply and the oxidation electrode 1 including a metal.
  • FIG. 5 is a diagram showing a configuration example of a carbon dioxide reduction device 100 according to the second embodiment.
  • the oxidation electrode 1 is platinum.
  • the oxidation electrode 1 may be, for example, gold or silver.
  • the external power supply 10 is an electrochemical measurement device, and is connected in series to the conductive wire 7 connecting the oxidation electrode 1 and the reduction electrode 4 .
  • the power supply 10 may be another power supply device.
  • Other components are the same as those of the first embodiment.
  • the oxidation reaction of water in the electrolytic solution 3 is performed by the current voltage (electrical energy) from the power supply 10 using the electrolytic solution 3 and the oxidation electrode 1 of platinum (metal) immersed in the electrolytic solution 3 .
  • the reduction reaction of carbon dioxide is performed using the reduction electrode 4 connected to the power supply 10 (source of electric energy) and carbon dioxide brought into direct contact with the reduction electrode 4 .
  • the power supply 10 applies a current voltage to the conductive wire 7 , electron-hole pairs are generated and separated at the oxidation electrode 1 in the oxidation tank 2 , and oxygen and protons are generated by the oxidation reaction of water in the electrolytic solution 3 .
  • the protons pass through the electrolyte membrane 6 and reach the reduction electrode 4 in the reduction tank 5 from the electrolytic solution 3 in the oxidation tank 2 .
  • the electrons flow from the power supply 10 to the reduction electrode 4 in the reduction tank 5 via the conductive wire 7 .
  • a reduction reaction of carbon dioxide by protons, electrons, and carbon dioxide in a gas phase brought into direct contact with the reduction electrode 4 is caused in the reduction electrode 4 .
  • the fibers 9 are woven into the electrolyte membrane 6 in a network shape.
  • the fibers 9 are woven into the electrolyte membrane 6 so as to have a regular triangular shape, a square shape, or a regular hexagonal shape.
  • FIG. 6 is a diagram showing a measurement result of the Faraday efficiency of formic acid according to the second embodiment. Examples using the same electrolyte membrane 6 as in Example 1 to Example 3 described in the first embodiment are referred to as Example 4 to Example 6, respectively. Comparative Example in which Nafion in which the fibers 9 are not woven is used as it is as the electrolyte membrane 6 is also described.
  • the second embodiment has been described above. According to the carbon dioxide reduction device 100 of the second embodiment, it is possible to provide the carbon dioxide reduction device 100 capable of allowing the carbon dioxide reduction reaction to proceed without reducing the Faraday efficiency.
  • the fibers 9 are woven in a network shape inside the electrolyte membrane 6 .
  • the present invention can be widely used in the field related to the recycling of carbon dioxide. Although light energy is used in the first embodiment and electric energy is used in the second embodiment, other renewable energy may be used. In addition, the first embodiment and the second embodiment can be combined.
  • the present invention can be also applied to any electrolyte membrane as long as it is the electrolyte membrane 6 used in the carbon dioxide reduction device 100 that is disposed between the electrolytic solution 3 in the oxidation tank 2 and the reduction electrode 4 in the reduction tank 5 in contact with the electrolytic solution 3 and the reduction electrode 4 and that performs the reduction reaction of carbon dioxide by bringing carbon dioxide into contact with the reduction electrode 4 .

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  • Chemical & Material Sciences (AREA)
  • Organic Chemistry (AREA)
  • Engineering & Computer Science (AREA)
  • Chemical Kinetics & Catalysis (AREA)
  • Electrochemistry (AREA)
  • Materials Engineering (AREA)
  • Metallurgy (AREA)
  • Inorganic Chemistry (AREA)
  • Electrolytic Production Of Non-Metals, Compounds, Apparatuses Therefor (AREA)
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JP2011146291A (ja) * 2010-01-15 2011-07-28 Toyota Motor Corp 高分子電解質膜の製造方法
JP2018090838A (ja) * 2016-11-30 2018-06-14 昭和シェル石油株式会社 二酸化炭素還元装置
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JP6940756B2 (ja) * 2017-06-29 2021-09-29 富士通株式会社 二酸化炭素還元用電極、及びその製造方法、並びに二酸化炭素還元装置
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US20210395907A1 (en) * 2018-12-10 2021-12-23 Nippon Telegraph And Telephone Corporation Carbon Dioxide Gas-Phase Reduction Device and Carbon Dioxide Gas-Phase Reduction Method
JP7287234B2 (ja) * 2019-10-08 2023-06-06 株式会社豊田中央研究所 Ｃｏ２還元反応装置
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