WO2009157454A1

WO2009157454A1 - Electrochemical reactor and fuel gas manufacturing method using the same

Info

Publication number: WO2009157454A1
Application number: PCT/JP2009/061426
Authority: WO
Inventors: 好洋平田
Original assignee: 国立大学法人鹿児島大学
Priority date: 2008-06-27
Filing date: 2009-06-23
Publication date: 2009-12-30
Also published as: JPWO2009157454A1; JP5376381B2

Abstract

An electrolyte film (3) is sandwiched between an anode electrode (1) and a cathode electrode (2). The anode electrode (1) is made from, for example, a mixture of SrRuO₃ and GDC. The cathode electrode (2) is made from, for example, a mixture of Ni and GDC. Moreover, the electrolyte film (3) is made from, for example, a porous material of GDC. Moreover, the electrolyte film (3) has a thickness in the order of 50 μm, for example. Thus, an electrochemical reactor is configured. The electrochemical reactor is inserted into a tube (4), for example, for use.

Description

Electrochemical reactor and fuel gas production method using the same

The present invention relates to an electrochemical reactor suitable for synthesizing fuel gas using an oxidation-reduction reaction and a method for producing fuel gas using the same.

Biogas generated by methane fermentation in livestock excreta and sewage treatment plants contains 60% methane (CH ₄ ) and 40% carbon dioxide (CO ₂ ). Hydrogen and carbon monoxide produced by these reactions can be used as various fuels. In addition, the fuel closed system can be established by mixing carbon dioxide with biogas again.

Conventionally, as a method of synthesizing an H ₂ —CO based fuel gas from a CH ₄ —CO ₂ based gas using an oxidation-reduction reaction at an electrode, there is CO ₂ dry reforming of methane using a Ni catalyst. This dry reforming is expressed by equation (1).
CH ₄ + CO ₂ → 2H ₂ + 2CO (1)

However, in dry reforming, as shown in the equation (2), carbon monoxide (CO) causes a disproportionation reaction in CO ₂ and C at a temperature of less than 600 ° C. For this reason, it is necessary to perform the treatment at a high temperature of 600 ° C. or higher.
2CO → CO ₂ + C (2)

On the other hand, at a high temperature, as shown in the equation (3), thermal decomposition of CH ₄ proceeds, and the precipitated carbon covers the Ni catalyst. For this reason, catalytic ability falls with progress of time. Further, the deposited carbon causes the reaction gas to be blocked.
CH ₄ → 2H ₂ + C (3)

As described above, in the conventional dry reforming, the fuel gas cannot be synthesized with high efficiency no matter what the temperature is.

An object of the present invention is to provide an electrochemical reactor capable of synthesizing fuel gas with high efficiency and a method for producing fuel gas using the same.

The inventor of the present application has come up with the following aspects of the invention as a result of intensive studies to solve the above problems.

An electrochemical reactor according to the present invention includes a ruthenium-containing anode, a ruthenium- or nickel-containing cathode, and a metal oxide that is provided between the anode electrode and the cathode electrode and exhibits oxide ion conductivity. And a porous electrolyte membrane containing.

The fuel gas production method according to the present invention includes an anode electrode containing ruthenium, a cathode electrode containing ruthenium or nickel, and an oxide ion conductivity provided between the anode electrode and the cathode electrode. A porous electrolyte membrane containing a metal oxide, and a method for producing a fuel gas using an electrochemical reactor, the step of applying a voltage between the anode electrode and the cathode electrode, And a step of supplying a gas containing methane and carbon dioxide toward the cathode electrode.

According to the present invention, an oxidation-reduction reaction can be caused at the anode electrode and the cathode electrode. Therefore, even when hydrogen gas and carbon monoxide gas are produced from a gas containing methane and carbon dioxide at a high temperature, carbon deposition can be suppressed and fuel gas can be obtained with high efficiency.

FIG. 1 is a flowchart showing a configuration of an electrochemical reactor according to an embodiment of the present invention. FIG. 2 is a diagram showing a method for producing a GDC electrolyte powder. FIG. 3 is a diagram showing a method for producing SrRuO ₃ powder. FIG. 4 is a diagram illustrating a method for producing an electrochemical reactor. FIG. 5 is a graph showing the results of the first experiment. FIG. 6A shows the contents of the second experiment. FIG. 6B is a diagram illustrating a result of the second experiment. FIG. 7 is a graph showing the results of the third experiment. FIG. 8 is a graph showing the results of the fourth experiment. FIG. 9 is a graph showing the results of the fifth experiment. FIG. 10 is a graph showing the results of the sixth experiment. FIG. 11 is a graph showing the results of the seventh experiment. FIG. 12 is a graph showing the results of the eighth experiment. FIG. 13 is also a graph showing the results of the eighth experiment.

Hereinafter, embodiments of the present invention will be specifically described with reference to the accompanying drawings. FIG. 1 is a flowchart showing a configuration of an electrochemical reactor according to an embodiment of the present invention.

In the electrochemical reactor according to this embodiment, an electrolyte membrane 3 is sandwiched between an anode electrode 1 and a cathode electrode 2 as shown in FIG. The anode electrode 1 is composed of, for example, a mixture of SrRuO ₃ and Ce _0.8 Gd _0.2 O _1.9 (hereinafter also referred to as GDC), and the cathode electrode 2 is composed of, for example, a mixture of Ni and GDC. ing. The electrolyte membrane 3 is composed of, for example, a GDC porous body. The thickness of the electrolyte membrane 3 is about 10 μm to 100 μm, for example, 50 μm. In this way, an electrochemical reactor is configured. Such an electrochemical reactor is used, for example, in a tube 4.

Here, the operation of the electrochemical reactor according to the present embodiment will be described. In this electrochemical reactor, a voltage of about 1 V to 5 V is applied between the anode electrode 1 and the cathode electrode 2. When CH ₄ and CO ₂ -based source gases are supplied toward the cathode electrode 2, a reduction reaction occurs at the cathode electrode 2 as shown in the formula (4).
CO ₂ + 2e ⁻ → CO + O ²⁻ (4)

Oxide ions (O ²⁻ ) generated by this reduction reaction pass through the electrolyte membrane 3 and reach the anode electrode 1. CH ₄ gas also reaches the anode electrode 1. When the oxide ions and CH ₄ gas reach the anode electrode 1, an oxidation reaction occurs in the anode electrode 1 as shown in the equation (5).
CH ₄ + O ²⁻ → CO + 2H ₂ + 2e ⁻ (5)

Therefore, the reaction formula of the total reaction in this electrochemical reactor is expressed by equation (6).
CH ₄ + CO ₂ → 2H ₂ + 2CO (6)

That is, according to the present embodiment, the H ₂ —CO based fuel gas can be synthesized from the CH ₄ —CO ₂ based gas. Further, as shown in the formula (5), since the reaction between the transported oxide ion (O ²⁻ ) and methane proceeds, the thermal decomposition of CH ₄ like conventional dry reforming is suppressed. Can do. Therefore, the H ₂ —CO based fuel gas can be produced with high efficiency.

Next, a method for manufacturing the electrochemical reactor as described above will be described.

First, a method for producing a GDC electrolyte powder used for the anode electrode 1 and the cathode electrode 2 will be described. FIG. 2 is a diagram showing a method for producing a GDC electrolyte powder. In the case of the GDC electrolyte powder, first, a 0.2 M Ce (NO ₃ ) ₃ aqueous solution and a 0.2 M Gd (NO ₃ ) ₃ aqueous solution are mixed at a molar ratio of Ce and Gd of 4 to 1 ( Ce: Gd = 4: 1). Next, this mixed solution is added to a 0.4 M oxalic acid aqueous solution and coprecipitated. Thereafter, filtration and drying are performed. For example, the drying temperature is 100 ° C., and the time is 24 hours. Subsequently, calcination at 600 ° C. is performed for 2 hours. Next, pulverization is performed by a ball mill using alumina spheres having a diameter of 3 mm to obtain GDC powder.

Next, a method for producing SrRuO ₃ powder used for the anode electrode 1 will be described. FIG. 3 is a diagram showing a method for producing SrRuO ₃ powder. First, a 0.2 M aqueous solution of Sr (NO ₃ ) ₂ and a 0.2 M aqueous solution of RuCl ₃ are mixed at a molar ratio of Sr ²⁺ and Ru ³⁺ of 1: 1 (Sr ²⁺ : Ru ³⁺ = 1: 1). Next, this mixed solution is added to a 1.0 M aqueous ammonia solution and coprecipitated. Thereafter, freeze drying is performed. Subsequently, calcination at 1000 ° C. is performed for 2 hours to obtain SrRuO ₃ powder.

Next, a method for producing an electrochemical reactor will be described. FIG. 4 is a diagram illustrating a method for producing an electrochemical reactor. First, the anode electrode 1 and the cathode electrode 2 are produced individually.

In the production of the anode electrode 1, SrRuO ₃ powder and GDC electrolyte powder are mixed at a volume ratio of 30 to 70, and a suspension of this mixture (suspension) is produced. The amount of solid in this suspension is about 10% by volume. Next, freeze-drying is performed, followed by baking at 600 ° C. for 1 hour. As a result, the anode electrode 1 is produced.

In the production of the cathode electrode 2, Ni (NO ₃ ) ₂ and GDC electrolyte powder are mixed in a volume ratio of Ni: GDC = 30: 70 in terms of Ni amount, and a suspension (suspension) of this mixture is produced. To do. The amount of solid in this suspension is about 10% by volume. Next, freeze-drying is performed, followed by baking at 600 ° C. for 1 hour. As a result, the cathode electrode 2 is produced.

Then, a GDC film is sandwiched as the electrolyte membrane 3 between the anode electrode 1 and the cathode electrode 2, and uniaxial press molding of 200 MPa is performed for 1 minute. In addition, as a GDC film, what was formed into a film by the doctor blade method of the nonaqueous suspension containing 30 volume% of GDC can be used. A GDC film having a thickness of about 50 μm can be produced by a doctor blade having a front blade height of 150 μm and a rear blade height of 80 μm.

After sandwiching the electrolyte membrane 3, sintering at 1200 ° C. is performed for 2 hours. Subsequently, NiO in the cathode electrode 2 is reduced to Ni by performing reduction treatment at 800 ° C. for 24 hours under a hydrogen atmosphere of 50 ml / min. An electrochemical reactor can be manufactured by these series of processes.

The material of the anode electrode is not limited to the above as long as Ru is included. For example, you may be comprised from the mixture of metal Ru or Ru oxide, and GDC. Further, two or more of metal Ru, Ru oxide and SrRuO ₃ may be included.

The material of the electrolyte membrane is not limited to the above as long as it contains a metal oxide exhibiting oxide ion conductivity. Examples of such metal oxides include cerium-rare earth elements (ytterbium, yttrium, gadolinium, samarium, neodymium, lanthanum, etc.) oxides, zirconium-yttrium oxides, and lanthanum-gallium oxides. .

Next, the experiment conducted by the inventors will be described.

(First experiment)
In the first experiment, a mixed gas of CH ₄ (25 cm ³ / min) and CO ₂ (25 cm ³ / min) was circulated from the cathode side in FIG. 1, and the change over time in the flow rate of the gas flowing out from the anode side was measured. . An electric field of 1.25 V / cm was applied and the reaction temperature was 400 ° C.-700 ° C. The result is shown in FIG.

An experiment for comparison was also conducted. In an experiment for comparison, Ni (NO ₃ ) ₂ and Al ₂ O ₃ powders were mixed at a ratio of 30 vol% Ni-70 vol% Al ₂ O ₃ and formed into a diameter of 16 mm and a height of 10 mm. The compact was fired at 800 ° C. for 1 hour. Further, NiO was reduced to Ni by heating at 700 ° C. for 10 hours in 70 vol% H ₂ -30 vol% Ar gas. In some experiments, only Al ₂ O ₃ compacts containing no Ni were produced. 50 vol% CH ₄ -50 vol% CO ₂ mixed gas was allowed to flow through this, and dry reforming was performed. The result is shown in FIG.

As shown in FIG. 5A, when the mixed gas was allowed to flow only through the Al ₂ O ₃ sintered body, the flow rate did not change. This is because the decomposition reaction of CH ₄ and CO ₂ does not proceed, so that no carbon deposition occurs and no blockage occurs. On the other hand, when the Ni / Al ₂ O ₃ catalyst was used (500 ° C.-700 ° C.), the flow rate of the outlet gas decreased after 30 minutes regardless of the temperature. This is because the decomposition reaction of CH ₄ and CO ₂ progressed by the Ni catalyst, and gas clogging occurred in the catalyst due to carbon deposition.

On the other hand, in the Ni / GDC-GDC-SrRuO ₃ / GDC reactor to which an electric field of 1.25 V / cm was applied, the flow rate did not decrease during the measured time (1.5 hours-6 hours), and the gas was blocked. Did not happen. This is because the electrochemical reaction due to the application of the electric field has progressed and carbon deposition has been suppressed.

(Second experiment)
In the second experiment, as shown in FIG. 6A, the length of the cathode electrode 2 is 4 mm, and four positions (positions A to A, 0.5 mm, 1.5 mm, 2.5 mm, and 3.5 mm away from the end). In D), EPMA analysis (Electron Probe Micro-Analysis) of carbon after synthesis of the fuel gas was performed. The result is shown in FIG. 6B.

In EPMA analysis, a decomposition reaction of 50 vol% CH ₄ -50 vol% CO ₂ was carried out at 400 ° C. to 700 ° C. under an electric field of 1.25 V / cm, and the cathode surface after 11 hours in total was analyzed.

As shown in FIG. 6B, the carbon content at any of the four points (positions A to D) was 13% to 18% with respect to the 100% carbon powder measured as a reference. This result indicates that although carbon deposition occurs uniformly inside the cathode, the amount is not so high as to cause gas blockage.

(Third experiment)
In the third experiment, using a Ni / GDC-GDC-SrRuO ₃ / GDC reactor to which an electric field of 1.25 V / cm was applied, a decomposition reaction of 50 vol% CH ₄ -50 vol% CO ₂ was performed at 400 ° C. to 700 ° C. The ratio of outlet gas was examined. The result is shown in FIG.

As shown in FIG. 7, as the temperature increased, decomposition of the introduced CH ₄ and CO ₂ proceeded, and as a result, the amounts of H ₂ and CO increased. The gas ratio at each temperature was almost constant regardless of time. CH ₄ and CO ₂ remaining at 700 ° C. were each about 10%. Further decomposition requires temperatures above 700 ° C.

(Fourth experiment)
In the fourth experiment, the Ni / GDC-GDC-SrRuO ₃ / GDC reactor was operated at 800 ° C. and the applied electric field was 1.25 V / cm or 6.25 V / cm. And the ratio of the exit gas was measured by setting the ratio of the mixed gas of CH ₄ and CO ₂ to be introduced to 30/70, 40/60, 50/50, 60/40, or 70/30. The result is shown in FIG.

As shown in FIG. 8, when the applied electric field was 1.25 V / cm, the remaining amounts of CH ₄ and CO ₂ were almost zero. H ₂ and CO were produced by mixing at any ratio. As the amount of methane at the inlet increases, more hydrogen is produced. A similar tendency was observed when the applied electric field was 6.25 V / cm. However, when the proportion of CH ₄ was small, it was confirmed that CO ₂ remained. It is conceivable that the reaction mechanism varies depending on the magnitude of the electric field. This will be described in detail later.

(Fifth experiment)
In the fifth experiment, using a Ni / GDC-GDC-SrRuO ₃ / GDC reactor to which an electric field of 1.25 V / cm was applied and the Ni / Al ₂ O ₃ catalyst prepared in the first experiment, 50 vol. % CH ₄ -50 vol% CO ₂ was decomposed at 400 ° C. to 700 ° C., and the molar ratio of H ₂ and CO produced was measured. The result is shown in FIG.

When the reaction (CH ₄ + CO ₂ → 2CO + 2H ₂ ) proceeds ideally, the H ₂ / CO ratio becomes 1. In the case of the Ni / Al ₂ O ₃ catalyst, the above-described formula (3) also occurs, and the H ₂ / CO ratio is 2 or more. On the other hand, in an electrochemical reactor to which an electric field of 1.25 V / cm was applied, the ideal ratio was close to 1 at any temperature. This is in good agreement with the fact that no gas blockage occurs.

(Sixth experiment)
In the sixth experiment, the decomposition reaction of 50 vol% CH ₄ -50 vol% CO ₂ was performed at 400 ° C. to 700 ° C. using an electrochemical reactor to which an electric field of 1.25 V / cm was applied. _Two partial pressures were measured. The result is shown in FIG.

As shown in FIG. 10, the oxygen partial pressure was 10 ⁻²⁹ Pa to 10 ⁻¹² Pa in the measured temperature range. This indicates that direct oxidation of methane (CH ₄ + 1 / 2O ₂ → CO + H ₂ ) did not occur.

(Seventh experiment)
In the seventh experiment, the CH ₄ / CO ₂ ratio (A) of the inlet gas and the H ₂ / CO ratio of the outlet gas (A) by an electrochemical reactor applied with an electric field of 1.25 V / cm or 6.25 V / cm ( B) was measured. The reaction temperature was 800 ° C. The result is shown in FIG.

Here, B ₁ , B ₂ , and B ₃ in FIG. 11 will be described.

When the reaction shown in the formula (7) and the reaction shown in the formula (7) proceed simultaneously electrochemically, the ratio B ₁ of H ₂ and CO produced is (3A-1) / (A + 1). .
CH ₄ + CO ₂ → 2H ₂ + 2CO (6)
CH ₄ + 3CO ₂ → 4CO + 2H ₂ 0 (7)

The cathode reaction and the anode reaction in the formula (7) are expressed by the formula (8) and the formula (9), respectively.
3CO ₂ + 6e ⁻ → 3CO + 3O ^2- (8)
CH ₄ + 3O ²⁻ → CO + 2H ₂ O + 6e ⁻ (9)

On the other hand, when the reaction shown in the formula (6) and the reaction shown in the formula (3) proceed simultaneously, the ratio B ₂ of H ₂ and CO to be generated becomes A.
CH ₄ + CO ₂ → 2H ₂ + 2CO (6)
CH ₄ → 2H ₂ + C (3)

Further, when the reaction shown in the formula (10) proceeds simultaneously with the reaction shown in the formula (6) electrochemically, the ratio B ₃ of H ₂ and CO to be generated becomes 2 / (3-A). The reaction shown in formula (10) shows the formation of H ₂ and acetaldehyde.
CH ₄ + CO ₂ → 2H ₂ + 2CO (6)
3CH ₄ + CO ₂ → 2H ₂ + 2CH ₃ CHO (10)

CH ₃ CHO is considered to be produced electrochemically by a chemical reaction between CO and CH ₄ produced by the reaction shown in the formula (6) (formula (11)).
CH ₄ + CO → CH ₃ CHO (11)

And the overall reaction of the reaction shown in the formula (11) and the reaction shown in the formula (6) is the reaction shown in the formula (10).

The calculated values of these ratios B ₁ , B ₂ , and B ₃ are shown in FIG. When the applied electric field was 6.25 V / cm, the H ₂ / CO ratio coincided with the calculated value of B ₃ . On the other hand, in the electric field of 1.25 V / cm, when A is smaller than 1, the H ₂ / CO ratio is close to B ₂ . When A was larger than 1, the H ₂ / CO ratio agreed with the calculated value of B ₁ . Therefore, it is inferred that the value of A changed the reaction mechanism.

(Eighth experiment)
In the eighth experiment, GDC (Ce _0.8 Gd _0.2 O _1.9 ) electrolyte powder was produced by the oxalate coprecipitation method. Further, 1.9 ml of isopropanol and 0.97 ml of toluene as a solvent, 0.63 g of polyethylene glycol as a plasticizer, and 0.35 g of polyvinyl butyral as a binder were mixed to prepare a mixed solution. Next, 7 g of GDC electrolyte powder was dispersed in this mixed solution, and stirred for 24 hours. Thereafter, a GDC electrolyte membrane having a thickness of 50 μm (± 3 μm) was produced by a doctor blade method.

Also, three types of mixed powders (mixed powder of NiO and GDC, mixed powder of RuO ₂ and GDC, mixed powder of SrRuO ₃ and GDC) were prepared for electrodes. In preparation of NiO and GDC mixed powder, GDC electrolyte powder and 1.4M Ni (NO ₃ ) ₂ aqueous solution are mixed so that Ni: GDC = 30: 70 (volume ratio) and stirred for 6 hours. went. Then, it lyophilized | freeze-dried and calcined at 600 degreeC in the air for 1 hour. In the preparation of the mixed powder of RuO ₂ and GDC, the GDC electrolyte powder and the RuCl ₃ · 2.7H ₂ O powder are mixed so that Ru: GDC = 30: 70 (volume ratio), and this is mixed with distilled water. And stirred for 6 hours. Then, it lyophilized | freeze-dried and calcined at 800 degreeC in the air for 1 hour. In the preparation of the mixed powder of SrRuO ₃ and GDC, the GDC electrolyte powder and the SrRuO ₃ powder were mixed so that SrRuO ₃ : GDC = 30: 70 (volume ratio), and distilled water was added and stirred for 6 hours. Went. Then, it lyophilized | freeze-dried and calcined at 600 degreeC in the air for 1 hour.

Then, three types of electrochemical cells shown in Table 1 were prepared using the above-mentioned mixed powder for GDC electrolyte membrane and electrode. The details will be described below.

First, a cathode electrode powder, a GDC electrolyte membrane, and an anode electrode powder were sequentially inserted into a molding machine having a diameter of 10 mm, and uniaxial pressure molding was performed at 100 MPa for 1 minute. Thereafter, isostatic pressing was performed at 298 MPa for 1 minute. The amount of the cathode electrode powder and the anode electrode powder was 1.3 g.

After isostatic pressing, co-sintering was performed in air for 2 hours. Electrochemical cell No. In the production of No. 1, the co-sintering temperature was set to 1000 ° C. 2 and no. In the production of 3, the co-sintering temperature was 1200 ° C. The co-sintering temperature was made different in this way in another experiment, when the NiO and GDC mixed powder was co-sintered at 1200 ° C., the RuO ₂ and GDC mixed powder was co-sintered. It was found that the shrinkage rate was higher and the gas flow rate was lower than when the SrRuO ₃ and GDC mixed powder was co-sintered at 1200 ° C. is there.

Subsequently, on both sides of the co-sintered body obtained by co-sintering, that is, on the portion where the powder for the electrode is sintered, a Pt mesh (current collector) in which Pt wire is welded using Pt paste. Glued. Next, the co-sintered body to which such Pt wires were connected was set in an alumina holder, and the gap between them was closed using a glass ring and glass powder. Electrochemical cell No. 3 was completed in this way.

Electrochemical cell No. 1 and no. In the preparation of 2, by further supplying a mixed gas of 97% by volume H ₂ and 3% H ₂ O to the co-sintered body at a flow rate of 50 ml / min, and performing a reduction treatment at 700 ° C. for 24 hours, NiO and RuO ₂ in the mixed powder for electrodes were changed to Ni and Ru, respectively. Electrochemical cell No. 1 and no. 2 was completed in this way.

Electrochemical cell No. 1-No. After producing 2, dry reforming was performed using these. In this dry reforming, the temperature was reduced from 400 ° C., which is the temperature of the reduction treatment, to 400 ° C. while flowing argon gas. Then, the electrochemical cell no. 1-No. 1.00 V was applied to 2. Then, CH ₄ and CO ₂ were allowed to flow at a flow rate of 25 ml / min on the cathode side. The dry forming temperature is the same as that of the electrochemical cell No. 1 is 400 ° C. and 500 ° C. 2, the temperature was set to 400 ° C. to 800 ° C. 3 was 800 ° C. And the measurement of the flow rate of an exit gas and the analysis by a gas chromatograph were performed, and the current density of the electric current which flows through each electrochemical cell was measured. These results are shown in FIGS. FIG. 12 shows the relationship between the temperature and time of dry forming (reforming) and the flow rate and current density of the outlet gas. FIG. 13 shows the temperature and time of dry forming (reforming) at 800 ° C. and the results of gas chromatographic analysis of the outlet gas.

As shown in FIG. 12, electrochemical cell no. In No. 1, when the dry forming temperature increased, the outlet gas flow rate rapidly decreased at 500 ° C., and the current density increased rapidly.

On the other hand, electrochemical cell No. 1 in which Ru is contained in the anode electrode. In No. 2, the outlet gas flow rate increased as the dry forming temperature increased. In addition, as shown in FIG. In 2, the amount of CH ₄ gas and CO ₂ gas decreased and the amount of H ₂ gas and CO gas increased as the temperature of dry forming increased. This indicates that dry reforming was promoted as the temperature increased.

Furthermore, as shown in FIG. Electrochemical cell no. 3 was promoted. In addition, electrochemical cell No. 2 and no. In No. 3, the gas flow rate did not decrease until reforming for at least 10 hours. Then, the amount of generated H ₂ gas and CO gas were similar to each other. The electrochemical cell No. In No. 3, the flow rate began to decrease after 13 hours of reforming, and carbon was deposited on the Pt mesh of the cathode electrode.

The present invention can be used for synthesis of fuel gas using an oxidation-reduction reaction.

Claims

An anode electrode containing ruthenium;
A cathode electrode containing ruthenium or nickel;
A porous electrolyte membrane provided between the anode electrode and the cathode electrode and containing a metal oxide exhibiting oxide ion conductivity;
An electrochemical reactor comprising:
The electrolyte membrane contains at least one selected from the group consisting of a cerium-rare earth element oxide, a zirconium-yttrium oxide, and a lanthanum-gallium oxide as the metal oxide. The electrochemical reactor according to claim 1.
The electrochemical reactor according to claim 1, wherein the anode electrode contains at least one selected from the group consisting of metal ruthenium, ruthenium oxide, and strontium ruthenium oxide.
The electrochemical reactor according to claim 1, wherein the cathode electrode contains a material constituting the electrolyte membrane and nickel or ruthenium.
2. The electrochemical reactor according to claim 1, wherein the thickness of the electrolyte membrane is 10 μm to 100 μm.
A porous electrolyte membrane containing an anode electrode containing ruthenium, a cathode electrode containing ruthenium or nickel, and a metal oxide provided between the anode electrode and the cathode electrode and exhibiting oxide ion conductivity And a method for producing fuel gas using an electrochemical reactor comprising:
Applying a voltage between the anode electrode and the cathode electrode;
Supplying a gas containing methane and carbon dioxide toward the cathode electrode;
A method for producing fuel gas, comprising: