A method for reducing carbon dioxide with use of a device for reducing carbon dioxide includes steps of (a) preparing the device. The device includes a vessel, a cathode electrode and an anode electrode. An electrolytic solution is stored in the vessel, the cathode electrode contains a copper rubeanate metal organic framework, the copper rubeanate metal organic framework is in contact with the electrolytic solution, the anode electrode is in contact with the electrolytic solution, and the electrolytic solution contains carbon dioxide. The method further includes step of (b) applying a voltage difference between the cathode electrode and the anode electrode so as to reduce the carbon dioxide.

Description

9 parts

›This application is a Continuation of PCT/JP2012/003502 filed…

This application is a Continuation of PCT/JP2012/003502 filed on May 29, 2012, which claims foreign priority of Japanese Patent Application No. 2011-185493 filed on Aug. 29, 2011, the entire contents of both of which are incorporated herein by reference.

›TECHNICAL FIELD

The present disclosure relates to a method for reducing carbon dioxide.

›SUMMARY

One of the purposes of the present disclosure is to provide a novel method for reducing carbon dioxide.

According to one aspect of the present disclosure, a method for reducing carbon dioxide with use of a device for reducing carbon dioxide includes the following steps (a) and (b). In step (a), the device for reducing carbon dioxide is prepared. The device includes a vessel, a cathode electrode, and an anode electrode. An electrolytic solution is stored in the vessel. The cathode electrode contains a copper rubeanate metal organic framework, and the copper rubeanate metal organic framework is in contact with the electrolytic solution. The anode electrode is in contact with the electrolytic solution, and the electrolytic solution contains carbon dioxide. In step (b), a voltage difference is applied between the cathode electrode and the anode electrode so as to reduce the carbon dioxide.

In some embodiments, the vessel may include a solid electrolyte membrane. The solid electrolyte membrane may be interposed between the cathode electrode and the anode electrode.

In some embodiments, in the step (b), the voltage difference may be not less than 2 volts.

In some embodiments, in the step (b), the carbon dioxide may be reduced on the cathode electrode.

In some embodiments, in the step (b), formic acid may be generated on the cathode electrode.

According to another aspect of the present disclosure, a method for generating formic acid includes the following steps (a) and (b). In step (a), a device is prepared. The device includes a vessel, a cathode electrode, and an anode electrode. An electrolytic solution is stored in the vessel. The cathode electrode contains a copper rubeanate metal organic framework and the copper rubeanate metal organic framework is in contact with the electrolytic solution. The anode electrode is in contact with the electrolytic solution, and the electrolytic solution contains carbon dioxide. In step (b), a voltage is applied difference between the cathode electrode and the anode electrode so as to generate the formic acid.

In some embodiments, the vessel may comprise a solid electrolyte membrane. The solid electrolyte membrane may be interposed between the cathode electrode and the anode electrode.

In some embodiments, in the step (b), the voltage difference may be not less than 2 volts.

In some embodiments, in the step (b), the carbon dioxide may be reduced on the cathode electrode.

In some embodiments, in the step (b), the formic acid may be generated on the cathode electrode.

The present disclosure provides a novel method for reducing carbon dioxide. In particular, the disclosed method is efficient in producing formic acid.

›BRIEF DESCRIPTION OF DRAWINGS

FIG. 1 shows an exemplary device for reducing carbon oxide according to the embodiment 1.

FIG. 2 shows a measurement result of the liquid chromatography according to the example 1A.

FIG. 3 shows a measurement result of the liquid chromatography according to the example 2A.

›DESCRIPTION OF EMBODIMENTS

The embodiment of the present disclosure is described below.

(Step (a))

In the step (a), a device 20 for reducing carbon dioxide is prepared.

As shown in FIG. 1 , the device 20 includes a vessel 21 , a cathode electrode 11 , and an anode electrode 13 .

An electrolytic solution 15 is stored in the vessel 21 . An example of the electrolytic solution 15 is a potassium bicarbonate aqueous solution or a potassium chloride aqueous solution. The electrolytic solution 15 contains carbon dioxide. It is preferable that the electrolytic solution 15 is weakly acidic in the state where carbon dioxide is dissolved in the electrolytic solution 15 .

The cathode electrode 11 contains a copper rubeanate metal organic framework. The copper rubeanate metal organic framework may be found in Japanese laid-open patent application publication No. Hei 05-074458, and has the following molecular structure.

An example of a method for preparing the cathode electrode 11 is described below.

First, a rubeanic acid solution is mixed to a solution containing copper ion to obtain precipitated particles each formed of copper rubeanate metal organic framework. The obtained particles each formed of copper rubeanate metal organic framework were dispersed in an organic solvent so as to obtain slurry. An example of the organic solvent is isopropyl alcohol.

Then, this slurry is applied to a conductive substrate to obtain a cathode electrode 11 .

It is preferable that the conductive substrate has a shape of a film or a plate. An example of the conductive substrate is a carbon paper, a metal substrate, a glassy carbon substrate or a conductive silicon substrate.

The cathode electrode 11 is in contact with the electrolytic solution 15 . To be more exact, the copper rubeanate metal organic framework included in the cathode electrode 11 is in contact with the electrolytic solution 15 . In FIG. 1 , the cathode electrode 11 is immersed in the electrolytic solution 15 . Only a part of the cathode electrode 11 may be immersed in the electrolytic solution 15 , as long as the copper rubeanate metal organic framework is in contact with the electrolytic solution 15 .

The anode electrode 13 contains a conductive material. An example of the suitable conductive material is carbon, platinum, gold, silver, copper, titanium, or iridium oxide. The material of the conductive material is not limited, as long as the conductive material is not decomposed.

The anode electrode 13 is in contact with the electrolytic solution 15 . To be more exact, the conductive material comprised in the anode electrode 13 is in contact with the electrolytic solution 15 . In FIG. 1 , the anode electrode 13 is immersed in the electrolytic solution 15 . Only a part of the anode electrode 13 may be immersed in the electrolytic solution 15 , as long as the conductive material is in contact with the electrolytic solution 15 .

As shown in FIG. 1 , it is preferable the vessel 21 includes a tube 17 . Carbon dioxide is supplied to the electrolytic solution 15 through the tube 17 . One end of the tube 17 is immersed in the electrolytic solution 15 .

It is preferable that a solid electrolyte membrane 16 is provided in the vessel 21 . This reason is mentioned later in the step (b). An example of the solid electrolyte membrane 16 is a Nafion (registered trademark) film available from Du Pont Kabushiki Kaisha. Only protons can penetrate the solid electrolyte membrane 16 .

The solid electrolyte membrane 16 is interposed between the cathode electrode 11 and the anode electrode 13 . The solid electrolyte membrane 16 divides the electrolytic solution 15 into an anode liquid 15 L and a cathode liquid 15 R. The anode electrode 13 is in contact with the anode liquid 15 L. The cathode electrode 11 is in contact with the cathode liquid 15 R.

As shown in FIG. 1 , it is preferable that a reference electrode 12 is provided. The reference electrode 12 is in contact with the electrolytic solution 15 . When the solid electrolyte membrane 16 is used, the reference electrode 12 is in contact with the cathode liquid 15 R. The reference electrode 12 is electrically connected to the cathode electrode 11 . An example of the reference electrode 12 is a silver/silver chloride electrode.

(Step (b))

In the step (b), the voltage difference is applied between the cathode electrode 11 and the anode electrode 13 . This causes carbon dioxide contained in the electrolytic solution 15 (to be more exact, the cathode liquid 15 R) to be reduced on the cathode electrode 11 . As a result, formic acid is produced on the cathode electrode 11 .

Oxygen is produced by oxidizing water on the anode electrode 13 . The solid electrolyte membrane 16 inhibits a reverse reaction which may occur on the anode electrode 13 . In other words, if the formic acid generated on the cathode electrode 11 reaches the anode electrode 13 , the formic acid would be oxidized on the anode electrode 13 . As a result, the generated formic acid would return to carbon dioxide. The solid electrolyte membrane 16 inhibits this reverse reaction.

It is preferable that a potentiostat 14 is used to apply a voltage difference between the cathode electrode 11 and the anode electrode 13 .

It is preferable that the voltage difference applied between the cathode electrode 11 and the anode electrode 13 is 2.0 volts or more.

›Examples3

›Example 1A

Preparation of Cathode Electrode 11

A cathode electrode 11 according to the example 1 was prepared as below. Rubeanic acid used in the example 1 was purchased from Wako Pure Chemical Industries, Ltd.

An ethanol solution of rubeanic acid having a concentration of 50 mM and an aqueous solution of cupric sulfate having a concentration of 50 mM were mixed to prepare a mixture. A precipitation was observed in the mixture. The precipitation was separated by centrifuge. The precipitation was washed with ethanol and subsequently washed with distilled water. Finally, the precipitation was air-dried. Thus, particles each formed of copper rubeanate metal organic framework (hereinafter, referred to as “CR-MOF”) were obtained. The CR-MOF particles had an average particle diameter of approximately 3 micrometers.

Then, these particles were dispersed in isopropyl alcohol to prepare slurry of CR-MOF.

The slurry of CR-MOF was dropped on a conductive carbon paper (hereinafter, referred to as “CP”) having a thickness of 0.36 millimeters and air-dried. In this manner, the cathode electrode 11 according to the example 1 was prepared. The distribution density of the CR-MOF particles on the cathode electrode 11 is approximately 1×10 7 /cm 2 .

(Preparation of Device 20 )

A device 20 shown in FIG. 1 was prepared with use of the cathode electrode 11 thus obtained. The vessel 21 had a volume of 230 milliliters. The reference electrode 12 and the anode electrode 13 were an Ag/AgCl electrode and a platinum wire electrode, respectively. An electrolytic solution 15 was a potassium bicarbonate (KHCO 3 ) aqueous solution having a concentration of 0.5M. In other words, both of the cathode liquid 15 R and the anode liquid 15 L were a potassium bicarbonate (KHCO 3 ) aqueous solution having a concentration of 0.5M. The amount of the electrolytic solution 15 was 140 milliliters. A solid electrolyte membrane 16 was purchased from Sigma-Aldrich Japan K.K. (trade name: Nafion (Registered trade mark) 117 ).

(Injection of Carbon Dioxide)

Carbon dioxide was injected by bubbling to the cathode liquid 15 R at a flow rate of 200 milliliters/minute for thirty minutes through the tube 17 . In this way, the carbon dioxide was saturated in the cathode liquid 15 R. The vessel having a volume of 230 milliliters included a lid (not shown), and had the electrolytic solution 15 (liquid phase) of 140 milliliters and gaseous carbon dioxide (gas phase) having a volume of 90 milliliters. The device 20 was sealed by the lid.

(Reduction of Carbon Dioxide)

Voltages of −1.4 volts, 0 volts, and +1.2 volts were applied to the cathode electrode 11 , the reference electrode 12 , and the anode electrode 13 , respectively. The current was 10 milli-amperes. This state was maintained for 1,000 seconds, namely 16 minutes 40 seconds. The total electric charge amount was 10 coulombs. Subsequently, a liquid phase component and a gas phase component were collected with use of syringes. The collected liquid phase component was analyzed with a liquid chromatography. The collected gas phase component was analyzed with a gas chromatography. The result is shown in Table 1.

›Example 1B

An experiment similar to the example 1A was performed, except that a voltage of −1.5 volts was applied to the cathode electrode 11 . The result is shown in Table 1.

›Example 1C

An experiment similar to the example 1A was performed, except that a voltage of −1.6 volts was applied to the cathode electrode 11 . The result is shown in Table 1.

Comparative Example 1A

An experiment similar to the example 1A was performed, except that the slurry of CR-MOF was not dropped on a carbon paper and a voltage of −1.8 volts was applied to the cathode electrode 11 . In other words, in the comparative example 1, the cathode electrode 11 was formed of a carbon paper. The result is shown in Table 1.

Comparative Example 1B

An experiment similar to the example 1A was performed, except that a copper electrode was used as the cathode electrode 11 and a voltage of −1.8 volts was applied to the cathode electrode 11 . The result is shown in Table 1.

Examples 2 and Comparative Examples 2

Experiments similar to the examples 1A and 1C and the comparative examples 1A and 1B were performed, except that a potassium chloride (KCl) aqueous solution having a concentration of 0.5M was used as the electrolytic solution 15 instead of the potassium bicarbonate (KHCO 3 ) aqueous solution. In the experiments similar to the comparative examples 1A and 1B, voltages applied to the cathode electrode 11 were different from those of the comparative examples 1A and 1B. The result is shown in Table 2.

Table 1 and Table 2 show amounts of formic acid, carbon monoxide, methane, ethylene, and ethane generated in the examples and the comparative examples.

As is clear from Table 1 and Table 2, the carbon oxide is reduced to formic acid in the examples. The generation rate of formic acid according to the examples is higher than those according to the comparative examples.

›INDUSTRIAL APPLICABILITY

The present disclosure provides a novel method for reducing carbon dioxide. In particular, the disclosed methods are efficient in producing formic acid.

›Tables in the description — 2

TABLE 1 — Electric

Solution	Potential of	amounts of the products [micro mol]	Selectivity
0.5M KHCO 3	Cathode	electrolysis	HCOOH	CO	CH 4	C 2 H 4	C 2 H 6	of HCOOH
Example 1A	CR-MOF	−1.4 V	9.5	0.02	0.001	0.0001	0.0001	99.8%
Example 1B	CR-MOF	−1.5 V	8.9	0.05	0.004	0.0003	0.0006	99.4%
Example 1C	CR-MOF	−1.6 V	12.9	0.05	0.007	0.0004	0.0006	99.6%
Comparative	CP	−1.8 V	0.2	0.02	0.016	0.0007	0.0014	84.1%
Example 1A
Comparative	Cu	−1.8 V	13.7	0.21	0.64	0.047	0.0004	93.9%
Example 1B

TABLE 2 — Electric

Solution		Potential of	amounts of the products [micro mol]	Selectivity
0.5M KCl	Cathode	electrolysis	HCOOH	CO	CH 4	C 2 H 4	C 2 H 6	of HCOOH
Example 2A	CR-MOF	−1.4 V	11.3	0.07	0.01	0.002	0.003	99.2%
Example 2B	CR-MOF	−1.6 V	22.3	0.22	0.02	0.003	0.003	98.9%
Comparative	CP	−2.0 V	2.6	0.26	0.04	0.001	0.001	89.8%
Example 2A
Comparative	Cu	−1.6 V	2.7	0.89	0.75	2.684	0.002	38.2%
Example 2B

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Claims as granted

12 claims

Classifications

11 codes

IPC · International Patent Classification

Section B — Performing operations; transporting

B01J27/04

Section C — Chemistry; metallurgy

C01B32/40
C25B9/19
C25B3/29
C25B3/25
C25B3/23
C07C53/02

USPC · US Patent Classification

205/440205/462205/555205/415

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