WO2014102898A1 - 電力貯蔵電池 - Google Patents
電力貯蔵電池 Download PDFInfo
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- WO2014102898A1 WO2014102898A1 PCT/JP2012/083453 JP2012083453W WO2014102898A1 WO 2014102898 A1 WO2014102898 A1 WO 2014102898A1 JP 2012083453 W JP2012083453 W JP 2012083453W WO 2014102898 A1 WO2014102898 A1 WO 2014102898A1
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- positive electrode
- electrode electrolyte
- manganese
- redox
- storage battery
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- H—ELECTRICITY
- H01—ELECTRIC ELEMENTS
- H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
- H01M8/00—Fuel cells; Manufacture thereof
- H01M8/18—Regenerative fuel cells, e.g. redox flow batteries or secondary fuel cells
- H01M8/184—Regeneration by electrochemical means
- H01M8/188—Regeneration by electrochemical means by recharging of redox couples containing fluids; Redox flow type batteries
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- H—ELECTRICITY
- H01—ELECTRIC ELEMENTS
- H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
- H01M8/00—Fuel cells; Manufacture thereof
- H01M8/20—Indirect fuel cells, e.g. fuel cells with redox couple being irreversible
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- Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
- Y02—TECHNOLOGIES OR APPLICATIONS FOR MITIGATION OR ADAPTATION AGAINST CLIMATE CHANGE
- Y02E—REDUCTION OF GREENHOUSE GAS [GHG] EMISSIONS, RELATED TO ENERGY GENERATION, TRANSMISSION OR DISTRIBUTION
- Y02E60/00—Enabling technologies; Technologies with a potential or indirect contribution to GHG emissions mitigation
- Y02E60/30—Hydrogen technology
- Y02E60/50—Fuel cells
Definitions
- the present invention relates to a power storage battery such as a redox flow battery.
- Patent Document 1 discloses a positive electrode electrolyte solution containing a manganese redox material and a complexing agent or chelating agent.
- Patent Document 1 describes aminopolycarboxylic acid, polycarboxylic acid, amino acid, oxyacid, polyalcohol, ⁇ -diketone, amine, and polyphosphoric acid.
- Non-Patent Document 1 describes that a Mn (III) -EDTA complex (ethylenediaminetetraacetatomanganate (III) complex) self-decomposes while generating carbon dioxide gas.
- Mn (III) -EDTA complex ethylenediaminetetraacetatomanganate (III) complex
- a strongly acidic electrolyte is used in a power storage battery.
- the metal redox ions are stably dissolved even at a relatively high concentration, so that the energy density of the battery can be increased.
- the ion-conducting carriers are H + ions or OH ⁇ ions. Since both the mobility of H + ions and the mobility of OH ⁇ ions are relatively high, the conductivity of the electrolytic solution is high. As a result, the battery resistance increases, resulting in an increase in battery efficiency.
- the material constituting the redox flow battery is required to have chemical resistance that can withstand the electrolytic solution.
- the chemical resistance necessary for the material constituting the battery can be reduced, and as a result, the manufacturing cost of the power storage battery can be reduced.
- the metal redox ions are difficult to dissolve stably. It is considered that the disadvantage that the solubility of metal redox ions is lowered in an electrolytic solution having a pH of 3 or more can be compensated by complexing metal redox ions by adding a chelating agent to the electrolytic solution.
- a chelating agent there is no report of practical use yet.
- the redox material of manganese is relatively inexpensive and has a high oxidation-reduction potential, so that it is advantageous as a redox material used for a positive electrode electrolyte of a power storage battery.
- Patent Document 1 described above describes that in a positive electrode electrolyte containing a manganese redox material and a chelating agent, precipitation of the manganese redox material is suppressed.
- the Mn (III) -EDTA complex since the Mn (III) -EDTA complex is self-decomposing with the generation of carbon dioxide gas, the original battery performance of the manganese redox system is exhibited. hard.
- the present invention has been made in view of such circumstances, and the object thereof is to easily use a manganese redox substance in the electrolyte even when the pH of the electrolyte is 3 or more. It is to provide a storage battery.
- n an integer of 0 to 4, and R 1 , R 2 , R 3 and R 4 independently represent a hydrogen atom, a methyl group or ethyl
- n 0, at least one selected from R 1 , R 2 , R 3 and R 4 represents a methyl group or an ethyl group). I will provide a.
- the amine preferably contains at least one selected from diethylenetriamine, triethylenetetramine, and N, N′-dimethylethylenediamine.
- the molar ratio of the amine to the redox substance of manganese in the positive electrode electrolyte is preferably in the range of 1 or more and 5 or less.
- the positive electrode electrolyte contains the manganese redox substance by dissolving manganese sulfate in water.
- the content of the manganese redox substance in the positive electrode electrolyte is in a range of 0.2 mol / L or more and 1.0 mol / L or less.
- the positive electrode electrolyte has a pH in the range of 3 or more and 7 or less.
- the positive electrode electrolyte is prepared by an electrolytic oxidation reaction of the manganese redox material in the presence of the amine.
- the redox flow battery includes a charge / discharge cell 11.
- the inside of the charge / discharge cell 11 is partitioned into a positive electrode side cell 21 and a negative electrode side cell 31 by a diaphragm 12.
- the redox flow type battery includes a positive electrode electrolyte tank 23 that stores a positive electrode electrolyte 22 used for the positive electrode side cell 21, and a negative electrode electrolyte tank 33 that stores a negative electrode electrolyte 32 used for the negative electrode side cell 31.
- the redox flow battery is provided with a temperature adjusting device for adjusting the temperature around the charge / discharge cell 11 as necessary.
- a positive electrode 21 a and a positive electrode current collector plate 21 b are arranged in contact with each other.
- the negative electrode 31a and the negative electrode side current collecting plate 31b are arranged in contact with each other.
- the positive electrode 21a and the negative electrode 31a are made of, for example, carbon felt.
- the positive electrode side current collector plate 21b and the negative electrode side current collector plate 31b are made of, for example, a glassy carbon plate.
- Each of the current collector plates 21 b and 31 b is electrically connected to the charging / discharging device 10.
- a positive electrode electrolyte tank 23 is connected to the positive electrode side cell 21 via a supply pipe 24 and a recovery pipe 25.
- the supply pipe 24 is equipped with a pump 26.
- the positive electrolyte solution 22 in the positive electrode electrolyte tank 23 is supplied to the positive electrode side cell 21 through the supply pipe 24.
- the positive electrode electrolyte 22 in the positive electrode side cell 21 is recovered in the positive electrode electrolyte tank 23 through the recovery tube 25. In this way, the positive electrode electrolyte 22 is circulated through the positive electrode electrolyte tank 23 and the positive electrode side cell 21.
- a negative electrode electrolyte tank 33 is connected to the negative electrode side cell 31 via a supply pipe 34 and a recovery pipe 35.
- the supply pipe 34 is equipped with a pump 36.
- the negative electrode electrolyte 32 in the negative electrode electrolyte tank 33 is supplied to the negative electrode side cell 31 through the supply pipe 34.
- the negative electrode electrolyte 32 in the negative electrode side cell 31 is recovered in the negative electrode electrolyte tank 33 through the recovery pipe 35.
- the negative electrode electrolyte 32 is circulated through the negative electrode electrolyte tank 33 and the negative electrode side cell 31.
- the inert gas supply pipe 13 for supplying an inert gas is connected to the charge / discharge cell 11, the positive electrode electrolyte tank 23, and the negative electrode electrolyte tank 33.
- the inert gas supply pipe 13 is supplied with an inert gas from an inert gas generator.
- the positive electrode electrolyte tank 23 and the negative electrode electrolyte tank 33 are supplied with an inert gas through the inert gas supply pipe 13 so that the positive electrode electrolyte 22 and the negative electrode electrolyte 32 are in contact with oxygen in the atmosphere. It is suppressed.
- nitrogen gas is used as the inert gas.
- the inert gas supplied to the positive electrode electrolyte tank 23 and the negative electrode electrolyte tank 33 is exhausted through the exhaust pipe 14.
- a water seal 15 for sealing the opening of the exhaust pipe 14 is provided at the tip of the exhaust pipe 14 on the discharge side.
- the water seal 15 prevents the air from flowing back into the exhaust pipe 14 and keeps the pressure in the positive electrolyte tank 23 and the negative electrolyte tank 33 constant.
- an oxidation reaction is performed in the positive electrode electrolyte solution 22 in contact with the positive electrode 21a, and a reduction reaction is performed in the negative electrode electrolyte solution 32 in contact with the negative electrode 31a. That is, the positive electrode 21a emits electrons and the negative electrode 31a receives electrons.
- the positive collector plate 21b supplies the electrons discharged from the positive electrode 21a to the charging / discharging device 10.
- the negative electrode current collector 31b supplies the electrons received from the charge / discharge device 10 to the negative electrode 31a.
- the negative electrode current collector 31b collects the electrons emitted from the negative electrode 31a and supplies them to the charging / discharging device 10.
- a reduction reaction is performed in the positive electrode electrolyte 22 in contact with the positive electrode 21a, and an oxidation reaction is performed in the negative electrode electrolyte 32 in contact with the negative electrode 31a. That is, the positive electrode 21a receives electrons and the negative electrode 31a emits electrons. At this time, the positive collector plate 21b supplies the electrons received from the charge / discharge device 10 to the positive electrode 21a.
- the redox flow type battery includes a positive electrode electrolyte solution 22 containing a redox material of manganese and an amine.
- Manganese functions as an active material in the positive electrode electrolyte 22, and for example, oxidation occurs from Mn (III) to Mn (IV) during charging, and Mn (IV) to Mn (III) during discharge. It is speculated that the reduction will occur.
- the concentration of manganese redox substance (manganese ions) in the positive electrode electrolyte 22 is preferably 0.1 mol / L or more, more preferably 0.2 mol / L or more, from the viewpoint of increasing the energy density. More preferably 0.4 mol / L or more.
- the concentration of manganese redox material (manganese ions) in the positive electrode electrolyte 22 is preferably 2.5 mol / L or less, more preferably 1 from the viewpoint of further suppressing precipitation of manganese redox material. 0.5 mol / L or less, more preferably 1.0 mol / L or less, and most preferably 0.8 mol mol / L or less.
- the amine contained in the positive electrode electrolyte 22 is represented by the following general formula (1).
- n any integer of 0 to 4
- R 1 , R 2 , R 3 and R 4 independently represent a hydrogen atom, a methyl group or an ethyl group
- n In the case of 0, at least one selected from R 1 , R 2 , R 3 and R 4 represents a methyl group or an ethyl group.
- the amine represented by the general formula (1) is a kind of chelating agent and has a function of forming a complex with manganese redox substance and suppressing precipitation of manganese redox substance in the positive electrode electrolyte 22.
- the positive electrode electrolyte solution 22 may contain only one kind of amine represented by the general formula (1), or may contain plural kinds.
- the positive electrode electrolyte 22 preferably contains at least one amine selected from diethylenetriamine, triethylenetetramine, and N, N′-dimethylethylenediamine.
- the molar ratio of the amine represented by the general formula (1) to the redox substance of manganese in the positive electrode electrolyte 22 is preferably in the range of 1 or more and 5 or less. When the molar ratio is 1 or more, it becomes even easier to suppress the precipitation of manganese redox substances. When the molar ratio is 5 or less, the reactivity and charge / discharge cycle characteristics (reversibility) tend to increase.
- the pH of the positive electrode electrolyte 22 is preferably in the range of 3 to 7, more preferably in the range of 5 to 7.
- the pH of the positive electrode electrolyte 22 is 3 or more, corrosion resistance is easily ensured.
- the pH of the positive electrode electrolyte 22 is 7 or less, it becomes easy to further suppress the precipitation of manganese redox substances.
- the positive electrode electrolyte solution 22 can contain a chelating agent other than the amine represented by, for example, an inorganic acid salt or an organic acid salt, or the general formula (1), as necessary.
- the active material used for the negative electrode electrolyte 32 is not particularly limited, and examples thereof include iron redox materials, chromium redox materials, titanium redox materials, copper redox materials, and vanadium redox materials. It is done.
- the concentration of the metal redox substance (metal ion) in the negative electrode electrolyte solution 32 is preferably 0.1 mol / L or more, more preferably 0.2 mol / L or more, from the viewpoint of increasing the energy density. More preferably 0.4 mol / L or more.
- the concentration of the metal redox substance (metal ion) in the negative electrode electrolyte solution 32 is preferably 2.5 mol / L or less, more preferably 1. from the viewpoint of suppressing the precipitation of the metal redox substance. 5 mol / L or less.
- the active material used for the negative electrode electrolyte 32 for example, a copper redox material is suitable.
- copper sulfate (CuSO 4 ) is preferably dissolved in water so that chlorine ions are not included.
- CuSO 4 copper sulfate
- the copper in the negative electrode electrolyte 32 is reduced from Cu (II) to Cu (I) during charging and is oxidized from Cu (I) to Cu (II) during discharging.
- the negative electrode electrolyte 32 further contains a chelating agent.
- the molar ratio of the chelating agent to the metal redox substance in the negative electrode electrolyte 32 is preferably in the range of 0.5 or more and 10 or less, and more preferably in the range of 1 or more and 5 or less. preferable.
- the negative electrode electrolyte solution 32 may contain, for example, an inorganic acid salt or an organic acid salt, if necessary.
- the pH of the negative electrode electrolyte solution 32 is preferably in the range of 3 or more and 11 or less.
- the positive electrode electrolyte 22 and the negative electrode electrolyte 32 can be prepared by a known method.
- the cathode electrolyte 22 contains a manganese redox-based material, for example, it is preferable to dissolve manganese sulfate (MnSO 4 ) in water because it is easily available.
- MnSO 4 manganese sulfate
- the positive electrode electrolyte solution 22 is preferably prepared by an electrolytic oxidation reaction of a manganese redox material in the presence of an amine represented by the general formula (1).
- a positive electrode electrolyte 22 having a high potential with respect to a silver-silver chloride (saturated KCl) electrode can be obtained.
- the electrolytic oxidation reaction should be performed at a Coulomb amount of 100% or more, where the Coulomb amount obtained by multiplying the number of moles of manganese redox substance contained in the positive electrode electrolyte 22 by the Faraday constant is 100%. Is preferred.
- the water used for the positive electrode electrolyte 22 and the negative electrode electrolyte 32 preferably has a purity equal to or higher than that of distilled water.
- the redox flow battery is preferably charged and discharged with the positive electrode electrolyte 22 and the negative electrode electrolyte 32 in an inert gas atmosphere.
- the performance of a redox flow battery can be evaluated by, for example, charge / discharge cycle characteristics (reversibility), coulomb efficiency, voltage efficiency, energy efficiency, electrolyte utilization, electromotive force, and electrolyte potential.
- charge / discharge cycle characteristics reversibility
- coulomb efficiency voltage efficiency
- energy efficiency energy efficiency
- electrolyte utilization electromotive force
- electrolyte potential electrolyte potential
- the charge / discharge cycle characteristics are calculated by substituting the coulomb amount (A) for the first cycle discharge and the coulomb amount (B) for the 90th cycle discharge into the following formula (1).
- Charging / discharging cycle characteristics [%] B / A ⁇ 100 (1)
- the charge / discharge cycle characteristics are preferably 80% or more.
- the coulomb efficiency is calculated by substituting the coulomb amount (C) for charging and the coulomb amount (D) for discharging in a predetermined cycle into the following equation (2).
- the coulomb efficiency is preferably 80% or more in a value calculated from the coulomb amount at the 75th cycle, for example.
- the voltage efficiency is calculated by substituting the average terminal voltage (E) for charging and the average terminal voltage (F) for discharging in a predetermined cycle into the following formula (3).
- Voltage efficiency [%] F / E ⁇ 100 (3)
- the voltage efficiency is preferably 60% or more in a value calculated from the terminal voltage at the 75th cycle, for example.
- Energy efficiency is calculated by substituting the electric energy (G) for charging and the electric energy (H) for discharging in a predetermined cycle into the following formula (4).
- Energy efficiency [%] H / G ⁇ 100 (4)
- the energy efficiency is preferably 60% or more in a value calculated from the electric energy at the 75th cycle.
- the utilization rate of the electrolytic solution is obtained by multiplying the number of moles of the active material of the electrolytic solution supplied to the positive electrode 21a side or the negative electrode 31a side by the Faraday constant (96500 coulomb / mol) to obtain the amount of coulomb (I) and the first cycle. Is calculated by substituting the coulomb amount (I) and the coulomb amount (J) into the following equation (5).
- a smaller number of moles is adopted.
- the utilization rate of the electrolyte after the first cycle can be calculated in the same manner.
- Utilization rate of electrolytic solution [%] J / I ⁇ 100 (5)
- the utilization factor of the electrolytic solution is preferably 40% or more in the value calculated from the coulomb amount in the first cycle.
- the electromotive force is a terminal voltage when switching from charge to discharge in a predetermined cycle (when the current is 0 mA).
- the electromotive force is preferably 1.0 V or more at the terminal voltage in the first cycle.
- the potential of the electrolytic solution is shown as the potential of the graphite electrode with respect to the silver-silver chloride electrode during charge and discharge when a graphite electrode and a silver-silver chloride (saturated KCl) electrode are inserted in the positive electrode electrolyte tank 23 in advance.
- the redox flow battery of this embodiment includes a positive electrode electrolyte solution 22 containing a redox material of manganese and an amine represented by the general formula (1).
- a positive electrode electrolyte solution 22 containing a redox material of manganese and an amine represented by the general formula (1).
- the pH of the positive electrode electrolyte solution 22 is 3 or more, precipitation of manganese redox substances is suppressed. Therefore, even when the pH of the electrolytic solution is 3 or more, it becomes easy to use a manganese redox material.
- the positive electrode electrolyte 22 preferably contains at least one amine selected from diethylenetriamine, triethylenetetramine, and N, N′-dimethylethylenediamine.
- the amine is a relatively small molecule, and has one or two secondary amine type structures represented by C—NH—C in the molecule. It is presumed that a more stable complex is formed with the substance.
- the molar ratio of the amine represented by the general formula (1) with respect to the redox substance of manganese in the positive electrode electrolyte 22 is preferably in the range of 1 or more and 5 or less. In this case, it becomes easier to suppress the precipitation of manganese redox substances.
- manganese electrolyte is contained in the cathode electrolyte 22 by dissolving manganese sulfate in water.
- the manganese sulfate is easily available, the positive electrode electrolyte 22 can be easily obtained.
- the content of the manganese redox substance in the positive electrode electrolyte 22 is in the range of 0.2 mol / L or more and 1.0 mol / L or less, so that the energy density is increased and the redox of manganese is performed. It becomes easier to further suppress the precipitation of the system material.
- the positive electrode electrolyte solution 22 is preferably prepared by subjecting a manganese redox substance to an electrolytic oxidation reaction in the presence of an amine represented by the general formula (1). In this case, the obtained voltage can be further increased.
- the shape, arrangement, or number of the charge / discharge cells 11 of the redox flow battery and the capacities of the positive electrode electrolyte tank 23 and the negative electrode electrolyte tank 33 may be changed according to the performance required for the redox flow battery. . Further, the supply amount of the positive electrode electrolyte 22 and the negative electrode electrolyte 32 to the charge / discharge cell 11 can also be set according to, for example, the capacity of the charge / discharge cell 11.
- a power storage battery other than a redox flow battery may be used.
- Plot A1 in FIG. 2 shows that no precipitate was confirmed in the solubility test
- plot A2 shows that precipitate was confirmed in the solubility test
- the Mn (II) -TETA complex has a high utility value as an electrolyte for a redox flow battery because the solubility is ensured even when the pH of the aqueous solution is 3 or higher.
- the molar ratio of TETA to Mn (II) is set to 1, but the solubility of Mn (II) -TETA complex is improved by increasing the molar ratio of TETA to Mn (II). I think that.
- Example 1 ⁇ Redox flow battery> As a positive electrode and a negative electrode, the electrode area was set to 10 cm 2 using carbon felt (trade name: GFA5, manufactured by SGL). As the positive electrode side current collector plate, pure titanium having a thickness of 0.6 mm was used. As the negative electrode side current collector plate, a glassy carbon plate (trade name: SG carbon, thickness 0.6 mm, manufactured by Showa Denko KK) was used. As the diaphragm, a cation exchange membrane (CMS, manufactured by Astom Corp.) was used.
- CMS cation exchange membrane
- a glass container with a capacity of 30 mL was used as the positive electrode electrolyte tank and the negative electrode electrolyte tank. Silicone tubes were used as the supply pipe, recovery pipe, inert gas supply pipe, and exhaust pipe.
- a micro tube pump MP-1000, manufactured by Tokyo Rika Kikai Co., Ltd.
- PFX200 manufactured by Kikusui Electronics Co., Ltd.
- TETA triethylenetetramine
- TETA triethylenetetramine
- a positive electrode electrolyte was prepared by electrolytic oxidation of an aqueous Mn (II) -TETA complex solution using the redox flow battery.
- 20 mL of a Mn (II) -TETA complex aqueous solution was placed in a positive electrode electrolyte tank, and 20 mL of a Zn (II) -TETA complex aqueous solution was placed in a negative electrode electrolyte tank.
- the redox flow battery was charged with a constant current of 100 mA for 60 minutes (total 386 coulombs). Nitrogen gas was supplied from an inert gas supply pipe before and during the start of charging.
- the Mn (II) -TETA complex contained in the aqueous solution in the positive electrode electrolyte tank was electrolytically oxidized to prepare an aqueous solution having a Mn (III) -TETA complex concentration of 0.2 mol / L. was used as the positive electrode electrolyte.
- Mn (III) Mn (III)
- a charge / discharge test was performed using an aqueous Mn (III) -TETA complex solution obtained by electrolytic oxidation as the positive electrode electrolyte and using an aqueous Zn (II) -TETA complex solution as the negative electrode electrolyte.
- the charge / discharge test starts from charging, and is first performed at a constant current of 100 mA. Charged for 1 minute (total 180 coulombs). Next, the battery was discharged at a constant current of 100 mA with a final discharge voltage of 1.0V. Nitrogen gas was supplied from an inert gas supply pipe before and during the charge / discharge test.
- the redox reaction that performs charge and discharge is estimated as follows.
- FIG. 3 shows the transition of the battery voltage when charging and discharging from the 75th cycle to the 77th cycle.
- charge / discharge cycle characteristics (reversibility), Coulomb efficiency, voltage efficiency, energy efficiency, electrolyte utilization, electromotive force, and electrolyte potential were determined.
- Charging / discharging cycle characteristics were determined from the first cycle discharge coulomb amount (A) and the 90th cycle discharge coulomb amount (B).
- the coulomb efficiency was determined from the coulomb amount at the 75th cycle.
- the voltage efficiency was obtained from the average terminal voltage at the 75th cycle.
- the utilization rate of the electrolytic solution was determined from the amount of coulomb in the first cycle.
- the electromotive force was the terminal voltage in the first cycle.
- the redox flow battery was allowed to stand at room temperature (about 25 ° C.) for about 18 hours, and then the voltage of the graphite electrode relative to the silver-silver chloride electrode was measured, and the two voltages were compared.
- the positive electrode electrolyte after charging when charged under the above conditions contains Mn (IV) -TETA complex at a concentration of about 0.1 mol / L.
- nitrogen gas was supplied from an inert gas supply pipe before and during the start of the self-discharge test.
- Example 1 From the results of the charge / discharge test shown in Table 1, it can be seen that in Example 1, good battery characteristics can be obtained. From the results of the self-discharge test shown in Table 1, it can be seen that self-discharge is sufficiently suppressed in Example 1.
- Example 2 In Example 2, in the preparation of the Mn (II) -TETA complex aqueous solution of Example 1, TETA was changed to N, N′-dimethylethylenediamine (DMEDA), and the concentration of Mn (II) -DMEDA complex was similarly changed. A 0.2 mol / L aqueous solution was prepared. The Mn (II) -DMEDA complex in the obtained aqueous solution was electrolytically oxidized in the same manner as in Example 1 to prepare a Mn (III) -DMEDA complex aqueous solution.
- DMEDA N′-dimethylethylenediamine
- Example 2 A self-discharge test was conducted in the same manner as in Example 1 except that this Mn (III) -DMEDA complex aqueous solution was used as the positive electrode electrolyte. The result of the self-discharge test of Example 2 was equivalent to that of Example 1.
- Example 3 In Example 3, in the preparation of the Mn (II) -TETA complex aqueous solution of Example 1, TETA was changed to diethylenetriamine (DETA), and the concentration of Mn (II) -DETA complex was similarly 0.2 mol / L. An aqueous solution of was prepared. The Mn (II) -DETA complex in the obtained aqueous solution was electrolytically oxidized in the same manner as in Example 1 to prepare a Mn (III) -DETA complex aqueous solution. A self-discharge test was conducted in the same manner as in Example 1 except that this Mn (III) -DETA complex aqueous solution was used as the positive electrode electrolyte. The result of the self-discharge test of Example 3 was equivalent to that of Example 1.
- Example 4 In Example 4, in the preparation of the aqueous Mn (II) -TETA complex solution of Example 1, TETA was changed to tetramethylethylenediamine (TMEDA), and the concentration of Mn (II) -TMEDA complex was 0.2 mol in the same manner. / L aqueous solution was prepared. The Mn (II) -TMEDA complex in the obtained aqueous solution was electrolytically oxidized in the same manner as in Example 1 to prepare a Mn (III) -TMEDA complex aqueous solution. A self-discharge test was conducted in the same manner as in Example 1 except that this Mn (III) -TMEDA complex aqueous solution was used as the positive electrode electrolyte. The result of the self-discharge test of Example 4 was inferior to that of Example 1.
- Example 5 In Example 5, in the preparation of the Mn (II) -TETA complex aqueous solution of Example 1, TETA was changed to tetraethylenepentamine (TEPA), and the concentration of Mn (II) -TEPA complex was 0.2. A mol / L aqueous solution was prepared. The Mn (II) -TEPA complex in the obtained aqueous solution was electrolytically oxidized in the same manner as in Example 1 to prepare a Mn (III) -TEPA complex aqueous solution. A self-discharge test was conducted in the same manner as in Example 1 except that this Mn (III) -TEPA complex aqueous solution was used as the positive electrode electrolyte. The result of the self-discharge test of Example 5 was inferior to that of Example 1.
- Comparative Example 1 In Comparative Example 1, in the preparation of the Mn (II) -TETA complex aqueous solution of Example 1, TETA was changed to ethylenediamine (EDA), and the concentration of Mn (II) -EDA complex was similarly 0.2 mol / L. Attempts were made to prepare an aqueous solution. As a result, a precipitate was immediately generated, and therefore it was judged that it could not be used as an electrolyte for a redox flow battery.
- EDA ethylenediamine
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Abstract
Description
図1に示すように、レドックスフロー型電池は、充放電セル11を備える。充放電セル11の内部は、隔膜12によって正極側セル21と負極側セル31とに仕切られている。レドックスフロー型電池は、正極側セル21に用いられる正極電解液22を貯蔵する正極電解液タンク23と、負極側セル31に用いられる負極電解液32を貯蔵する負極電解液タンク33とを備える。レドックスフロー型電池には、充放電セル11周辺の温度を調節する温度調節装置が必要に応じて設けられる。
レドックスフロー型電池は、マンガンのレドックス系物質とアミンとを含有する正極電解液22を備える。マンガンは、正極電解液22中においてはマンガンが活物質として機能し、例えば、充電時には、Mn(III)からMn(IV)への酸化が起こり、放電時には、Mn(IV)からMn(III)への還元が起こると推測される。
マンガンのレドックス系物質と一般式(1)で表されるアミンとを含有する正極電解液22中では、マンガンのレドックス系物質と前記アミンとが錯体を形成することで、マンガンの析出が抑制される。また、この正極電解液22を用いることで、良好な電池性能が発揮される。
充放電サイクル特性は、80%以上であることが好ましい。
クーロン効率は、例えば、75サイクル目のクーロン量から算出される値において、好ましくは80%以上である。
電圧効率は、例えば、75サイクル目の端子電圧から算出される値において、好ましくは60%以上である。
エネルギー効率は、75サイクル目の電力量から算出される値において、好ましくは60%以上である。
電解液の利用率は、1サイクル目のクーロン量から算出される値において、好ましくは40%以上である。
前記実施形態は以下のように変更されてもよい。
蒸留水10mLに0.014モル(2.04g)のトリエチレンテトラミン(TETA)を溶解させた。この水溶液に、2.5モル/Lの希硫酸を添加することで、pHを6に調整した。この水溶液に、0.014モル(2.36g)のMnSO4・H2Oを溶解させた後、全量が20mLとなるように蒸留水を加えた。これにより、pHが6のMn(II)-TETA錯体水溶液を調製した。
<レドックスフロー型電池>
正極及び負極としては、カーボンフェルト(商品名:GFA5、SGL社製)を用いて電極面積を10cm2に設定した。正極側集電板としては、厚み0.6mmの純チタンを用いた。負極側集電板としては、ガラス状カーボン板(商品名:SGカーボン、厚み0.6mm、昭和電工株式会社製)を用いた。隔膜としては、陽イオン交換膜(CMS、アストム社製)を用いた。
蒸留水50mLに0.02モル(2.92g)のトリエチレンテトラミン(TETA)を溶解させた。この水溶液に、2.5モル/Lの希硫酸を添加することで、pHを6に調整した。この水溶液に、0.02モル(3.38g)のMnSO4・H2Oを溶解させた後、さらに0.05モル(7.1g)のNa2SO4を溶解させた。次に、この水溶液に、2.5モル/Lの希硫酸を添加することで、pHを5に調整した後に、全量が100mLとなるように蒸留水を加えた。これにより、マンガン(II)-TETA錯体の濃度が0.2モル/Lの水溶液を得た。
蒸留水50mLに0.04モル(5.84g)のトリエチレンテトラミン(TETA)を溶解させた。この水溶液に、0.02モル(5.75g)のZnSO4・7H2Oを溶解させた後、さらに0.05モル(7.1g)のNa2SO4を溶解させた。次に、この水溶液に、2.5モル/Lの希硫酸を添加することで、pHを6に調整した後に、全量が100mLとなるように蒸留水を加えた。これにより、Zn(II)-TETA錯体の濃度が0.2モル/Lの水溶液を得た。
上記レドックスフロー型電池を用いて、Mn(II)-TETA錯体水溶液を電解酸化することで、正極電解液を調製した。まず、正極電解液タンクにMn(II)-TETA錯体水溶液20mLを入れるとともに、負極電解液タンクにZn(II)-TETA錯体水溶液20mLを入れた。次に、レドックスフロー型電池を100mAの定電流で60分間(合計386クーロン)充電した。なお、充電の開始前及び期間中、不活性ガス供給管から窒素ガスを供給した。
正極電解液として電解酸化反応により得られたMn(III)-TETA錯体水溶液を用いるとともに、負極電解液としてZn(II)-TETA錯体水溶液を用いて充放電試験を行った。充放電試験は、充電から開始し、まず、100mAの定電流で30
分間充電した(合計180クーロン)。次に、100mAの定電流で、放電終止電圧を1.0Vとして放電した。なお、充放電試験の開始前及び期間中、不活性ガス供給管から窒素ガスを供給した。
負極:Zn(II)-TETA錯体+2e- ⇔ Zn(0)+TETA
75サイクル目から77サイクル目までの充放電した際の電池電圧の推移を図3に示す。
上記レドックスフロー型電池の正極電解液タンクに、電解酸化反応により得られたMn(III)-TETA錯体水溶液20mLを入れ、負極電解液タンクに、TETA水溶液20mLを入れた。また、正極電解液タンクに予め黒鉛電極と銀-塩化銀(飽和KCl)電極とを挿入した。次に、100mAの定電流で30分間充電(合計180クーロン)し、充電後の銀-塩化銀電極に対する黒鉛電極の電圧を測定した。続いて、レドックスフロー型電池を室温(約25℃)で約18時間静置した後、銀-塩化銀電極に対する黒鉛電極の電圧を測定し、両電圧を比較した。
実施例2では、実施例1のMn(II)-TETA錯体水溶液の調製において、TETAをN,N´-ジメチルエチレンジアミン(DMEDA)に変更し、同様にしてMn(II)-DMEDA錯体の濃度が0.2モル/Lの水溶液を調製した。得られた水溶液中のMn(II)-DMEDA錯体を実施例1と同様に電解酸化することで、Mn(III)-DMEDA錯体水溶液を調製した。このMn(III)-DMEDA錯体水溶液を正極電解液として用いた以外は、実施例1と同様にして自己放電試験を行った。実施例2の自己放電試験の結果は実施例1と同等であった。
実施例3では、実施例1のMn(II)-TETA錯体水溶液の調製において、TETAをジエチレントリアミン(DETA)に変更し、同様にしてMn(II)-DETA錯体の濃度が0.2モル/Lの水溶液を調製した。得られた水溶液中のMn(II)-DETA錯体を実施例1と同様に電解酸化することで、Mn(III)-DETA錯体水溶液を調製した。このMn(III)-DETA錯体水溶液を正極電解液として用いた以外は、実施例1と同様にして自己放電試験を行った。実施例3の自己放電試験の結果は実施例1と同等であった。
実施例4では、実施例1のMn(II)-TETA錯体水溶液の調製において、TETAをテトラメチルエチレンジアミン(TMEDA)に変更し、同様にしてMn(II)-TMEDA錯体の濃度が0.2モル/Lの水溶液を調製した。得られた水溶液中のMn(II)-TMEDA錯体を実施例1と同様に電解酸化することで、Mn(III)-TMEDA錯体水溶液を調製した。このMn(III)-TMEDA錯体水溶液を正極電解液として用いた以外は、実施例1と同様にして自己放電試験を行った。実施例4の自己放電試験の結果は実施例1よりも劣るものであった。
実施例5では、実施例1のMn(II)-TETA錯体水溶液の調製において、TETAをテトラエチレンペンタミン(TEPA)に変更し、同様にしてMn(II)-TEPA錯体の濃度が0.2モル/Lの水溶液を調製した。得られた水溶液中のMn(II)-TEPA錯体を実施例1と同様に電解酸化することで、Mn(III)-TEPA錯体水溶液を調製した。このMn(III)-TEPA錯体水溶液を正極電解液として用いた以外は、実施例1と同様にして自己放電試験を行った。実施例5の自己放電試験の結果は実施例1よりも劣るものであった。
比較例1では、実施例1のMn(II)-TETA錯体水溶液の調製において、TETAをエチレンジアミン(EDA)に変更し、同様にしてMn(II)-EDA錯体の濃度が0.2モル/Lの水溶液の調製を試みた。その結果、析出物が直ちに生じたため、レドックスフロー型電池の電解液としては使用不可能であると判断した。
Claims (7)
- 前記アミンは、ジエチレントリアミン、トリエチレンテトラミン、及びN,N´-ジメチルエチレンジアミンから選ばれる少なくとも一種を含む、請求項1に記載の電力貯蔵電池。
- 前記正極電解液中のマンガンのレドックス系物質に対する前記アミンのモル比は、1以上、5以下の範囲内とされる、請求項1又は請求項2に記載の電力貯蔵電池。
- 硫酸マンガンを水に溶解させることで前記正極電解液に前記マンガンのレドックス系物質を含有させる、請求項1から請求項3のいずれか一項に記載の電力貯蔵電池。
- 前記正極電解液中の前記マンガンのレドックス系物質の含有量が0.2モル/L以上、1.0モル/L以下の範囲内である、請求項1から請求項4のいずれか一項に記載の電力貯蔵電池。
- 前記正極電解液のpHが3以上、7以下の範囲内である、請求項1から請求項5のいずれか一項に記載の電力貯蔵電池。
- 前記正極電解液は、前記アミンの存在下で前記マンガンのレドックス系物質を電解酸化反応させることで調製される、請求項1から請求項6のいずれか一項に記載の電力貯蔵電池。
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JPS579073A (en) * | 1980-06-17 | 1982-01-18 | Agency Of Ind Science & Technol | Bedox battery |
JPS6215770A (ja) * | 1985-07-11 | 1987-01-24 | Yamaguchi Univ | レドックス二次電池 |
WO2012117543A1 (ja) * | 2011-03-02 | 2012-09-07 | 日新電機株式会社 | 電力貯蔵電池 |
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US4362791A (en) * | 1980-06-17 | 1982-12-07 | Agency Of Industrial Science & Technology | Redox battery |
JPH09507950A (ja) * | 1993-11-17 | 1997-08-12 | ユニサーチ リミテッド | 安定電解液およびその製造方法と、レドックス電池の製造方法、および安定した電解液を含む電池 |
EP0829104B1 (en) * | 1995-05-03 | 2003-10-08 | Pinnacle VRB Limited | Method of preparing a high energy density vanadium electrolyte solution for all-vanadium redox cells and batteries |
EP2355223B1 (en) * | 2010-01-29 | 2019-04-17 | Samsung Electronics Co., Ltd. | Redox flow battery including an organic electrolyte soution |
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JPS579073A (en) * | 1980-06-17 | 1982-01-18 | Agency Of Ind Science & Technol | Bedox battery |
JPS6215770A (ja) * | 1985-07-11 | 1987-01-24 | Yamaguchi Univ | レドックス二次電池 |
WO2012117543A1 (ja) * | 2011-03-02 | 2012-09-07 | 日新電機株式会社 | 電力貯蔵電池 |
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