JPH04101358A - Double fluid cell - Google Patents

Abstract

PURPOSE:To obtain a cell having high electromotive force and high function by using an acidic electrolyte and an alkaline electrolyte as a cathode electrolyte and an anode electrolyte, respectively and bipolar ion-exchange membrane as a diaphragm. CONSTITUTION:An acidic electrolyte 14 and an alkaline electrolyte 15 are used as a cathode electrolyte 12 and an anode electrolyte, respectively and a bipolar ion-exchange membrane 11 is used as a diaphragm. That is, the acidic electrolyte 14 and the alkaline electrolyte 15 are separated by the bipolar ion-exchange membrane 11 to prevent direct contact and neutralization reaction between these electrolytes and based on the mutural function of a cation-exchange group and an anode-exchange group by the bipolar ion-exchange membrane combination of the electrode reaction in the anodic electrolyte and the electrode reaction in the alkaline electrolyte is made possible. As a result, improved electromotive force is obtained.

Description

DETAILED DESCRIPTION OF THE INVENTION Field of Industrial Application The present invention comprises two different aqueous electrolytes using an acidic electrolyte and an alkaline electrolyte as the electrolytes of the positive and negative electrodes, respectively, and a bipolar ion exchange membrane as the diaphragm. Regarding batteries.

More specifically, the present invention relates to primary batteries, secondary batteries, redox flow batteries, zinc chloride batteries, zinc bromine batteries, and fuel cells that use two electrolytes (hereinafter referred to as two-component).

Prior Art Almost all conventional batteries that use aqueous electrolytes do not have membranes that can stably separate acidic and alkaline electrolytes over a long period of time, so they cannot use electrolytes that have either acidic or alkaline properties. , had a configuration that was commonly used for both positive and negative electrodes.

Problems to be Solved by the Invention However, in the conventional configuration described above, the reaction between the two electrodes occurs in either an acidic or alkaline electrolyte, so there is a difference between the reaction in an acidic electrolyte and the reaction in an alkaline electrolyte. It was not possible to obtain a practical electromotive force by combining the two. In addition, in an electrode using oxygen as an active material,
When air and an alkaline electrolytic solution are respectively used as sources of active material, there is a problem in that carbonates precipitate in the electrolytic solution.

The present invention solves the above-mentioned conventional problems, and provides a battery with higher performance than the conventional one by obtaining an electromotive force by combining an electrode reaction in an acidic electrolyte and an electrode reaction in an alkaline electrolyte. With the goal.

Means for Solving the Problems To achieve this object, the battery of the present invention is constructed using an acidic electrolyte and an alkaline electrolyte as positive and negative electrode electrolytes, and a bipolar ion exchange membrane as a diaphragm. It is.

Function: With this configuration, the bipolar ion exchange membrane separates acidic and alkaline electrolytes, preventing direct contact between the electrolytes and neutralization reactions, and the bipolar ion exchange membrane separating cations. The functions of both the exchange group and the anion exchange group make it possible to combine the electrode reaction in an acidic electrolyte and the electrode reaction in an alkaline electrolyte. As a result, as shown in the examples described later, it is possible to obtain a higher electromotive force than the conventional electromotive force between two electrodes in the same electrolytic solution.

The bipolar ion exchange membrane here is an amphoteric ion exchange membrane that shares a cation exchange group and an anion exchange group.
It is made from a composite of a cation exchange membrane and an anion exchange membrane, and has excellent permselectivity for hydrogen ions.

Further, as an example of the electrode using oxygen as the active material of the positive electrode described above, pure oxygen is used in a conventional oxygen-hydrogen fuel cell using an alkaline electrolyte in consideration of life characteristics, but the structure of the present invention By adopting this method and using a sulfuric acid electrolyte for the positive electrode, in addition to increasing the potential of the positive electrode, the electrolyte no longer deteriorates due to carbon dioxide gas, making it possible to use air as an oxidizing agent. .

Example Hereinafter, the present invention will be explained in more detail with reference to Examples.

FIG. 1 shows an H-type glass test cell used in the batteries of Examples (1) to (4) of the present invention. 11 indicates a bipolar ion exchange membrane. In the present invention, a membrane made of a copolymer of tetrafluoroethylene and perfluorovinylether and a membrane made of a copolymer of styrene and vinylhenzene were used as the bipolar ion exchange membrane. 12 is a positive electrode test piece, 13 is a negative electrode test piece, and acidic and alkaline electrolytes were placed in the electrolyte chambers 14 and 15, respectively. Sixteen stirrers were placed in each electrolyte chamber to stir the electrolyte as needed.

(Example 1) In the test cell shown in FIG. 1, a paste type lead dioxide electrode (reaction area 3.75 c♂), 3
A zinc plate (each with a reaction area of 9.75 cm) was used as the negative electrode of 14. The electrolyte chambers in 15 contained sulfuric acid (0.5M#) aqueous solution and potassium hydroxide (1.0M/#), respectively.
Q.) An example of constructing a zinc-lead battery by injecting an aqueous solution will be explained.

The reaction formula for the lead dioxide diameter of the positive electrode is as follows.

e PbO2+5O42+2e-+4)1";
PbSO4+2H20...(1) The potential of this electrode relative to the standard hydrogen electrode is +1.685V
It is.

On the other hand, the reaction formula at the negative zinc electrode is as follows.

e Zn+20H-;l:! Zn(OH)2+
2e - (2) The potential of this electrode relative to the standard hydrogen electrode is 1.245V. In the above two equations, the reaction from left to right is a discharge reaction, and the reaction from right to left is a charge reaction.

The theoretical battery voltage of a battery constructed with these two electrodes is 2
．． It is 93V.

When we measured the open circuit voltage of this battery at room temperature, we found that
It showed a stable voltage of 2.80 V. Further, FIG. 2 shows the results of a charge/discharge cycle test conducted at a constant current of 10 mA with an upper limit voltage of 3.5 V and a lower limit voltage of 2.2 V. As shown in FIG. 2, a flat potential of 2.4 to 2.3 V was exhibited during discharging, and a flat potential of 3.2 to 3.4 V was exhibited during charging.

In addition, the capacity gradually decreased with each repetition of charging and discharging, but in Example 1, charging and discharging up to 85 cycles were possible. Further, no abnormality was observed in the bipolar ion exchange membrane after the charge/discharge cycle test. There was no change in the appearance of lead oxide, but one tent light was formed on the zinc electrode, and zinc hydroxide was attached to the wall of the electrolyte chamber on the zinc electrode side. The decrease in cycle life is thought to be due to the zinc electrode, and it is thought that this can be easily improved by examining the battery configuration conditions, electrolyte concentration, and electrode materials.

It can be inferred that the following water decomposition reaction is progressing on the bipolar ion exchange membrane.

H2O,=! OH-+1+ ・
(3) In this equation, a reaction from left to right is a discharge reaction, and a reaction from right to left is a charge reaction.

During discharging, only hydrogen ions generated by water decomposition on the membrane selectively permeate through this bipolar ion exchange membrane, and during charging, hydrogen ions that permeate in the opposite direction combine with hydroxide ions generated at the zinc electrode. combine to form water. In this way, the bipolar ion exchange membrane prevents the immediate neutralization reaction of the two electrolytes. Due to this effect, the zinc-lead battery of the present invention has a high voltage 2.
8V, and the reaction of the above formula was carried out stably, so it became clear that charging and discharging was possible.

(Example 2) Pressure-molded manganese dioxide electrodes (reaction area 4, Oc!) were used as the 12 positive electrodes shown in FIG.
A zinc plate (reaction area 10.0 crj> e) was injected, and a 30% by weight potassium hydroxide aqueous solution was injected into the negative electrode electrolyte chamber 15.An example in which a zinc-mancan dioxide battery was constructed using the same members as in Example 1. I will explain about it.

The reaction formula at the manganese dioxide electrode is as follows.

■ MnO2+4H++2e-E Mn”2H20
... (4:) The potential of this electrode with respect to the standard hydrogen electrode is +1.23V.

On the other hand, the reaction formula at the zinc electrode is as follows.

θ Zn+20H-d Zn(OH)2+2e
-(5) The potential of this electrode relative to the standard hydrogen electrode is 1
．． It is 245V. In the above two equations, the reaction from left to right is a discharge reaction, and the reaction from right to left is a charge reaction.

The theoretical battery voltage of a battery constructed with these two electrodes is 2
．． It is 475V.

When we measured the open circuit voltage of this battery at room temperature, we found that
It stably showed 2.40V. Also, in Figure 3, the upper limit voltage 3
．． 2V, a lower limit voltage of 1.6V, and a charge/discharge cycle test using a constant current of 10 mA. As shown in FIG. 3, a flat potential of 2.0 to 1.9 V was exhibited during discharging, and a flat potential of 2.7 to 2.9 V was exhibited during charging. In addition, the capacity gradually decreased with each repetition of charging and discharging, but in Example 2, 10 cycles of charging and discharging were possible.

(Example 3) A paste-type lead dioxide electrode (reaction area: 4.0 cnf) was used as the positive electrode No. 12 shown in FIG. An electrode (reaction area: 4.0 cd) molded with the addition of was used. A 35% by weight sulfuric acid aqueous solution and a 30% by weight potassium hydroxide aqueous solution were respectively injected into the electrolyte chambers 14 and 15.

An example in which a hydrogen-lead battery is constructed using the same members as in Example 1 in other respects will be described.

The reaction formula for the type of carbon dioxide ship is as follows.

'FB PbO2"SO42-"2e-"4H";
! PbSO4”2H20・・・・・・(6) The potential of this electrode with respect to the standard hydrogen electrode is +1.685V
It is.

On the other hand, the reaction formula for the hydrogen storage alloy electrode is as follows.

e MHx+1+OH-:” MHx+H20+
e-,,---・(7) The potential of this electrode with respect to the standard hydrogen electrode is -0,8285V. In the above two equations, the reaction from left to right is a discharge reaction, and the reaction from right to left is a charge reaction. The theoretical battery voltage of the battery configured with these two electrodes is 2.51V.

When we measured the open circuit voltage of this battery at room temperature, we found that
It stably showed 2.45V. Also, in Fig. 4, the upper limit voltage 3
．． Ov, lower limit voltage 2. The results of a charge/discharge cycle test conducted at a constant current of 20 mA at Ov are shown. As shown in Figure 4, the discharge shows a flat potential of 2.3 to 2.2V,
During charging, a flat potential of 2.7 to 2.8V was exhibited. In addition, the capacity gradually decreased with repeated charging and discharging.
In Example 3, 13 cycles of charging and discharging were possible.

(Example 4) Paste type lead dioxide electrodes (reaction area 4.0cd) were used as the 12 positive electrodes shown in Figure 1, and paste type cadmium electrodes (reaction area 4, Oc/) were used as the 13 negative electrodes. there was. Further, a cadmium-lead battery was constructed in the same manner as in Example 1 except that a 35% by weight sulfuric acid aqueous solution and a 30% by weight potassium hydroxide aqueous solution were injected into the electrolyte chambers 14 and 15, respectively.

Here, the reaction formula for the carbon dioxide funabashi is as follows.

pbo2+5o42 +2e-+4H”:
PbSO4+2H20...(8) The potential of this electrode with respect to the standard hydrogen electrode is ±1.685V
It is.

On the other hand, the reaction formula at the cadmium electrode is as follows.

e Cd+20Hd Cd(OH)2”2e---(
9) The potential of this electrode relative to the standard hydrogen electrode is -0.82
It is 5V. In the above two equations, the reaction from left to right is a discharge reaction, and the reaction from right to left is a charge reaction.

The theoretical battery voltage of a battery constructed with these two electrodes is 2
．． It is 51V.

When we measured the open circuit voltage of this battery at room temperature, we found that
It showed a stable voltage of 2.45V. Moreover, in FIG. 5, upper limit voltage 3. OV, lower limit voltage 2. The results of a charge/discharge cycle test conducted at OV and a constant current of 20 mA are shown. As shown in FIG. 5, a flat potential of 2.3 to 2.2 V was exhibited during discharging, and a flat potential of 2.7 to 2.8 V was exhibited during charging. In addition, the capacity gradually decreased with each repetition of charging and discharging, but in Example 4, charging and discharging up to 95 cycles was possible.

In Examples 2 to 4 above, water decomposition reactions also occurred on the ion exchange membrane. Therefore, it is possible to expect a large potential difference between the positive and negative electrodes similar to that in Example 1, so that the electromotive force of conventional manganese dry batteries, silver oxide batteries, mercury batteries, etc. can be reduced to 1
．． The electromotive voltage of 3-1.7v primary batteries, nickel-cadmium batteries, nickel-zinc batteries, lead-acid batteries, etc. is 1.2-2.
2, which could not be obtained with aqueous batteries such as OV secondary batteries.
, it became possible to extract a high voltage of 4 to 2.5V.

(Example 5) The battery configuration of the present invention was
ow) An example of application to batteries will be shown.

FIG. 6 shows a glass test cell used in a redox flow battery according to an example of the present invention. In the figure, 21 indicates a bipolar ion exchange membrane. In the present invention, a membrane made of a copolymer of tetrafluoroethylene and perfluorovinylether and a membrane made of a copolymer of styrene and vinylbenzene were used as the bipolar ion exchange membrane. 22 is the positive electrode, 2
3 indicates a negative electrode, and a carbon porous electrode was used in each case. An acidic electrolyte containing metal ions (F e'') IM/i! in an oxidized state is transferred from one tank 26, and an alkaline electrolyte containing metal ions (Cr (CN6)'-) IM/C in a reduced state is transferred from another tank 26. The tank 27 was sent to the positive electrode chamber 24 and negative electrode chamber 25 of each battery to discharge.
B: The electrolyte was supplied from a 2 g tank in the reverse manner. Sulfuric acid (LM/i aqueous solution was used as the acidic electrolyte, and potassium hydroxide (2M/f!) was used as the alkaline electrolyte.
) an aqueous solution was used.

The reaction at the positive electrode is as shown in the following equation.

■ Fe”10e: Fe2+
-G ■ The potential of this positive electrode with respect to the standard hydrogen electrode is +0.771V.

On the other hand, the reaction formula at the negative electrode is as follows.

e [Cr(CN)s]'--! [Cr(
CN)s] 3-+ e (11) The potential of this negative electrode with respect to the standard hydrogen electrode is -1.28V. In the above two equations, a reaction from left to right is a discharge reaction, and a reaction from right to left is a charge reaction.

The theoretical battery voltage of a battery constructed with these two electrodes is 2
．． 05V.

When we measured the open circuit voltage of this battery at room temperature, we found that
It showed a stable voltage of 1,90V. Also, in Figure 7, 10
The results of a charge/discharge test conducted at a constant current of mA/cnf are shown. As shown in FIG. 7, a flat potential of 1.76 V was exhibited during discharge, and a flat potential of 2.21 V was exhibited during charging. Further, the capacity gradually decreased with each repetition of charging and discharging, but in this example, charging and discharging for 20 cycles or more were possible.

The conventional redox flow battery using iron chloride and chromium chloride, which was examined for comparison, mainly uses sulfuric acid or hydrochloric acid as the electrolyte.

The reaction at the positive electrode of this battery is as shown in the following equation.

Fe"+e: Fe"-(12) The potential of this electrode with respect to the standard hydrogen electrode is +0.7'71V.

On the other hand, the reaction formula at the negative electrode is as follows.

+9 Cr" -=! Cr"+e
-(13) The potential of this electrode relative to a standard hydrogen electrode is -0,408V. In the above two equations, the reaction from left to right is a discharge reaction, and the reaction from right to left is a charge reaction.

The theoretical battery voltage of a battery constructed with these two electrodes is 1
．． It is 179V.

According to the structure of the present invention, the electrolyte of the negative electrode is changed from an acidic electrolyte to an alkaline potassium hydroxide as in this example, and by using the reaction of chromium cyanide, a redox flow using only a conventional acidic electrolyte can be achieved. than batteries,
It has become possible to construct a redox flow battery with considerably high voltage.

(Example 6) An example in which the battery configuration of the present invention is applied to a zinc-chloride battery will be described.

FIG. 8 shows a glass test cell used in the zinc-chloride battery of this example. 31 indicates a cation exchange membrane. In the present invention, a membrane made of a copolymer of styrene and vinylbenzene was used as the bipolar ion exchange membrane. 32 indicates a positive electrode, which is a porous titanium plate using ruthenium oxide as a catalyst. 33 indicates a negative electrode, and a high-density porous carbon electrode was used. An acidic electrolyte consisting of an aqueous zinc chloride solution or hydrochloric acid with a pH of 1 to 3 is added from one tank 38 to 30% by weight of K containing zincate ions (Zn(OH)4'').
An alkaline electrolyte consisting of an OH aqueous solution is stored in another tank 39.
From there, it was circulated to the positive electrode electrolyte chamber 36 and negative electrode electrolyte chamber 37 of each battery. Chlorine gas is drawn out from the gas tank 34 to the waste inlet port 35 through the gas passage, and then passed through the porous electrode 3.
The excess chlorine gas was returned to the gas tank 34. During charging, chlorine gas generated by decomposition of the acidic electrolyte was collected into the same gas tank 34.

The reaction at the positive electrode is as shown in the following equation.

e C(1:+2e-;=! 2Ce -...
-(14) The potential of this electrode relative to the standard hydrogen electrode is +
It is 1.40V.

On the other hand, the reaction formula at the negative electrode is as follows.

e Zn+20H: Zn(OH)2”2e
--- (15) The nominal potential of this electrode with respect to a standard hydrogen electrode is -1.25V. In the above two equations, the reaction from left to right is a discharge reaction, and the reaction from right to left is a charge reaction.

The theoretical battery voltage of a battery constructed with these two electrodes is 2
．． It is 65V.

When we measured the open circuit voltage of this battery at room temperature, we found that
It showed a stable voltage of 2.60 V. Also, in Figure 9, 10
The results of a charge/discharge test performed at a constant current of mA/cd are shown. As shown in Figure 9, the discharge is approximately 2.30V.
It showed a flat potential of about 2.90 V during charging. Further, the capacity gradually decreased with each repetition of charging and discharging, but in this example, charging and discharging for 10 or more cycles was possible.

As a comparative example, a conventional zinc chloride battery uses a zinc chloride aqueous solution as the negative electrode electrolyte. Therefore, the reaction formula at the negative electrode is as follows.

e7. n: Zn"+2e-...-
(16) The potential of this electrode relative to the standard hydrogen electrode is -0,
It is 763■. In the above equation, a reaction from left to right is a discharge reaction, and a reaction from right to left is a charge reaction.

On the other hand, since the reaction of the positive electrode is the same as in the case of the present invention, the theoretical battery voltage of the battery configured with these two electrodes is 2.
It becomes 16V.

According to the structure of the present invention, by changing the electrolyte of the negative electrode from acidic to alkaline potassium hydroxide as in this example and using the reaction of zincate ions, the zinc chloride electrolyte using only the conventional zinc chloride electrolyte alone can be used. It became possible to construct a battery with considerably higher voltage than a battery.

(Example 7) An example in which the battery configuration of the present invention is applied to a zinc bromine battery will be described.

The test cell was adapted from the cell shown in Figure 8, and the positive electrode electrolyte was mixed with an acidic aqueous solution containing mainly zinc chloride to zinc bromide (pH 1).
~3), the reaction gas chlorine gas was replaced with bromine gas. Further, as the bipolar ion exchange membrane, a membrane made of a copolymer of tetrafluoroethylene and perfluorovinyl ether was used.

The reaction at the positive electrode is as shown in the following equation.

Br2+2e-: 2Br-- (17) The potential of this electrode with respect to the standard hydrogen electrode is ±1.06V.

On the other hand, the reaction formula at the negative electrode is as follows.

○ Zn+20H-: Zn(OH)2"2e-=-・
= (18) The potential of this negative electrode with respect to the standard hydrogen electrode is -
The voltage is 1.25V. In the above two equations, the reaction from left to right is the main reaction, and the reaction from right to left is the charging reaction.

The theoretical battery voltage of a battery constructed with these two electrodes is 2
．． It is 31V.

When we measured the open circuit voltage of this battery at room temperature, we found that
It showed a stable voltage of 2.25V. Also, in Figure 10, 10
The results of a charge/discharge test conducted at a constant current of mA and 'cd are shown. As shown in FIG. 10, the discharge is about 2. O
It showed a flat potential of OV, and a flat potential of about 2.60 V during charging. In addition, the capacity gradually decreased with each repetition of charging and discharging, but in Example 7, charging and discharging for 10 cycles or more was possible.

As a comparative example, a conventional zinc bromine battery uses a zinc bromide aqueous solution as the negative electrode electrolyte. Therefore, the reaction formula at the negative electrode is as follows.

02n ;=! Zn”+2 e ---(19) The potential of this electrode with respect to the standard hydrogen electrode is -0,763V.The reaction from left to right in the above equation is the discharge reaction, and the reaction from right to left is This is a charging reaction.

Since the reaction of the positive electrode is the same as in the case of the present invention, the theoretical battery voltage of the battery configured with these two electrodes is 1.83V.
becomes.

According to the structure of the present invention, by changing the negative electrode electrolyte from acidic to alkaline potassium hydroxide as in this example and using the reaction of zincate ions, a zinc bromine battery using a conventional zinc chloride electrolyte alone can be created. It has now become possible to construct batteries with significantly higher voltages.

(Example 8) An example in which the cell configuration of the present invention is applied to an oxygen-hydrogen fuel cell will be described.

FIG. 11 shows an acrylic test cell used in the fuel cell of this example. In the figure, 41 indicates a bipolar ion exchange membrane, and in the present invention, a membrane made of a copolymer of styrene and vinylhenzene was used. 42 is a positive electrode, 43 is a negative electrode,
In both cases, a carbon porous electrode plate supporting a platinum catalyst was used. Air is supplied from the air inlet 46, and hydrogen is supplied from the fuel chamber inlet 47.
were introduced into the electrodes. A 20 wt.
% by weight aqueous potassium hydroxide solution was injected.

The reaction at the positive electrode is as shown in the following equation.

e O2+4H"+4e-→2H20-(20) The potential of this electrode with respect to the standard hydrogen electrode is +1.229V.

On the other hand, the reaction formula at the negative electrode is as follows.

8th+20H・→2H20+2e
--(21) The potential of this electrode with respect to the standard hydrogen electrode is 0.8285V. The theoretical battery voltage of a battery configured with these two electrodes is 2.0575V.

In the case of a fuel cell using a conventional alkaline electrolyte,
The reaction at the positive electrode is as shown in the following equation.

■ 02+2H20+4e−−+ 40H−−−(
22) The potential of this electrode relative to the standard hydrogen electrode is +0.4
It is 01V. However, this reaction does not proceed in one step; 02+H20+2e--) o211-+all
＋・＋＋＋＋ (23
), if there is a catalyst that quickly decomposes the hydrogen peroxide ions generated, then 02H-→OH+1/202...
...The reaction of (24) progresses and can be summarized as shown in the above equation. The theoretical battery voltage of this battery is 1.229V,
In reality, the open circuit voltage is about 1.1 V or less because the above-mentioned process is performed.

FIG. 12 shows the current-voltage characteristics of the fuel cell of the present invention and a conventional fuel cell using an alkaline electrolyte when tested at 60°C.

In the characteristics of the fuel cell of the present invention (curve A), the open circuit voltage was 1.85V, and the cell voltage at a current density of 2 (10) mA/C- was 1.50V.

On the other hand, in the characteristics of a conventional fuel cell (curve B), the open circuit voltage shows 1.05 V and the current density 2 (10) m
The battery voltage in A/c♂ showed 0.75V.

As described above, by adopting the battery configuration of the present invention,
It has become clear that higher voltage can be obtained than in conventional fuel cells using only an alkaline electrolyte. Further, no deterioration due to contamination of the positive electrode electrolyte due to carbon dioxide gas in the air was observed.

It goes without saying that the effects of adopting the battery configuration of the present invention are not limited to the combination of positive and negative electrodes as described in the examples, and that various combinations are possible.

In addition, in the examples, as an example of bipolar ion exchange membrane,
We used a membrane made of a copolymer of tetrafluoroethylene and perfluorovinyl ether, a membrane made of a copolymer of styrene and vinylhenzene, or a membrane made of both, and these showed almost the same results in terms of battery characteristics. , the results for one or the other are listed.

Furthermore, although this example describes a secondary battery, a redox flow battery, a zinc chloride battery, a zinc bromine battery, and a fuel cell, it is also effective for a primary battery that uses two different types of electrolytes, acid and alkaline. The gains are clear.

Effects of the Invention As described above, the present invention is characterized in that an acidic electrolyte and an alkaline electrolyte are used as the electrolytes of the positive and negative electrodes, respectively, and a bipolar ion exchange membrane is used as the diaphragm. As a result, the electrode reaction in the acidic electrolyte and the electrode reaction in the alkaline electrolyte can be achieved independently, and a large electrode potential difference can be expected. It is possible to provide a high-performance battery with higher electromotive force than other batteries.

[Brief explanation of drawings]

Fig. 1 is a schematic diagram of the configuration of batteries according to Examples 1 to 4 of the present invention, Fig. 2 is a charge-discharge characteristic diagram of the battery according to Example 1 of the present invention, and Fig. 3 is a diagram of the battery according to Example 2 of the present invention. Charging and discharging characteristic diagram, FIG. 4 is a charging and discharging characteristic diagram of the battery of Example 3 of the present invention, FIG. 5 is a charging and discharging characteristic diagram of the battery of Example 4 of the present invention, and FIG. 6 is a diagram of the charging and discharging characteristic of the battery of Example 4 of the present invention. 7 is a diagram showing the charging and discharging characteristics of the battery according to Example 5 of the present invention. FIG. 8 is a schematic diagram of the configuration of the battery according to Examples 6 and 7 of the present invention. FIG. 10 is a charge-discharge characteristic diagram of the battery of Example 6 of the present invention, FIG. 11 is a schematic diagram of the structure of the battery of Example 8 of the present invention, and FIG. FIG. 6 is a current-voltage characteristic diagram of a battery according to Example 8 of the invention. 11.21.31.41...Bipolar ion exchange membrane, 12.22,32.42...Positive electrode, 1
3゜23.33.43...Negative electrode, 16...
...Stirrer, 24...Positive electrode chamber, 25...
・Negative electrode chamber, 26.28.38...Positive electrode tank,
27,29.39・・・Negative electrode tank, 14,36
．． 44... Positive electrode electrolyte chamber, 15°37.45.
...Negative electrode electrolyte chamber, 34 ... Gas tank, 35 ... Gas inlet, 46 ... Air chamber inlet, 47 ... Fuel Room entrance. Name of agent: Patent attorney Shigetaka Awano and 1 other name wShakusemi-2-v V 1) Ko-yen-v-day? Hoto C Power-Jakukenkuni Mi-Snoring--9

Claims (17)

[Claims] (1) A two-component system characterized by comprising a positive electrode and a negative electrode, an acidic electrolyte as the positive electrode electrolyte, an alkaline electrolyte as the negative electrode electrolyte, and a bipolar ion exchange membrane used as a diaphragm for the electrolyte. battery. (2) A patent characterized in that at least one of a membrane made of a copolymer of tetrafluoroethylene and perfluorovinylether or a membrane made of a copolymer of styrene and vinylbenzene is used as the bipolar ion exchange membrane. A two-component battery according to claim 1. (3) The two-component battery according to claim 1, characterized in that lead dioxide is used as the positive electrode and zinc is used as the negative electrode. (4) The two-component battery according to claim 1, characterized in that manganese dioxide is used as the positive electrode and zinc is used as the negative electrode. (5) Claim 1 characterized in that lead dioxide is used as the positive electrode and a hydrogen storage alloy is used as the negative electrode.
2-component battery as described in section. (6) The two-component battery according to claim 1, characterized in that lead dioxide is used as the positive electrode and cadmium is used as the negative electrode. (7) A two-component system characterized by using a positive electrode and a negative electrode, an acidic electrolyte as the positive electrode electrolyte, an alkaline electrolyte as the negative electrode electrolyte, a bipolar ion exchange membrane as the diaphragm, and a redox reaction. battery. (8) The two-component battery according to claim 7, characterized in that porous carbon electrodes are used as the positive electrode and the negative electrode. (9) A patent characterized in that at least one of a membrane made of a copolymer of tetrafluoroethylene and perfluorovinylether or a membrane made of a copolymer of styrene and vinylbenzene is used as the bipolar ion exchange membrane. A two-component battery according to claim 7. (10) A two-component battery according to claim 7, characterized in that iron is used as the active material of the positive electrode, and chromium cyanide is used as the active material of the negative electrode. (11) A positive electrode and a negative electrode, a positive electrode active material made of chlorine, a negative electrode active material made of zinc, an acidic electrolyte as a positive electrode electrolyte, an alkaline electrolyte as a negative electrode electrolyte, and a bipolar ion as a diaphragm. A two-component battery characterized by using an exchange membrane. (12) A patent characterized in that at least one of a membrane made of a copolymer of tetrafluoroethylene and perfluorovinylether or a membrane made of a copolymer of styrene and vinylbenzene is used as the bipolar ion exchange membrane. A two-component battery according to claim 11. (13) Claim 11, wherein the positive electrode is a porous body of corrosion-resistant metal equipped with a catalyst, and the negative electrode is a porous carbon electrode.
2-component battery as described in section. (14) A positive electrode and a negative electrode, a positive electrode active material made of bromine, a negative electrode active material made of zinc, an acidic electrolyte as a positive electrode electrolyte, an alkaline electrolyte as a negative electrode electrolyte, and a bipolar lion as a diaphragm. A two-component battery characterized by using an exchange membrane. (15) A patent claim characterized in that the ion exchange membrane is a membrane made of a copolymer of tetrafluoroethylene and perfluorovinylether, or a membrane made of at least one of a copolymer of styrene and vinylbenzene. The two-component battery according to item 14. (16) a positive electrode, a negative electrode, and a positive electrode active material made of oxygen;
A two-component battery comprising a negative electrode active material made of hydrogen, an acidic electrolyte as a positive electrode electrolyte, an alkaline electrolyte as a negative electrode electrolyte, and a bipolar ion exchange membrane as a diaphragm. (17) A patent claim characterized in that at least one of a membrane made of a copolymer of tetrafluoroethylene and perfluorovinylether or a membrane made of a copolymer of styrene and vinylbenzene is used as the ion exchange membrane. The two-component battery according to item 16.