JP2806233B2 - Electrolytic manganese dioxide and method for producing the same - Google Patents
Electrolytic manganese dioxide and method for producing the sameInfo
- Publication number
- JP2806233B2 JP2806233B2 JP5302655A JP30265593A JP2806233B2 JP 2806233 B2 JP2806233 B2 JP 2806233B2 JP 5302655 A JP5302655 A JP 5302655A JP 30265593 A JP30265593 A JP 30265593A JP 2806233 B2 JP2806233 B2 JP 2806233B2
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- Japan
- Prior art keywords
- manganese dioxide
- electrolytic manganese
- electrolytic
- surface potential
- battery
- Prior art date
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Classifications
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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
- Y02E60/10—Energy storage using batteries
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- Inorganic Compounds Of Heavy Metals (AREA)
- Battery Electrode And Active Subsutance (AREA)
Description
【０００１】[0001]
【産業上の利用分野】本発明は、マンガン乾電池または
アルカリマンガン乾電池の正極活物質として使用される
電解二酸化マンガン及びその製造方法に関する。BACKGROUND OF THE INVENTION 1. Field of the Invention The present invention relates to an electrolytic manganese dioxide used as a positive electrode active material of a manganese dry battery or an alkaline manganese dry battery and a method for producing the same.
【０００２】[0002]
【従来の技術】近年、乾電池の水銀ゼロ使用に伴う電池
内部抵抗の増加のため、各電池構成材料に品質改善に求
められている。2. Description of the Related Art In recent years, in order to increase the internal resistance of batteries due to the use of zero mercury in dry batteries, there is a demand for improving the quality of each battery constituent material.
【０００３】特に、正極合剤として使用されている二酸
化マンガン、又は、導電性カーボン（アセチレンブラッ
ク、または、グラファイト）の品質改善が強く要望され
ている。In particular, there is a strong demand for improving the quality of manganese dioxide or conductive carbon (acetylene black or graphite) used as a positive electrode mixture.
【０００４】導電剤として使用されているアセチレンブ
ラックは正極合剤の抵抗低減のため、従来よりもさらに
微粉化（約４０００オングストローム→約４００オング
ストローム）したものが使用されるようになった。Acetylene black, which is used as a conductive agent, has been used in the form of finer powder (about 4,000 angstroms → about 400 angstroms) in order to reduce the resistance of the positive electrode mixture.
【０００５】しかしながら、これに伴い、電池の保存性
能の低下（放電性能低下、液漏れ）が問題になってき
た。[0005] However, the storage performance of the battery (reduction in discharge performance, liquid leakage) has become a problem.
【０００６】[0006]
【発明が解決しようとする課題】本発明の目的は、マン
ガン乾電池、または、アルカリマンガン乾電池の保存性
能を改善する、例えば、放電性能低下及び液漏れを改善
する電解二酸化マンガン及びその製造方法を提供するこ
とにある。SUMMARY OF THE INVENTION It is an object of the present invention to provide an electrolytic manganese dioxide for improving the storage performance of a manganese dry battery or an alkaline manganese dry battery, for example, for reducing the discharge performance and improving the liquid leakage, and a method for producing the same. Is to do.
【０００７】[0007]
【課題を解決するための手段】本発明者らは、電池の保
存性能の低下防止について鋭意検討した結果、電池の正
極に用いる電解二酸化マンガンの表面電位を１５０〜２
４０ｍＶ（ｖｓ．Ｈｇ／ＨｇＯ（４０ｗｔ％ＫＯＨ））
とすることにより、電池の保存性能が改善できることを
見出だし、本発明を完成するに至った。Means for Solving the Problems The inventors of the present invention have conducted intensive studies on preventing the storage performance of a battery from deteriorating, and as a result, have found that the surface potential of electrolytic manganese dioxide used for the positive electrode of the battery is 150 to 2 times.
40 mV (vs. Hg / HgO (40 wt% KOH))
As a result, it has been found that the storage performance of the battery can be improved, and the present invention has been completed.
【０００８】本発明について、以下にさらに詳細に説明
する。The present invention will be described in more detail below.
【０００９】[0009]
【作用】マンガン乾電池、または、アルカリマンガン乾
電池の保存劣化（放電性能低下、液漏れ）の原因は、正
極合剤中の電解二酸化マンガンと導電性カーボン（アセ
チレンブラック、または、グラファイト）が酸化還元反
応することによる。[Function] The cause of storage deterioration (decrease in discharge performance, liquid leakage) of manganese dry batteries or alkaline manganese dry batteries is due to the oxidation-reduction reaction between electrolytic manganese dioxide in the positive electrode mixture and conductive carbon (acetylene black or graphite). By doing.
【００１０】即ち、酸化還元反応により、電解二酸化マ
ンガンが還元され酸化度が低下して、放電性能が低下す
ると同時に、導電性カーボンが酸化されてＣＯ2ガスの
発生が起こり、このガス発生による電池の膨脹により液
漏れが起こる。That is, by the oxidation-reduction reaction, electrolytic manganese dioxide is reduced, the degree of oxidation is reduced, and the discharge performance is reduced. At the same time, the conductive carbon is oxidized to generate CO 2 gas, and the gas generated by the gas generation Leakage occurs due to the expansion of.
【００１１】この様な現象に着目し、ＣＯ2ガス発生量
と電解二酸化マンガンの表面電位との関係について検討
を行った結果、電解二酸化マンガンの表面電位が高いほ
どＣＯ2ガス発生量が多く、表面電位が低いほどＣＯ2ガ
ス発生量が少ないという相関性があり、電解二酸化マン
ガンの表面電位が２４０ｍＶ（ｖｓ．Ｈｇ／ＨｇＯ（４
０ｗｔ％ＫＯＨ））以下の場合、実質的に、ＣＯ2ガス
の発生量が無視しうることを見出だした。Focusing on such a phenomenon, the relationship between the amount of generated CO 2 gas and the surface potential of electrolytic manganese dioxide was examined. As a result, the higher the surface potential of electrolytic manganese dioxide, the larger the amount of CO 2 gas generated. There is a correlation that the lower the surface potential, the smaller the amount of CO 2 gas generated, and the surface potential of electrolytic manganese dioxide is 240 mV (vs. Hg / HgO (4
0 wt% KOH)), it was found that the amount of generated CO 2 gas was substantially negligible.
【００１２】一方、電解二酸化マンガンの表面電位は、
放電容量の尺度の一つである酸化度と関係があり、電位
が低すぎると放電性能も低下する傾向にある。実質的
に、放電性能を低下させない電解二酸化マンガンの表面
電位の下限は、１５０ｍＶ（ｖｓ．Ｈｇ／ＨｇＯ（４０
ｗｔ％ＫＯＨ））である。On the other hand, the surface potential of electrolytic manganese dioxide is
It is related to the degree of oxidation, which is one of the measures of the discharge capacity. If the potential is too low, the discharge performance tends to decrease. The lower limit of the surface potential of electrolytic manganese dioxide that does not substantially lower the discharge performance is 150 mV (vs. Hg / HgO (40
wt% KOH)).
【００１３】このような理由から、放電性能の低下を伴
わずに保存劣化を防止する電解二酸化マンガンの表面電
位の範囲は、１５０〜２４０ｍＶ（ｖｓ．Ｈｇ／ＨｇＯ
（４０ｗｔ％ＫＯＨ））の範囲であり、さらに１８０〜
２３０ｍＶ（ｖｓ．Ｈｇ／ＨｇＯ（４０ｗｔ％ＫＯ
Ｈ））の範囲が特に好ましい。For these reasons, the range of surface potential of electrolytic manganese dioxide for preventing storage deterioration without deterioration of discharge performance is 150 to 240 mV (vs. Hg / HgO).
(40 wt% KOH)), and more
230 mV (vs. Hg / HgO (40 wt% KO)
The range H)) is particularly preferred.
【００１４】ところが、通常の電解二酸化マンガンの表
面電位の範囲は、２４０〜２７０ｍＶ（ｖｓ．Ｈｇ／Ｈ
ｇＯ（４０ｗｔ％ＫＯＨ））であるため、表面電位を低
下させる必要がある。However, the surface potential of ordinary electrolytic manganese dioxide ranges from 240 to 270 mV (vs. Hg / H
gO (40 wt% KOH)), it is necessary to lower the surface potential.
【００１５】本発明者らは、この様な事情に鑑み、電解
二酸化マンガンの表面電位を低下させる方法についてさ
らに詳細に検討を行った結果、電解により電解二酸化マ
ンガンを得た後の工程で、マンガン塩水溶液、亜硫酸
水、ＯＨ基を有する有機化合物、ＣＨＯ基を有する有機
化合物、ＣＯＯＨ基を有する有機化合物のうち１種類、
または、複数の物質で湿式処理することにより、上記課
題を解決できることを見出だした。In view of such circumstances, the present inventors have studied in more detail a method for lowering the surface potential of electrolytic manganese dioxide. As a result, in the process after obtaining electrolytic manganese dioxide by electrolysis, One of a salt aqueous solution, a sulfite solution, an organic compound having an OH group, an organic compound having a CHO group, and an organic compound having a COOH group,
Alternatively, it has been found that the above problem can be solved by wet treatment with a plurality of substances.
【００１６】ＯＨ基を有する有機化合物としては、エチ
ルアルコールなどのアルコール類、ＣＨＯ基を有する有
機化合物としては、アセトアルデヒドなどのアルデヒド
類、ＣＯＯＨ基を有する有機化合物としてはシュウ酸な
どの有機酸類などがあげられ、また、多糖類のようにこ
れらの官能基を複数有しているものであっても良い。Organic compounds having an OH group include alcohols such as ethyl alcohol, organic compounds having a CHO group include aldehydes such as acetaldehyde, and organic compounds having a COOH group include organic acids such as oxalic acid. And those having a plurality of these functional groups, such as polysaccharides.
【００１７】これら以外の還元剤、例えばホウ化水素ナ
トリウムの様な強い還元剤を使用すると、表面電位のみ
ならず電解二酸化マンガンのバルクの酸化度も低下し
て、放電性能が劣化するため好ましくない。If a reducing agent other than these, for example, a strong reducing agent such as sodium borohydride is used, not only the surface potential but also the degree of oxidation of the electrolytic manganese dioxide bulk is reduced, and the discharge performance is deteriorated. .
【００１８】また、一般に、二酸化マンガンは加熱処理
により酸化度の低下を伴わずに電位が低下することが知
られているが、この場合、放電性能に重要な電解二酸化
マンガンの結晶水、吸着水が失われるため十分な放電特
性を示さない。It is generally known that manganese dioxide decreases its potential by heat treatment without lowering the degree of oxidation. In this case, water of crystallization and adsorption of electrolytic manganese dioxide, which is important for discharge performance, are known. , And does not exhibit sufficient discharge characteristics.
【００１９】同様な理由で、乾式処理（還元性ガスによ
る方法）でも十分な特性が得られていない。For the same reason, dry treatment (a method using a reducing gas) does not provide sufficient characteristics.
【００２０】更に、本発明者らは、別の電解二酸化マン
ガンの表面電位を低下させる方法として、電解二酸化マ
ンガンの電解製造工程において電解液の（マンガン／硫
酸）のモル比を１．５〜１００に調製すれば電解二酸化
マンガンの表面電位を低下させることが可能であること
を見出だした。Furthermore, the present inventors have proposed another method for lowering the surface potential of electrolytic manganese dioxide, in which the molar ratio of (manganese / sulfuric acid) in the electrolytic solution is 1.5 to 100 in the electrolytic production process of electrolytic manganese dioxide. It has been found that it is possible to lower the surface potential of electrolytic manganese dioxide if prepared.
【００２１】一般の電解二酸化マンガンの製造条件は、
次の表１のとうりである。The production conditions of general electrolytic manganese dioxide are as follows:
This is shown in Table 1 below.
【００２２】[0022]
【表１】 [Table 1]
【００２３】本発明者等は、この電解液の（マンガン／
硫酸）のモル比に注目し、電解液の（マンガン／硫酸）
モル比を高くする（１．５〜１００）ことにより、表面
電位の低い二酸化マンガンを製造できることを見出だし
た。（通常の電解二酸化マンガン製造における電解液の
（マンガン／硫酸）のモル比は、一般に０．５〜１．５
程度である。）この電解時における電流密度は５０〜１
００Ａ／ｍ 2の範囲が好ましく、電解温度は９０〜１０
０℃の範囲が好ましい。The inventors of the present invention have proposed that the electrolytic solution (manganese /
Paying attention to the molar ratio of (sulfuric acid), (manganese / sulfuric acid)
It has been found that by increasing the molar ratio (1.5 to 100), manganese dioxide having a low surface potential can be produced. (The molar ratio of (manganese / sulfuric acid) of the electrolytic solution in the usual electrolytic manganese dioxide production is generally 0.5 to 1.5.
It is about. ) The current density during this electrolysis is 50-1.
The electrolysis temperature is preferably 90 to 10 A / m 2.
A range of 0 ° C. is preferred.
【００２４】以下の実施例により本発明を具体的に示す
が、この実施例により本発明は何等限定されるものでは
ない。The present invention is specifically illustrated by the following examples, but the present invention is not limited by these examples.
【００２５】[0025]
実施例１ 常法の電解で得られた電解二酸化マンガンのブロック１
００ｋｇを２００リットルの水に浸漬し、ＭｎＯ2重量
に対しＭｎ重量が１ｗｔ％（１ｋｇ）になるように硫酸
マンガンを添加した。更に、９５℃、２４時間、加熱処
理を施した後、電解二酸化マンガンに常法の製品処理を
施して表面電位の低い（２２０ｍＶｖｓ．Ｈｇ／ＨｇＯ
（４０ｗｔ％ＫＯＨ））電解二酸化マンガンを得た。ま
た、この二酸化マンガンを正極活物質として図１に示す
マンガン乾電池を試作した。この乾電池を４５℃で１ケ
月間放置し、放置後の放電持続時間を測定した結果は、
表１に示すとおりであり、後で示す比較例の電解二酸化
マンガンよりも放電持続時間が１２％程度長くなった。Example 1 Block 1 of electrolytic manganese dioxide obtained by conventional electrolysis
00 kg was immersed in 200 liters of water, and manganese sulfate was added so that the Mn weight was 1 wt% (1 kg) with respect to the MnO 2 weight. Further, after subjecting to a heat treatment at 95 ° C. for 24 hours, electrolytic manganese dioxide is subjected to a usual product treatment to have a low surface potential (220 mV vs. Hg / HgO).
(40 wt% KOH)) Electrolytic manganese dioxide was obtained. Further, a manganese dry battery shown in FIG. 1 was experimentally manufactured using this manganese dioxide as a positive electrode active material. This battery was left at 45 ° C. for one month, and the result of measuring the discharge duration after leaving the battery was as follows.
As shown in Table 1, the discharge duration was about 12% longer than that of the electrolytic manganese dioxide of the comparative example described later.
【００２６】[0026]
【表２】 [Table 2]
【００２７】なお、正極活物質に用いた二酸化マンガン
とアセチレンブラックの配合重量比は６：１とし、電池
内の正極活物質の重量を一定とした。The mixing ratio of manganese dioxide and acetylene black used for the positive electrode active material was 6: 1, and the weight of the positive electrode active material in the battery was kept constant.
【００２８】実施例２ 常法の電解で得られた電解二酸化マンガンのブロックを
約２０μｍ迄粉砕し、１００ｋｇの粉状電解二酸化マン
ガンを得た。これに２００リットルの水を加えてスラリ
ーとし、更に、ＭｎＯ2重量に対しＭｎ重量が０．５ｗ
ｔ％（５００ｇ）になるように硫酸マンガンを添加し
た。更に、６０℃、１時間、加熱処理を施した後、電解
二酸化マンガンに常法の製品処理を施して表面電位の低
い（２００ｍＶ ｖｓ．Ｈｇ／ＨｇＯ（４０ｗｔ％ＫＯ
Ｈ））電解二酸化マンガンを得た。Example 2 A block of electrolytic manganese dioxide obtained by conventional electrolysis was ground to about 20 μm to obtain 100 kg of powdery electrolytic manganese dioxide. To this was added 200 liters of water to form a slurry, further, Mn weight relative to MnO 2 weight 0.5w
Manganese sulphate was added to give a t% (500 g). Further, after a heat treatment at 60 ° C. for 1 hour, electrolytic manganese dioxide is subjected to a usual product treatment to have a low surface potential (200 mV vs. Hg / HgO (40 wt% KO).
H)) Electrolytic manganese dioxide was obtained.
【００２９】また、実施例１と同様な方法により電池試
験を行った。A battery test was performed in the same manner as in Example 1.
【００３０】表２に示されている様に、後で示す比較例
の電解二酸化マンガンよりも放電持続時間が９％程度長
くなった。As shown in Table 2, the discharge duration was about 9% longer than the electrolytic manganese dioxide of the comparative example described later.
【００３１】実施例３ 常法の電解で得られた電解二酸化マンガンのブロックを
約２０μｍ迄粉砕し、１００ｋｇの粉状電解二酸化マン
ガンを得た。これに２００リットルの水を加えてスラリ
ーとし、更に、ＭｎＯ2重量に対しＳＯ2重量が０．５ｗ
ｔ％（５００ｇ）になるように亜硫酸水を添加した。更
に、６０℃、１時間、加熱処理を施した後、電解二酸化
マンガンに常法の製品処理を施して表面電位の低い（２
００ｍＶｖｓ．Ｈｇ／ＨｇＯ（４０ｗｔ％ＫＯＨ））電
解二酸化マンガンを得た。Example 3 A block of electrolytic manganese dioxide obtained by conventional electrolysis was ground to about 20 μm to obtain 100 kg of powdery electrolytic manganese dioxide. To this was added 200 liters of water to form a slurry, further, with respect to MnO 2 wt SO 2 weight 0.5w
Sulfuric acid aqueous solution was added so that t% (500 g) was obtained. Furthermore, after performing a heat treatment at 60 ° C. for one hour, electrolytic manganese dioxide is subjected to a normal product treatment to obtain a low surface potential (2
00mVvs. Hg / HgO (40 wt% KOH)) electrolytic manganese dioxide was obtained.
【００３２】また、実施例１と同様な方法により電池試
験を行った。A battery test was performed in the same manner as in Example 1.
【００３３】表２に示されている様に、後で示す比較例
の電解二酸化マンガンよりも放電持続時間が１０％程度
長くなった。As shown in Table 2, the discharge duration was about 10% longer than that of the electrolytic manganese dioxide of the comparative example described later.
【００３４】実施例４ 常法の電解で得られた電解二酸化マンガンのブロックを
約２０μｍ迄粉砕し、１００ｋｇの粉状電解二酸化マン
ガンを得た。これに２００リットルの水を加えてスラリ
ーとし、更に、ＭｎＯ2重量に対しエチルアルコール重
量が２．０ｗｔ％（２ｋｇ）になるようにエチルアルコ
ールを添加した。Example 4 A block of electrolytic manganese dioxide obtained by conventional electrolysis was ground to about 20 μm to obtain 100 kg of powdery electrolytic manganese dioxide. 200 liters of water was added thereto to form a slurry, and ethyl alcohol was further added so that the weight of ethyl alcohol was 2.0 wt% (2 kg) based on the weight of MnO 2 .
【００３５】更に、４０℃、１時間、加熱処理を施した
後、電解二酸化マンガンに常法の製品処理を施して表面
電位の低い（２００ｍＶ ｖｓ．Ｈｇ／ＨｇＯ（４０ｗ
ｔ％ＫＯＨ））電解二酸化マンガンを得た。Further, after subjecting to a heat treatment at 40 ° C. for one hour, electrolytic manganese dioxide is subjected to a usual product treatment to have a low surface potential (200 mV vs. Hg / HgO (40 watts).
t% KOH)) An electrolytic manganese dioxide was obtained.
【００３６】また、実施例１と同様な方法により電池試
験を行った。A battery test was performed in the same manner as in Example 1.
【００３７】表２に示されている様に、後で示す比較例
の電解二酸化マンガンよりも放電持続時間が８％程度長
くなった。As shown in Table 2, the discharge duration was about 8% longer than the electrolytic manganese dioxide of the comparative example described later.
【００３８】実施例５ 常法の電解で得られた電解二酸化マンガンのブロックを
約２０μｍ迄粉砕し、１００ｋｇの粉状電解二酸化マン
ガンを得た。これに２００リットルの水を加えてスラリ
ーとし、更に、ＭｎＯ2重量に対しアセトアルデヒド重
量が０．２ｗｔ％（２００ｇ）になるようにアセトアル
デヒドを添加した。Example 5 A block of electrolytic manganese dioxide obtained by conventional electrolysis was ground to about 20 μm to obtain 100 kg of powdery electrolytic manganese dioxide. 200 liters of water was added thereto to form a slurry, and acetaldehyde was further added so that the weight of acetaldehyde was 0.2 wt% (200 g) based on the weight of MnO 2 .
【００３９】更に、４０℃、１時間、加熱処理を施した
後、電解二酸化マンガンに常法の製品処理を施して表面
電位の低い（２００ｍＶ ｖｓ．Ｈｇ／ＨｇＯ（４０ｗ
ｔ％ＫＯＨ））電解二酸化マンガンを得た。Further, after subjecting to a heat treatment at 40 ° C. for 1 hour, electrolytic manganese dioxide is subjected to a usual product treatment to have a low surface potential (200 mV vs. Hg / HgO (40 W
t% KOH)) An electrolytic manganese dioxide was obtained.
【００４０】また、実施例１と同様な方法により電池試
験を行った。A battery test was performed in the same manner as in Example 1.
【００４１】表２に示されている様に、後で示す比較例
の電解二酸化マンガンよりも放電持続時間が１１％程度
長くなった。As shown in Table 2, the discharge duration was about 11% longer than the electrolytic manganese dioxide of the comparative example described later.
【００４２】実施例６ 常法の電解で得られた電解二酸化マンガンのブロックを
約２０μｍ迄粉砕し、１００ｋｇの粉状電解二酸化マン
ガンを得た。これに２００リットルの水を加えてスラリ
ーとし、更に、ＭｎＯ2重量に対しシュウ酸重量が０．
５ｗｔ％（５００ｇ）になるようにシュウ酸を添加し
た。Example 6 A block of electrolytic manganese dioxide obtained by conventional electrolysis was ground to about 20 μm to obtain 100 kg of powdery electrolytic manganese dioxide. 200 liters of water was added thereto to form a slurry, and the weight of oxalic acid was 0.1 to the weight of MnO 2 .
Oxalic acid was added so as to be 5 wt% (500 g).
【００４３】更に、４０℃、１時間、加熱処理を施した
後、電解二酸化マンガンに常法の製品処理を施して表面
電位の低い（２００ｍＶ ｖｓ．Ｈｇ／ＨｇＯ（４０ｗ
ｔ％ＫＯＨ））電解二酸化マンガンを得た。Further, after subjecting to a heat treatment at 40 ° C. for 1 hour, electrolytic manganese dioxide is subjected to a usual product treatment to have a low surface potential (200 mV vs. Hg / HgO (40 watts).
t% KOH)) An electrolytic manganese dioxide was obtained.
【００４４】また、実施例１と同様な方法により電池試
験を行った。A battery test was performed in the same manner as in Example 1.
【００４５】表２に示されている様に、後で示す比較例
の電解二酸化マンガンよりも放電持続時間が７％程度長
くなった。As shown in Table 2, the discharge duration was about 7% longer than the electrolytic manganese dioxide of the comparative example described later.
【００４６】比較例１ 常法の電解で得られた電解二酸化マンガンのブロック１
００ｋｇを２００リットルの水に浸漬し、常法の製品処
理を施して表面電位の高い（２５０ｍＶ ｖｓ．Ｈｇ／
ＨｇＯ（４０ｗｔ％ＫＯＨ））電解二酸化マンガンを得
た。Comparative Example 1 Block 1 of electrolytic manganese dioxide obtained by conventional electrolysis
00 kg is immersed in 200 liters of water, subjected to a usual product treatment, and has a high surface potential (250 mV vs. Hg /
HgO (40 wt% KOH)) electrolytic manganese dioxide was obtained.
【００４７】また、実施例１と同様な方法により電池試
験を行った。A battery test was performed in the same manner as in Example 1.
【００４８】実施例７ （Ｍｎ／硫酸）のモル比が５になるように、マンガン濃
度が１．０ｍｏｌ／リットル、硫酸濃度が０．２ｍｏｌ
／リットルである電解液を調製し、この電解液を加温可
能な内容積２０リットルの電解槽に張り込んだ。陽極に
チタン板、陰極にカーボン板を使用して、電流密度＝６
０Ａ／ｍ2、温度＝９５±１℃で電解を実施した。Example 7 The manganese concentration was 1.0 mol / liter and the sulfuric acid concentration was 0.2 mol so that the molar ratio of (Mn / sulfuric acid) was 5.
Per liter of an electrolytic solution was prepared, and this electrolytic solution was placed in a 20-liter electrolytic bath capable of heating. Using a titanium plate for the anode and a carbon plate for the cathode, current density = 6
Electrolysis was performed at 0 A / m 2 and at a temperature of 95 ± 1 ° C.
【００４９】１０日間電解した後、剥離し常法の後処理
を行い、得られた二酸化マンガンの表面電位を測定し
た。又、この二酸化マンガンを正極活物質として図１に
示すマンガン乾電池を試作した。この試作したマンガン
乾電池を４５℃で１ケ月間放置し、放置後の放電持続時
間を測定した。表面電位および放電持続時間の測定結果
を表３に示す。After electrolysis for 10 days, the resultant was peeled off and post-treated by a conventional method, and the surface potential of the obtained manganese dioxide was measured. Further, a manganese dry battery shown in FIG. 1 was experimentally manufactured using this manganese dioxide as a positive electrode active material. The prototype manganese dry battery was allowed to stand at 45 ° C. for one month, and the duration of discharge after the standing was measured. Table 3 shows the measurement results of the surface potential and the discharge duration.
【００５０】[0050]
【表３】 [Table 3]
【００５１】表３に示されている様に、後で示す比較例
の電解二酸化マンガンよりも放電持続時間が９％程度長
くなった。As shown in Table 3, the discharge duration was about 9% longer than the electrolytic manganese dioxide of the comparative example described later.
【００５２】実施例８ （Ｍｎ／硫酸）のモル比が２．５になるように、マンガ
ン濃度が０．５ｍｏｌ／リットル、硫酸濃度が０．２ｍ
ｏｌ／リットルである電解液を調製し、実施例１と同じ
電解条件で電解を実施した。Example 8 The manganese concentration was 0.5 mol / liter and the sulfuric acid concentration was 0.2 m so that the molar ratio of (Mn / sulfuric acid) was 2.5.
ol / liter of an electrolytic solution was prepared, and electrolysis was performed under the same electrolysis conditions as in Example 1.
【００５３】実施例１と同じ方法で表面電位及び放電持
続時間を測定し、その測定結果を表３に示す。The surface potential and the discharge duration were measured in the same manner as in Example 1, and the measurement results are shown in Table 3.
【００５４】表３に示されている様に、後で示す比較例
の電解二酸化マンガンよりも放電持続時間が１０％程度
長くなった。As shown in Table 3, the discharge duration was about 10% longer than that of the electrolytic manganese dioxide of the comparative example described later.
【００５５】比較例２ （Ｍｎ／硫酸）のモル比が１．０になるように、マンガ
ン濃度が０．５ｍｏｌ／リットル、硫酸濃度が０．５ｍ
ｏｌ／リットルである電解液を調製し、実施例１と同じ
電解条件で電解を実施した。Comparative Example 2 The manganese concentration was 0.5 mol / liter and the sulfuric acid concentration was 0.5 m so that the molar ratio of (Mn / sulfuric acid) was 1.0.
ol / liter of an electrolytic solution was prepared, and electrolysis was performed under the same electrolysis conditions as in Example 1.
【００５６】実施例１と同じ方法で表面電位及び放電持
続時間を測定し、その測定結果を表３に示す。The surface potential and the discharge duration were measured in the same manner as in Example 1, and the measurement results are shown in Table 3.
【００５７】[0057]
【発明の効果】本発明の電解二酸化マンガンをマンガン
乾電池の正極活物質に使用すると、表面電位が低い為、
正極合剤中の電解二酸化マンガンと導電性カーボンとの
間で酸化還元反応がおこらず、ガス発生がおこらない。
このことにより電池性能の保存性が良くなる、即ち放電
持続時間が長くなる。When the electrolytic manganese dioxide of the present invention is used as a positive electrode active material of a manganese dry battery, the surface potential is low.
No oxidation-reduction reaction occurs between the electrolytic manganese dioxide in the positive electrode mixture and the conductive carbon, and no gas is generated.
This improves the preservability of battery performance, that is, prolongs the discharge duration.
【図１】実施例１〜８及び比較例１〜２の電池性能評価
用乾電池の断面図FIG. 1 is a cross-sectional view of dry batteries for evaluating battery performance in Examples 1 to 8 and Comparative Examples 1 and 2.
１ 亜鉛缶（負極） ２ セパレーター ３ 底紙 ４ 正極 ５ 上紙 ６ 炭素棒 ７ 上蓋 ８ 封口剤 ９ 正極キャップ DESCRIPTION OF SYMBOLS 1 Zinc can (negative electrode) 2 Separator 3 Bottom paper 4 Positive electrode 5 Top paper 6 Carbon rod 7 Top lid 8 Sealing agent 9 Positive electrode cap
Claims (3)
ｇ／ＨｇＯ（４０ｗｔ％ＫＯＨ））である事を特徴とす
る電解二酸化マンガン。A surface potential of 150 to 240 mV (vs. H
g / HgO (40 wt% KOH)).
造する方法において、電解後の工程で、下記Ａ群に記載
の物質から選ばれる１つ、または複数の物質を用いて、
湿式法で表面電位を調整することを特徴とする請求項１
に記載の電解二酸化マンガンの製造方法。 Ａ群 マンガン塩水溶液、亜硫酸水、次の群の官能基（ＯＨ
基、ＣＨＯ基及びＣＯＯＨ基）の内少なくとも１つの官
能基を有する有機化合物2. The method for producing electrolytic manganese dioxide according to claim 1, wherein in the step after electrolysis, one or more substances selected from the following substances in Group A are used:
2. The method according to claim 1, wherein the surface potential is adjusted by a wet method.
3. The method for producing electrolytic manganese dioxide according to item 1. Group A Manganese salt aqueous solution, sulfite water, the following group of functional groups (OH
Organic compound having at least one functional group of the following groups:
造する方法において、電解液の（マンガン／硫酸）のモ
ル比が１．５〜１００の電解液を用いて電解製造するこ
とを特徴とする請求項１に記載の電解二酸化マンガンの
製造方法。3. The method for producing electrolytic manganese dioxide according to claim 1, wherein the electrolytic production is carried out using an electrolytic solution having a (manganese / sulfuric acid) molar ratio of 1.5 to 100. The method for producing electrolytic manganese dioxide according to claim 1.
Applications Claiming Priority (2)
| Application Number | Priority Date | Filing Date | Title |
|---|---|---|---|
| JP5-281133 | 1993-11-10 | ||
| JP28113393 | 1993-11-10 |
Publications (2)
| Publication Number | Publication Date |
|---|---|
| JPH07183032A JPH07183032A (en) | 1995-07-21 |
| JP2806233B2 true JP2806233B2 (en) | 1998-09-30 |
Family
ID=17634829
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| Application Number | Title | Priority Date | Filing Date |
|---|---|---|---|
| JP5302655A Expired - Fee Related JP2806233B2 (en) | 1993-11-10 | 1993-12-02 | Electrolytic manganese dioxide and method for producing the same |
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| Country | Link |
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Families Citing this family (4)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| JP3873760B2 (en) * | 2002-02-07 | 2007-01-24 | 松下電器産業株式会社 | Alkaline battery |
| AU2003213400A1 (en) * | 2002-10-11 | 2004-05-04 | Mitsui Mining And Smelting Co., Ltd. | Positive plate active material for cell, method for producing electrolytic manganese dioxide, and cell |
| JP5352173B2 (en) | 2008-10-01 | 2013-11-27 | パナソニック株式会社 | Alkaline battery |
| US7820326B2 (en) | 2008-10-17 | 2010-10-26 | Panasonic Corporation | Alkaline battery |
-
1993
- 1993-12-02 JP JP5302655A patent/JP2806233B2/en not_active Expired - Fee Related
Also Published As
| Publication number | Publication date |
|---|---|
| JPH07183032A (en) | 1995-07-21 |
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