Electrochemical properties of chloranilic acid and its application to the anode material of alkaline secondary batteries

Tetsuya Osaka, Toshiyuki Momma, Satoru Komoda, Nobuhiro Shiraishi, Susumu Kikuyama, Kohji Yuasa

Research output: Contribution to journalArticle

2 Citations (Scopus)

Abstract

For alkaline batteries, it is important to investigate prospective materials with higher energy density and lower cost. We paid attention to the reaction of quinone compounds and investigated the electrochemical properties of these compounds in alkaline solution and discussed the possibility for a negative active material of alkaline secondary batteries. In alkaline solution, most of these materials, e.g. p-benzoquinone, dissolved, while only chloranilic acid (C6Cl2(OH)2O2) did not. We have found that chloranilic acid is the most possible candidate for the negative active materials of alkaline batteries because of its insolubility to alkaline solutions. There were three couples of peaks in cyclic voltammogram (-1.2 to approximately -0.1 V vs. Ag/AgCl) for the electrode of chloranilic acid. With cathodic scan of cyclic voltammogram on -0.8 V vs. Ag/AgCl, the color of solution changed. It seems that this change is caused by the influence of dissolved products, which was formed by electrochemical redox reaction of chloranilic acid around -1.0 V vs. Ag/AgCl. When the charge-discharge test was conducted in the potential range between -0.45 V and -0.8 V, no colored substance was formed in the solution and the discharge capacity reached to approximate 150 mAh g-1 at the first cycle. From these results, on chloranilic acid, it was suggested that there was a possibility of application for a negative active material of alkaline secondary batteries.

Original languageEnglish
Pages (from-to)238-242
Number of pages5
JournalElectrochemistry
Volume67
Issue number3
Publication statusPublished - 1999

Fingerprint

Secondary batteries
Electrochemical properties
Anodes
Acids
Redox reactions
Discharge (fluid mechanics)
Solubility
chloranilic acid
Color
Electrodes
Costs

ASJC Scopus subject areas

  • Electrochemistry

Cite this

Electrochemical properties of chloranilic acid and its application to the anode material of alkaline secondary batteries. / Osaka, Tetsuya; Momma, Toshiyuki; Komoda, Satoru; Shiraishi, Nobuhiro; Kikuyama, Susumu; Yuasa, Kohji.

In: Electrochemistry, Vol. 67, No. 3, 1999, p. 238-242.

Research output: Contribution to journalArticle

Osaka, Tetsuya ; Momma, Toshiyuki ; Komoda, Satoru ; Shiraishi, Nobuhiro ; Kikuyama, Susumu ; Yuasa, Kohji. / Electrochemical properties of chloranilic acid and its application to the anode material of alkaline secondary batteries. In: Electrochemistry. 1999 ; Vol. 67, No. 3. pp. 238-242.
@article{facb2763657846f788a8841d11b38087,
title = "Electrochemical properties of chloranilic acid and its application to the anode material of alkaline secondary batteries",
abstract = "For alkaline batteries, it is important to investigate prospective materials with higher energy density and lower cost. We paid attention to the reaction of quinone compounds and investigated the electrochemical properties of these compounds in alkaline solution and discussed the possibility for a negative active material of alkaline secondary batteries. In alkaline solution, most of these materials, e.g. p-benzoquinone, dissolved, while only chloranilic acid (C6Cl2(OH)2O2) did not. We have found that chloranilic acid is the most possible candidate for the negative active materials of alkaline batteries because of its insolubility to alkaline solutions. There were three couples of peaks in cyclic voltammogram (-1.2 to approximately -0.1 V vs. Ag/AgCl) for the electrode of chloranilic acid. With cathodic scan of cyclic voltammogram on -0.8 V vs. Ag/AgCl, the color of solution changed. It seems that this change is caused by the influence of dissolved products, which was formed by electrochemical redox reaction of chloranilic acid around -1.0 V vs. Ag/AgCl. When the charge-discharge test was conducted in the potential range between -0.45 V and -0.8 V, no colored substance was formed in the solution and the discharge capacity reached to approximate 150 mAh g-1 at the first cycle. From these results, on chloranilic acid, it was suggested that there was a possibility of application for a negative active material of alkaline secondary batteries.",
author = "Tetsuya Osaka and Toshiyuki Momma and Satoru Komoda and Nobuhiro Shiraishi and Susumu Kikuyama and Kohji Yuasa",
year = "1999",
language = "English",
volume = "67",
pages = "238--242",
journal = "Electrochemistry",
issn = "1344-3542",
publisher = "Electrochemical Society of Japan",
number = "3",

}

TY - JOUR

T1 - Electrochemical properties of chloranilic acid and its application to the anode material of alkaline secondary batteries

AU - Osaka, Tetsuya

AU - Momma, Toshiyuki

AU - Komoda, Satoru

AU - Shiraishi, Nobuhiro

AU - Kikuyama, Susumu

AU - Yuasa, Kohji

PY - 1999

Y1 - 1999

N2 - For alkaline batteries, it is important to investigate prospective materials with higher energy density and lower cost. We paid attention to the reaction of quinone compounds and investigated the electrochemical properties of these compounds in alkaline solution and discussed the possibility for a negative active material of alkaline secondary batteries. In alkaline solution, most of these materials, e.g. p-benzoquinone, dissolved, while only chloranilic acid (C6Cl2(OH)2O2) did not. We have found that chloranilic acid is the most possible candidate for the negative active materials of alkaline batteries because of its insolubility to alkaline solutions. There were three couples of peaks in cyclic voltammogram (-1.2 to approximately -0.1 V vs. Ag/AgCl) for the electrode of chloranilic acid. With cathodic scan of cyclic voltammogram on -0.8 V vs. Ag/AgCl, the color of solution changed. It seems that this change is caused by the influence of dissolved products, which was formed by electrochemical redox reaction of chloranilic acid around -1.0 V vs. Ag/AgCl. When the charge-discharge test was conducted in the potential range between -0.45 V and -0.8 V, no colored substance was formed in the solution and the discharge capacity reached to approximate 150 mAh g-1 at the first cycle. From these results, on chloranilic acid, it was suggested that there was a possibility of application for a negative active material of alkaline secondary batteries.

AB - For alkaline batteries, it is important to investigate prospective materials with higher energy density and lower cost. We paid attention to the reaction of quinone compounds and investigated the electrochemical properties of these compounds in alkaline solution and discussed the possibility for a negative active material of alkaline secondary batteries. In alkaline solution, most of these materials, e.g. p-benzoquinone, dissolved, while only chloranilic acid (C6Cl2(OH)2O2) did not. We have found that chloranilic acid is the most possible candidate for the negative active materials of alkaline batteries because of its insolubility to alkaline solutions. There were three couples of peaks in cyclic voltammogram (-1.2 to approximately -0.1 V vs. Ag/AgCl) for the electrode of chloranilic acid. With cathodic scan of cyclic voltammogram on -0.8 V vs. Ag/AgCl, the color of solution changed. It seems that this change is caused by the influence of dissolved products, which was formed by electrochemical redox reaction of chloranilic acid around -1.0 V vs. Ag/AgCl. When the charge-discharge test was conducted in the potential range between -0.45 V and -0.8 V, no colored substance was formed in the solution and the discharge capacity reached to approximate 150 mAh g-1 at the first cycle. From these results, on chloranilic acid, it was suggested that there was a possibility of application for a negative active material of alkaline secondary batteries.

UR - http://www.scopus.com/inward/record.url?scp=0033360004&partnerID=8YFLogxK

UR - http://www.scopus.com/inward/citedby.url?scp=0033360004&partnerID=8YFLogxK

M3 - Article

AN - SCOPUS:0033360004

VL - 67

SP - 238

EP - 242

JO - Electrochemistry

JF - Electrochemistry

SN - 1344-3542

IS - 3

ER -