Thermodynamic investigations of nitrogen electrode reaction in a LiCl-KCl-CsCl Melt

Katsutoshi Kobayashi, Hironori Nakajima, Takuya Goto, Yasuhiko Ito

Research output: Contribution to journalArticle

4 Citations (Scopus)

Abstract

Nitrogen electrode reaction has been investigated in a LiCl-KCl-CsCl melt containing Li3N. The following reaction, N3- → 1/2N2 + 3e-, is confirmed by quantitative analysis of anodically evolved gas. The Nernst relation holds for the rest potential of Ni electrodes at nitrogen gas pressure, pN2, of 0.1-1.0 atm and the anion fraction of N3- ion, xN3-, of 0.003-0.020 (anion fraction). Then the standard formal potential of N2/N3-, EN2/N3-0′, is evaluated to be 0.193 ± 0.003 V vs. Li+/Li (pN2 = 1 atm,xN3- = 1) at 673 K. The dependence of EN2/N3-0′ upon the temperature (605-721 K) gives a linear relation, whose slope is (-0.790 ± 0.096) × 10-3 V K-1. Thermodynamic quantities for formation of Li3N in the melt are also estimated.

Original languageEnglish
JournalJournal of the Electrochemical Society
Volume152
Issue number7
DOIs
Publication statusPublished - Aug 22 2005

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Anions
Nitrogen
Negative ions
Gases
Thermodynamics
anions
nitrogen
thermodynamics
Electrodes
electrodes
quantitative analysis
gas pressure
Ions
slopes
Chemical analysis
gases
ions
Temperature
temperature
cesium chloride

All Science Journal Classification (ASJC) codes

  • Electronic, Optical and Magnetic Materials
  • Renewable Energy, Sustainability and the Environment
  • Surfaces, Coatings and Films
  • Electrochemistry
  • Materials Chemistry

Cite this

Thermodynamic investigations of nitrogen electrode reaction in a LiCl-KCl-CsCl Melt. / Kobayashi, Katsutoshi; Nakajima, Hironori; Goto, Takuya; Ito, Yasuhiko.

In: Journal of the Electrochemical Society, Vol. 152, No. 7, 22.08.2005.

Research output: Contribution to journalArticle

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abstract = "Nitrogen electrode reaction has been investigated in a LiCl-KCl-CsCl melt containing Li3N. The following reaction, N3- → 1/2N2 + 3e-, is confirmed by quantitative analysis of anodically evolved gas. The Nernst relation holds for the rest potential of Ni electrodes at nitrogen gas pressure, pN2, of 0.1-1.0 atm and the anion fraction of N3- ion, xN3-, of 0.003-0.020 (anion fraction). Then the standard formal potential of N2/N3-, EN2/N3-0′, is evaluated to be 0.193 ± 0.003 V vs. Li+/Li (pN2 = 1 atm,xN3- = 1) at 673 K. The dependence of EN2/N3-0′ upon the temperature (605-721 K) gives a linear relation, whose slope is (-0.790 ± 0.096) × 10-3 V K-1. Thermodynamic quantities for formation of Li3N in the melt are also estimated.",
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AU - Kobayashi, Katsutoshi

AU - Nakajima, Hironori

AU - Goto, Takuya

AU - Ito, Yasuhiko

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N2 - Nitrogen electrode reaction has been investigated in a LiCl-KCl-CsCl melt containing Li3N. The following reaction, N3- → 1/2N2 + 3e-, is confirmed by quantitative analysis of anodically evolved gas. The Nernst relation holds for the rest potential of Ni electrodes at nitrogen gas pressure, pN2, of 0.1-1.0 atm and the anion fraction of N3- ion, xN3-, of 0.003-0.020 (anion fraction). Then the standard formal potential of N2/N3-, EN2/N3-0′, is evaluated to be 0.193 ± 0.003 V vs. Li+/Li (pN2 = 1 atm,xN3- = 1) at 673 K. The dependence of EN2/N3-0′ upon the temperature (605-721 K) gives a linear relation, whose slope is (-0.790 ± 0.096) × 10-3 V K-1. Thermodynamic quantities for formation of Li3N in the melt are also estimated.

AB - Nitrogen electrode reaction has been investigated in a LiCl-KCl-CsCl melt containing Li3N. The following reaction, N3- → 1/2N2 + 3e-, is confirmed by quantitative analysis of anodically evolved gas. The Nernst relation holds for the rest potential of Ni electrodes at nitrogen gas pressure, pN2, of 0.1-1.0 atm and the anion fraction of N3- ion, xN3-, of 0.003-0.020 (anion fraction). Then the standard formal potential of N2/N3-, EN2/N3-0′, is evaluated to be 0.193 ± 0.003 V vs. Li+/Li (pN2 = 1 atm,xN3- = 1) at 673 K. The dependence of EN2/N3-0′ upon the temperature (605-721 K) gives a linear relation, whose slope is (-0.790 ± 0.096) × 10-3 V K-1. Thermodynamic quantities for formation of Li3N in the melt are also estimated.

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