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The voltaic cell described by the notation below measured a potential of 2.3 V. If the reaction was maintained at 30° calculate the standard reduction potential of the cathode half-cell. Pt(s) | J²- (1.50 M) | J(1) || Ag* (0.013 M) | Ag(s) Use R = 8.314 J/mol-K; F = 96485 C/mol)

The voltaic cell described by the notation below measured a potential of 2.3 V. If the reaction was maintained at 30° calculate the standard reduction potential of the cathode half-cell. Pt(s) | J²- (1.50 M) | J(1) || Ag* (0.013 M) | Ag(s) Use R = 8.314 J/mol-K; F = 96485 C/mol)

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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The voltaic cell described by the notation below measured a potential of 2.3 V. If the reaction was maintained at 30°C calculate the standard reduction potential of the cathode half-cell. Pt(s) | J²- (1.50 M) | J(1) || Ag† (0.013 M) | Ag(s) (Use R = 8.314 J/mol-K; F = 96485 C/mol)
Transcribed Image Text:The voltaic cell described by the notation below measured a potential of 2.3 V. If the reaction was maintained at 30°C calculate the standard reduction potential of the cathode half-cell. Pt(s) | J²- (1.50 M) | J(1) || Ag† (0.013 M) | Ag(s) (Use R = 8.314 J/mol-K; F = 96485 C/mol)
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