3. (a) b C. d. e. f. Given 0.01 Molar concentration Au³+ ion and 0.01 molar of Ag+ ion, and the following reaction: T Au³(aq) Ag+ (aq) -→ Au (s) -→ Ag (s) Write the balanced oxidation reduction equation for the cell E° = 1.52 V Eº = 0.80 V Which specie is being oxidized Which Specie is at the anode? Which Specie is the oxidizing agent? Which specie lost electron/s? Which specie saw an increase in oxidation state? Calculate the Ecell at non-standard condition for the reaction

3. (a) b C. d. e. f. Given 0.01 Molar concentration Au³+ ion and 0.01 molar of Ag+ ion, and the following reaction: T Au³(aq) Ag+ (aq) -→ Au (s) -→ Ag (s) Write the balanced oxidation reduction equation for the cell E° = 1.52 V Eº = 0.80 V Which specie is being oxidized Which Specie is at the anode? Which Specie is the oxidizing agent? Which specie lost electron/s? Which specie saw an increase in oxidation state? Calculate the Ecell at non-standard condition for the reaction

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 76AP

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