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3. A battery is available using Ni-Cd redox reaction. Given the half-cell reactions for these species as follows. NiO2(s) + 2H2O + 2e Ni(OH)2(s) + 20H Cd2+ + 2e Cd(s) E° = -0.49 volts E° = -0.783 volts (a) Write the cathode and anode half reactions and the whole stoichiometric equation. (b) What is the value of the cell electrode potential (E° cell) and the equilibrium constant (K), respectively, for the reaction under standard condition? (c) What is the free energy change (AG) for the reaction?

3. A battery is available using Ni-Cd redox reaction. Given the half-cell reactions for these species as follows. NiO2(s) + 2H2O + 2e Ni(OH)2(s) + 20H Cd2+ + 2e Cd(s) E° = -0.49 volts E° = -0.783 volts (a) Write the cathode and anode half reactions and the whole stoichiometric equation. (b) What is the value of the cell electrode potential (E° cell) and the equilibrium constant (K), respectively, for the reaction under standard condition? (c) What is the free energy change (AG) for the reaction?

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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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3. A battery is available using Ni-Cd redox reaction. Given the half-cell reactions for these species as follows. NiO2(s) + 2H2O + 2e Ni(OH)2(s) + 20H Cd2+ + 2e Cd(s) E° = -0.49 volts E° = -0.783 volts (a) Write the cathode and anode half reactions and the whole stoichiometric equation. (b) What is the value of the cell electrode potential (E° cell) and the equilibrium constant (K), respectively, for the reaction under standard condition? (c) What is the free energy change (AG) for the reaction?
Transcribed Image Text:3. A battery is available using Ni-Cd redox reaction. Given the half-cell reactions for these species as follows. NiO2(s) + 2H2O + 2e Ni(OH)2(s) + 20H Cd2+ + 2e Cd(s) E° = -0.49 volts E° = -0.783 volts (a) Write the cathode and anode half reactions and the whole stoichiometric equation. (b) What is the value of the cell electrode potential (E° cell) and the equilibrium constant (K), respectively, for the reaction under standard condition? (c) What is the free energy change (AG) for the reaction?
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