In an electrochemical cell, Cu(s) is placed in the anode half-cell while Ag(s) in the cathode half-cell. The standard potential of the half-reactionsare as follows:Ag++e¯→ Ag(s)(aq)E°red = +0.80 VCu2+(aq)E°red = +0.34 V+2 e -Cu(s)What can be said about the reaction?O The reaction is non-spontaneous.O The reaction is spontaneous.O The reaction produces electricity.O The reaction will proceed naturally.

Given: Anode is Cu and cathode is Ag.

In an electrochemical cell, Cu(s) is placed in the anode half-cell while Ag(s) in the cathode half-cell. The standard potential of the half-reactions are as follows: Ag+ +e→ (aq) Ag(s) E°red = +0.80 V Cu2+ (ад) + 2 e → Cu(s) E°red = +0. 34 V What can be said about the reaction? O The reaction is non-spontaneous, O The reaction is spontaneous. O The reaction produces electricity. O The reaction will proceed naturally.

In an electrochemical cell, Cu(s) is placed in the anode half-cell while Ag(s) in the cathode half-cell. The standard potential of the half-reactions are as follows: Ag+ +e→ (aq) Ag(s) E°red = +0.80 V Cu2+ (ад) + 2 e → Cu(s) E°red = +0. 34 V What can be said about the reaction? O The reaction is non-spontaneous, O The reaction is spontaneous. O The reaction produces electricity. O The reaction will proceed naturally.

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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