The diagram below shows the experimental setup for a typical electrochemical cell that contains two standard half-cells. The cell operates according to the reaction represented by the following equation. Zn (s) + Ni2+ (aq) → Ni (s) + Zn²+ (aq) Salt Bridge in SO X2+ SO a. Identify M and M²+ in the diagram and specify the initial concentration for M²+ in solution. b. Indicate which of the metal electrodes is the cathode. Write the balanced equation for the reaction that occurs in the half-cell containing the cathode. c. What would be the effect on the cell voltage if the concentration of Zn2+ was reduced to 0.100 Min the half-cell containing the Zn electrode? d. Describe what would happen to the cell voltage if the salt bridge was removed. Explain.

The diagram below shows the experimental setup for a typical electrochemical cell that contains two standard half-cells. The cell operates according to the reaction represented by the following equation. Zn (s) + Ni2+ (aq) → Ni (s) + Zn²+ (aq) Salt Bridge in SO X2+ SO a. Identify M and M²+ in the diagram and specify the initial concentration for M²+ in solution. b. Indicate which of the metal electrodes is the cathode. Write the balanced equation for the reaction that occurs in the half-cell containing the cathode. c. What would be the effect on the cell voltage if the concentration of Zn2+ was reduced to 0.100 Min the half-cell containing the Zn electrode? d. Describe what would happen to the cell voltage if the salt bridge was removed. Explain.

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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Question

The diagram below shows the experimental setup for a typical electrochemical cell that contains two standard half-cells. The cell operates according to the reaction represented by the following
equation.
Zn (s) + Ni²+ (aq) → Ni (s) + Zn²+ (aq)
M²+ SO
Salt Bridge
SO₂²
a. Identify M and M²+ in the diagram and specify the initial concentration for M²+ in solution.
b. Indicate which of the metal electrodes is the cathode. Write the balanced equation for the reaction that occurs in the half-cell containing the cathode.
c. What would be the effect on the cell voltage if the concentration of Zn2+ was reduced to 0.100 M in the half-cell containing the Zn electrode?
d. Describe what would happen to the cell voltage if the salt bridge was removed. Explain.

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