**Electrochemical Reactions in a Tin-Silver Cell**In this exercise, we will write the half-reactions for each electrode and the net cell reaction for an electrochemical cell containing tin and silver. The cell notation is as follows:\[ \text{Sn(s)} \lvert \text{Sn}^{2+}(\text{aq}) \parallel \text{Ag}^{+}(\text{aq)} \lvert \text{Ag(s)} \]**Anode Reaction:**At the anode, oxidation occurs. The half-reaction is:\[ \text{Sn(s)} \rightarrow \text{Sn}^{2+}(\text{aq}) + 2\text{e}^- \]**Cathode Reaction:**At the cathode, reduction happens. The half-reaction is:\[ \text{Ag}^{+}(\text{aq}) + \text{e}^- \rightarrow \text{Ag(s)} \]**Net Cell Reaction:**Combining the half-reactions, the net cell reaction is:\[ \text{Sn(s)} + 2\text{Ag}^{+}(\text{aq}) \rightarrow \text{Sn}^{2+}(\text{aq}) + 2\text{Ag(s)} \]This shows the overall electron transfer and species involved.

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Write the half-reactions as they occur at each electrode and the net cell reaction for this electrochemical cell containing tin and silver. Sn(s)|Sn²* (aq)||Ag*(aq)|Ag(s) anode: cathode: net cell reaction:

Write the half-reactions as they occur at each electrode and the net cell reaction for this electrochemical cell containing tin and silver. Sn(s)|Sn²* (aq)||Ag*(aq)|Ag(s) anode: cathode: net cell reaction:

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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