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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![**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.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1d39eb1c-3154-4bee-b19a-a1be6277f6e8%2F3b4abd4e-8605-4917-8d48-528766a37718%2F6wt11rk_processed.png&w=3840&q=75)
Transcribed Image Text:**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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