What is E cell for the following reaction? 2 Ag(s) + Sn²+ (aq) → 2 Ag*(aq) + Sn(s) Ag (aq) + e E = 0.80 V Sn4+ (aq) + 2e E = 0.13 V (aq) 2+ Sn²(aq) + 2e Ag(s) → Sn2+ Sn2+ Sn(s) E = -0.14 V
What is E cell for the following reaction? 2 Ag(s) + Sn²+ (aq) → 2 Ag*(aq) + Sn(s) Ag (aq) + e E = 0.80 V Sn4+ (aq) + 2e E = 0.13 V (aq) 2+ Sn²(aq) + 2e Ag(s) → Sn2+ Sn2+ Sn(s) E = -0.14 V
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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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![### Calculation of Cell Potential for a Redox Reaction
The following problem involves determining the standard cell potential (\(E^\circ_{\text{cell}}\)) for a given redox reaction. The cell reaction is:
\[ 2 \text{Ag}(s) + \text{Sn}^{2+}(aq) \rightarrow 2 \text{Ag}^+(aq) + \text{Sn}(s) \]
**Standard Reduction Potentials:**
1. \(\text{Ag}^+(aq) + e^- \rightarrow \text{Ag}(s)\)
- \(E^\circ = 0.80 \, \text{V}\)
2. \(\text{Sn}^{4+}(aq) + 2e^- \rightarrow \text{Sn}^{2+}(aq)\)
- \(E^\circ = 0.13 \, \text{V}\)
3. \(\text{Sn}^{2+}(aq) + 2e^- \rightarrow \text{Sn}(s)\)
- \(E^\circ = -0.14 \, \text{V}\)
**Explanation of Reaction Components:**
- The reaction involves silver (\(\text{Ag}\)) and tin (\(\text{Sn}\)) ions where silver is oxidized from its elemental form to \(\text{Ag}^+\) ions, and \(\text{Sn}^{2+}\) ions are reduced to tin metal.
- The cell potential is calculated using the standard reduction potentials provided for each half-reaction, which will help in determining the feasibility and spontaneity of the reaction.
**Graphical Explanation (If Applicable):**
For educational purposes, graphs or diagrams might typically illustrate the process such as placing the reactions on an electrochemical series chart, or visualizing cell components. However, in this context, no specific diagrams are provided with the information.
The final step would be to use the given potentials to calculate the standard cell potential for the complete reaction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2ceb2d65-29b4-49d4-9830-4ba06589987b%2F4d0bc412-e64d-4541-85c9-22bda0ce6957%2Fo8li1wn_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Calculation of Cell Potential for a Redox Reaction
The following problem involves determining the standard cell potential (\(E^\circ_{\text{cell}}\)) for a given redox reaction. The cell reaction is:
\[ 2 \text{Ag}(s) + \text{Sn}^{2+}(aq) \rightarrow 2 \text{Ag}^+(aq) + \text{Sn}(s) \]
**Standard Reduction Potentials:**
1. \(\text{Ag}^+(aq) + e^- \rightarrow \text{Ag}(s)\)
- \(E^\circ = 0.80 \, \text{V}\)
2. \(\text{Sn}^{4+}(aq) + 2e^- \rightarrow \text{Sn}^{2+}(aq)\)
- \(E^\circ = 0.13 \, \text{V}\)
3. \(\text{Sn}^{2+}(aq) + 2e^- \rightarrow \text{Sn}(s)\)
- \(E^\circ = -0.14 \, \text{V}\)
**Explanation of Reaction Components:**
- The reaction involves silver (\(\text{Ag}\)) and tin (\(\text{Sn}\)) ions where silver is oxidized from its elemental form to \(\text{Ag}^+\) ions, and \(\text{Sn}^{2+}\) ions are reduced to tin metal.
- The cell potential is calculated using the standard reduction potentials provided for each half-reaction, which will help in determining the feasibility and spontaneity of the reaction.
**Graphical Explanation (If Applicable):**
For educational purposes, graphs or diagrams might typically illustrate the process such as placing the reactions on an electrochemical series chart, or visualizing cell components. However, in this context, no specific diagrams are provided with the information.
The final step would be to use the given potentials to calculate the standard cell potential for the complete reaction.
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