Calculate the cell potential of a cell operating with the following reaction at 25°C in which [CryO,] 0.040 M, I] 0.015 M. [Cr+] 0.35 M, and [H*]=0.35 M. Or3O (aq) + 61 (aq) + 14H* (aq) → 2Cr** (aq) + 312(s) + 7H3O(1) Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Standard Half-Reaction Potential, E (V) I(s) +2e 21 (aq) 0.54 CryO, (aq) + 14H* (aq) + 6e" 2Cr* (aq) + 7H30(1) 1.33
Calculate the cell potential of a cell operating with the following reaction at 25°C in which [CryO,] 0.040 M, I] 0.015 M. [Cr+] 0.35 M, and [H*]=0.35 M. Or3O (aq) + 61 (aq) + 14H* (aq) → 2Cr** (aq) + 312(s) + 7H3O(1) Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Standard Half-Reaction Potential, E (V) I(s) +2e 21 (aq) 0.54 CryO, (aq) + 14H* (aq) + 6e" 2Cr* (aq) + 7H30(1) 1.33
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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**
Calculate the cell potential of a cell operating with the following reaction at 25°C in which:
- \([ \text{Cr}_2\text{O}_7^{2-} ] = 0.040 \, M\)
- \([ \text{I}^- ] = 0.015 \, M\)
- \([ \text{Cr}^{3+} ] = 0.35 \, M\)
- \([ \text{H}^+ ] = 0.35 \, M\)
**Chemical Reaction:**
\[
\text{Cr}_2\text{O}_7^{2-} (\text{aq}) + 6 \text{I}^- (\text{aq}) + 14 \text{H}^+ (\text{aq}) \rightarrow 2 \text{Cr}^{3+} (\text{aq}) + 3 \text{I}_2 (\text{s}) + 7 \text{H}_2\text{O} (\text{l})
\]
**Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C:**
| **Cathode (Reduction) Half-Reaction** | **Standard Potential, \(E^\circ\) (V)** |
|---------------------------------------------------------------|---------------------------|
| \(\text{I}_2 (\text{s}) + 2 \text{e}^- \rightarrow 2 \text{I}^- (\text{aq}) \) | 0.54 |
| \(\text{Cr}_2\text{O}_7^{2-} (\text{aq}) + 14 \text{H}^+ (\text{aq}) + 6 \text{e}^- \rightarrow 2 \text{Cr}^{3+} (\text{aq}) + 7 \text{H}_2\text{O} (\text{l}) \) | 1.33 |
This information details the standard reduction potentials for the half-reactions occurring in the cell, which are necessary to compute the total cell potential.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbb73fb8a-31b7-4923-8717-ff0579a4856b%2F0861f34d-6cb9-454c-b5ad-de771c706242%2Fcxrlu8_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Calculation of Cell Potential**
Calculate the cell potential of a cell operating with the following reaction at 25°C in which:
- \([ \text{Cr}_2\text{O}_7^{2-} ] = 0.040 \, M\)
- \([ \text{I}^- ] = 0.015 \, M\)
- \([ \text{Cr}^{3+} ] = 0.35 \, M\)
- \([ \text{H}^+ ] = 0.35 \, M\)
**Chemical Reaction:**
\[
\text{Cr}_2\text{O}_7^{2-} (\text{aq}) + 6 \text{I}^- (\text{aq}) + 14 \text{H}^+ (\text{aq}) \rightarrow 2 \text{Cr}^{3+} (\text{aq}) + 3 \text{I}_2 (\text{s}) + 7 \text{H}_2\text{O} (\text{l})
\]
**Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C:**
| **Cathode (Reduction) Half-Reaction** | **Standard Potential, \(E^\circ\) (V)** |
|---------------------------------------------------------------|---------------------------|
| \(\text{I}_2 (\text{s}) + 2 \text{e}^- \rightarrow 2 \text{I}^- (\text{aq}) \) | 0.54 |
| \(\text{Cr}_2\text{O}_7^{2-} (\text{aq}) + 14 \text{H}^+ (\text{aq}) + 6 \text{e}^- \rightarrow 2 \text{Cr}^{3+} (\text{aq}) + 7 \text{H}_2\text{O} (\text{l}) \) | 1.33 |
This information details the standard reduction potentials for the half-reactions occurring in the cell, which are necessary to compute the total cell potential.
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