A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ MnO₂ (s) + 4H* (aq) + 2Cr²+ (aq) → Mn²+ (aq) + 2H₂O (1) +2Cr³+ (aq) Suppose the cell is prepared with 3.73 MH* and 1.42 M Cr²+ in one half-cell and 4.21 M Mn² and 3.05 M Cr³+ in the other. 2+ 2+ 3+ Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 0 0 x10 0.0 X μ ☐ □
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ MnO₂ (s) + 4H* (aq) + 2Cr²+ (aq) → Mn²+ (aq) + 2H₂O (1) +2Cr³+ (aq) Suppose the cell is prepared with 3.73 MH* and 1.42 M Cr²+ in one half-cell and 4.21 M Mn² and 3.05 M Cr³+ in the other. 2+ 2+ 3+ Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 0 0 x10 0.0 X μ ☐ □
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 77AP
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![A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction:
\[ \text{MnO}_2(s) + 4\text{H}^+ (aq) + 2\text{Cr}^{2+} (aq) \rightarrow \text{Mn}^{2+} (aq) + 2\text{H}_2\text{O} (l) + 2\text{Cr}^{3+} (aq) \]
Suppose the cell is prepared with 3.73 M \(\text{H}^+\) and 1.42 M \(\text{Cr}^{2+}\) in one half-cell and 4.21 M \(\text{Mn}^{2+}\) and 3.05 M \(\text{Cr}^{3+}\) in the other.
Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.
**Diagram Explanation:**
The image contains a box indicating input for calculations and a button interface with mathematical symbols. These symbols assist in inputting values or equations for calculating the cell voltage, such as exponents or square roots. The diagram does not provide specific values or results.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4d129ec3-2103-4980-864a-9b2eb629bd11%2Fc7ed66f3-283f-4a6a-91fc-fb4424575b83%2F833fisj_processed.jpeg&w=3840&q=75)
Transcribed Image Text:A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction:
\[ \text{MnO}_2(s) + 4\text{H}^+ (aq) + 2\text{Cr}^{2+} (aq) \rightarrow \text{Mn}^{2+} (aq) + 2\text{H}_2\text{O} (l) + 2\text{Cr}^{3+} (aq) \]
Suppose the cell is prepared with 3.73 M \(\text{H}^+\) and 1.42 M \(\text{Cr}^{2+}\) in one half-cell and 4.21 M \(\text{Mn}^{2+}\) and 3.05 M \(\text{Cr}^{3+}\) in the other.
Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.
**Diagram Explanation:**
The image contains a box indicating input for calculations and a button interface with mathematical symbols. These symbols assist in inputting values or equations for calculating the cell voltage, such as exponents or square roots. The diagram does not provide specific values or results.
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