What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the H, pressure is 8.62×10-3 atm, the H* concentration is 1.06M, and the Mn²+ concentration is 8.18×10-4M ? 2H*(aq) + Mn(s)→ H2(g) + Mn²+(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given:
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the H, pressure is 8.62×10-3 atm, the H* concentration is 1.06M, and the Mn²+ concentration is 8.18×10-4M ? 2H*(aq) + Mn(s)→ H2(g) + Mn²+(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given:
Chemistry
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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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![**Problem Statement:**
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the \( \text{H}_2 \) pressure is \( 8.62 \times 10^{-3} \) atm, the \( \text{H}^+ \) concentration is 1.06M, and the \( \text{Mn}^{2+} \) concentration is \( 8.18 \times 10^{-4} \) M?
**Chemical Equation:**
\[ 2\text{H}^+(\text{aq}) + \text{Mn(s)} \rightarrow \text{H}_2(\text{g}) + \text{Mn}^{2+}(\text{aq}) \]
**Input Field:**
- **Answer:** [Input Box] V
**Question:**
- The cell reaction as written above is spontaneous for the concentrations given: [Dropdown Menu]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb2c2bfdd-c795-4c13-bc09-4b743040f0d9%2F2fab29cb-6de6-49da-b013-00599187057c%2Fi6vifn5_processed.png&w=3840&q=75)
Transcribed Image Text:**Problem Statement:**
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the \( \text{H}_2 \) pressure is \( 8.62 \times 10^{-3} \) atm, the \( \text{H}^+ \) concentration is 1.06M, and the \( \text{Mn}^{2+} \) concentration is \( 8.18 \times 10^{-4} \) M?
**Chemical Equation:**
\[ 2\text{H}^+(\text{aq}) + \text{Mn(s)} \rightarrow \text{H}_2(\text{g}) + \text{Mn}^{2+}(\text{aq}) \]
**Input Field:**
- **Answer:** [Input Box] V
**Question:**
- The cell reaction as written above is spontaneous for the concentrations given: [Dropdown Menu]
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