For the electrochemical cell Al(s) + 3 Mn²+ (aq) → 2 Al³+ (aq) + 3 Mn(s) (E° = 0.48 V, [A1³*] = 1.0 M), what is the value of E when [Mn²+] = 0.078 M? Assume T is 298 K
For the electrochemical cell Al(s) + 3 Mn²+ (aq) → 2 Al³+ (aq) + 3 Mn(s) (E° = 0.48 V, [A1³*] = 1.0 M), what is the value of E when [Mn²+] = 0.078 M? Assume T is 298 K
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...
Related questions
Question
![**Electrochemical Cell Calculation**
**Question 9 of 9**
**Scenario:**
For the electrochemical cell:
\[ 2 \text{Al(s)} + 3 \text{Mn}^{2+}\text{(aq)} \rightarrow 2 \text{Al}^{3+}\text{(aq)} + 3 \text{Mn(s)} \]
- Standard Cell Potential (\(E^\circ\)) = 0.48 V
- Concentration of \([\text{Al}^{3+}]\) = 1.0 M
**Problem:**
Determine the value of the cell potential (\(E\)) when the concentration of \([\text{Mn}^{2+}]\) is 0.078 M. Assume the temperature (\(T\)) is 298 K.
---
**Notes:**
- Inputs such as the standard cell potential and concentrations are vital for calculating the actual cell potential using the Nernst equation.
- The Nernst equation will account for non-standard conditions, incorporating temperature and ion concentrations to provide the cell potential (\(E\)) under specified conditions.
**Interactive Element:**
- A numeric keypad interface is provided to input answers, with buttons for numbers, decimal points, positive/negative signs, and exponential notation (x10).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbae483e7-f3a4-4a9a-ba35-bb8b04de3604%2F3012d194-0ac5-4342-a967-023aa2638c90%2Fpm7qu7w_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Electrochemical Cell Calculation**
**Question 9 of 9**
**Scenario:**
For the electrochemical cell:
\[ 2 \text{Al(s)} + 3 \text{Mn}^{2+}\text{(aq)} \rightarrow 2 \text{Al}^{3+}\text{(aq)} + 3 \text{Mn(s)} \]
- Standard Cell Potential (\(E^\circ\)) = 0.48 V
- Concentration of \([\text{Al}^{3+}]\) = 1.0 M
**Problem:**
Determine the value of the cell potential (\(E\)) when the concentration of \([\text{Mn}^{2+}]\) is 0.078 M. Assume the temperature (\(T\)) is 298 K.
---
**Notes:**
- Inputs such as the standard cell potential and concentrations are vital for calculating the actual cell potential using the Nernst equation.
- The Nernst equation will account for non-standard conditions, incorporating temperature and ion concentrations to provide the cell potential (\(E\)) under specified conditions.
**Interactive Element:**
- A numeric keypad interface is provided to input answers, with buttons for numbers, decimal points, positive/negative signs, and exponential notation (x10).
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 3 steps with 3 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY