A solution containing 0.20 M Pb²*, 1.5 × 10-6 M Pb** , 1.5 × 10-“ M Mn²+ , 0.20 M MnO, , and 0.88 M HNO, was prepared. For this solution, the balanced reduction half-reactions and overall net reaction shown can occur. 5 [Pb++ + 2e- = Pb²+] 2 [MnO, + 8 H* + 5e-= Mn²+ + 4H,0] 5 Pb** + 2 Mn²* + 8 H,0=5 Pb²* + 2MNO, + 16H* E; = 1.690 V E = 1.507 V Determine Eel, AG", and K for this reaction.
A solution containing 0.20 M Pb²*, 1.5 × 10-6 M Pb** , 1.5 × 10-“ M Mn²+ , 0.20 M MnO, , and 0.88 M HNO, was prepared. For this solution, the balanced reduction half-reactions and overall net reaction shown can occur. 5 [Pb++ + 2e- = Pb²+] 2 [MnO, + 8 H* + 5e-= Mn²+ + 4H,0] 5 Pb** + 2 Mn²* + 8 H,0=5 Pb²* + 2MNO, + 16H* E; = 1.690 V E = 1.507 V Determine Eel, AG", and K for this reaction.
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
Calculate the value for the cell potential, ?cellEcell, and the free energy, Δ?ΔG, for the given conditions.
Calculate the value of ?cellEcell for this system at equilibrium.
Determine the pH at which the given concentrations of Pb2+Pb2+ , Pb4+Pb4+ , Mn2+Mn2+ , and MnO−4MnO4− would be at equilibrium.
![**Chemistry Problem: Determining Cell Potential and Free Energy**
A solution containing 0.20 M \( \text{Pb}^{2+} \), \( 1.5 \times 10^{-6} \) M \( \text{Pb}^{4+} \), \( 1.5 \times 10^{-6} \) M \( \text{Mn}^{2+} \), 0.20 M \( \text{MnO}_4^- \), and 0.88 M \( \text{HNO}_3 \) was prepared. For this solution, the balanced reduction half-reactions and overall net reaction shown can occur:
1. \( 5[\text{Pb}^{4+} + 2e^- \rightleftharpoons \text{Pb}^{2+}] \)
- \( E^{o} = 1.690 \, \text{V} \)
2. \( 2[\text{MnO}_4^- + 8 \text{H}^+ + 5e^- \rightleftharpoons \text{Mn}^{2+} + 4 \text{H}_2\text{O}] \)
- \( E^{o} = 1.507 \, \text{V} \)
**Overall Reaction:**
\[ 5\text{Pb}^{4+} + 2\text{Mn}^{2+} + 8 \text{H}_2\text{O} \rightleftharpoons 5\text{Pb}^{2+} + 2\text{MnO}_4^- + 16 \text{H}^+ \]
---
**Determine \( E_{\text{cell}}^{o} \), \( \Delta G^{o} \), and \( K \) for this reaction.**
\[ E_{\text{cell}}^{o} = \underline{\hspace{5cm}} \, \text{V} \]
\[ \Delta G^{o} = \underline{\hspace{5cm}} \, \text{J} \]
\[ K = \underline{\hspace{6cm}} \]
---
**Calculate the value for the cell potential, \( E_{\text{cell}} \), and the free energy, \( \Delta G \), for the given conditions.**
\[ E_{\text{cell}} = \underline](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8d1b31df-0f67-47d9-936e-b5ce55c8aa00%2Fd2176ae8-63be-45c3-aba1-af0925c66648%2Fbr3bqkl_processed.png&w=3840&q=75)
Transcribed Image Text:**Chemistry Problem: Determining Cell Potential and Free Energy**
A solution containing 0.20 M \( \text{Pb}^{2+} \), \( 1.5 \times 10^{-6} \) M \( \text{Pb}^{4+} \), \( 1.5 \times 10^{-6} \) M \( \text{Mn}^{2+} \), 0.20 M \( \text{MnO}_4^- \), and 0.88 M \( \text{HNO}_3 \) was prepared. For this solution, the balanced reduction half-reactions and overall net reaction shown can occur:
1. \( 5[\text{Pb}^{4+} + 2e^- \rightleftharpoons \text{Pb}^{2+}] \)
- \( E^{o} = 1.690 \, \text{V} \)
2. \( 2[\text{MnO}_4^- + 8 \text{H}^+ + 5e^- \rightleftharpoons \text{Mn}^{2+} + 4 \text{H}_2\text{O}] \)
- \( E^{o} = 1.507 \, \text{V} \)
**Overall Reaction:**
\[ 5\text{Pb}^{4+} + 2\text{Mn}^{2+} + 8 \text{H}_2\text{O} \rightleftharpoons 5\text{Pb}^{2+} + 2\text{MnO}_4^- + 16 \text{H}^+ \]
---
**Determine \( E_{\text{cell}}^{o} \), \( \Delta G^{o} \), and \( K \) for this reaction.**
\[ E_{\text{cell}}^{o} = \underline{\hspace{5cm}} \, \text{V} \]
\[ \Delta G^{o} = \underline{\hspace{5cm}} \, \text{J} \]
\[ K = \underline{\hspace{6cm}} \]
---
**Calculate the value for the cell potential, \( E_{\text{cell}} \), and the free energy, \( \Delta G \), for the given conditions.**
\[ E_{\text{cell}} = \underline
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 5 steps with 4 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