Homework Help is Here – Start Your Trial Now!
Science
Chemistry
3. In the lead storage battery, lead serves as the anode, and lead coated with lead oxide serves as the cathode. Both electrodes dip into an electrolyte solution of sulfuric acid. The electrode reactions are Pb(s) + HSO4 (aq) → PbSO4(s) + H+ (aq) + 2e¯ PbO₂ (s) + HSO4 (aq) + 3H+ (aq) + 2e → PbSO4(s) + 2H₂O(l) E ox = +0.35V Eºred = +1.69V Cell reaction: Pb(s) + PbO₂ (s) + 2HSO (aq) + 2H+ (aq) → 2PbSO4(s) + 2H₂0 (1) (The given standard reduction/oxidation potentials were measured at 25°C). a. b. Calculate the standard cell potential, Eº, for this cell at 25°C. The concentration of sulfuric acid in a car battery is 6 M, when the battery is fully charged. Use the Nernst equation to determine the cell potential, E. Remember that sulfuric acid is a strong acid (use only the first proton).

3. In the lead storage battery, lead serves as the anode, and lead coated with lead oxide serves as the cathode. Both electrodes dip into an electrolyte solution of sulfuric acid. The electrode reactions are Pb(s) + HSO4 (aq) → PbSO4(s) + H+ (aq) + 2e¯ PbO₂ (s) + HSO4 (aq) + 3H+ (aq) + 2e → PbSO4(s) + 2H₂O(l) E ox = +0.35V Eºred = +1.69V Cell reaction: Pb(s) + PbO₂ (s) + 2HSO (aq) + 2H+ (aq) → 2PbSO4(s) + 2H₂0 (1) (The given standard reduction/oxidation potentials were measured at 25°C). a. b. Calculate the standard cell potential, Eº, for this cell at 25°C. The concentration of sulfuric acid in a car battery is 6 M, when the battery is fully charged. Use the Nernst equation to determine the cell potential, E. Remember that sulfuric acid is a strong acid (use only the first proton).

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter19: Electrochemistry
Section: Chapter Questions
Problem 19.118QP
See similar textbooks
icon
Related questions
Question
How can we solve question 3 ?
3. In the lead storage battery, lead serves as the anode, and lead coated with lead oxide serves as the cathode. Both electrodes dip into an electrolyte solution of sulfuric acid. The electrode reactions are Pb(s) + HSO4 (aq) → PbSO4(s) + H+ (aq) + 2e¯ PbO₂ (s) + HSO4 (aq) + 3H+ (aq) + 2e → → PbSO4(s) + 2H₂O(l) E ox = +0.35V Eºred = +1.69V Cell reaction: Pb(s) + PbO₂ (s) + 2HSO (aq) + 2H+ (aq) → 2PbSO4(s) + 2H₂O(l) (The given standard reduction/oxidation potentials were measured at 25°C). a. b. Calculate the standard cell potential, Eº, for this cell at 25°C. The concentration of sulfuric acid in a car battery is 6 M, when the battery is fully charged. Use the Nernst equation to determine the cell potential, E. Remember that sulfuric acid is a strong acid (use only the first proton).
Transcribed Image Text:3. In the lead storage battery, lead serves as the anode, and lead coated with lead oxide serves as the cathode. Both electrodes dip into an electrolyte solution of sulfuric acid. The electrode reactions are Pb(s) + HSO4 (aq) → PbSO4(s) + H+ (aq) + 2e¯ PbO₂ (s) + HSO4 (aq) + 3H+ (aq) + 2e → → PbSO4(s) + 2H₂O(l) E ox = +0.35V Eºred = +1.69V Cell reaction: Pb(s) + PbO₂ (s) + 2HSO (aq) + 2H+ (aq) → 2PbSO4(s) + 2H₂O(l) (The given standard reduction/oxidation potentials were measured at 25°C). a. b. Calculate the standard cell potential, Eº, for this cell at 25°C. The concentration of sulfuric acid in a car battery is 6 M, when the battery is fully charged. Use the Nernst equation to determine the cell potential, E. Remember that sulfuric acid is a strong acid (use only the first proton).
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 4 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Balancing of Redox Reactions
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.
Similar questions
Recommended textbooks for you
General Chemistry - Standalone book (MindTap Cour…
General Chemistry - Standalone book (MindTap Cour…
Chemistry
ISBN:
9781305580343
Author:
Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:
Cengage Learning
Chemistry: Principles and Practice
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781133949640
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Principles of Modern Chemistry
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
SEE MORE TEXTBOOKS