4. Lead-acid batteries are used in automobiles. The oxidation and reduction half-reactions are: Pb(s) + HSO4 → PbSO4(s) + H* + 2 e PbO2(s) + 3 H* + HSO4 + 2 e → PBSO4(s) + 2 H2O(1) E° = +0.356 V E° = +1.685 V %3D a. Write out the complete balanced redox equation and calculate its standard potential (E°). b. Write out the reaction quotient expression (Q) for this system. c. Calculate the actual voltage (E) generated by the battery at 100.0 °C when [H*]= [HSO4] = 18.1 M %3D %3D d. If a higher (positive) voltage is desired, can this be accomplished by lowering the operational temperature? ... by adding water to dilute the H* and HSO4 species in the battery? Justify your answers.
4. Lead-acid batteries are used in automobiles. The oxidation and reduction half-reactions are: Pb(s) + HSO4 → PbSO4(s) + H* + 2 e PbO2(s) + 3 H* + HSO4 + 2 e → PBSO4(s) + 2 H2O(1) E° = +0.356 V E° = +1.685 V %3D a. Write out the complete balanced redox equation and calculate its standard potential (E°). b. Write out the reaction quotient expression (Q) for this system. c. Calculate the actual voltage (E) generated by the battery at 100.0 °C when [H*]= [HSO4] = 18.1 M %3D %3D d. If a higher (positive) voltage is desired, can this be accomplished by lowering the operational temperature? ... by adding water to dilute the H* and HSO4 species in the battery? Justify your answers.
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
parts c and d!
![4. Lead-acid batteries are used in automobiles. The oxidation and reduction half-reactions are:
Pb(s) + HSO4 → PbSO4(s) + H* + 2 e
PbO2(s) + 3 H* + HSO4 + 2 e → PBSO4(s) + 2 H2O(1)
E° = +0.356 V
E° = +1.685 V
%3D
a.
Write out the complete balanced redox equation and calculate its standard potential (E°).
b. Write out the reaction quotient expression (Q) for this system.
c. Calculate the actual voltage (E) generated by the battery at 100.0 °C when [H*]= [HSO4]
= 18.1 M
%3D
%3D
d. If a higher (positive) voltage is desired, can this be accomplished by lowering the
operational temperature? ... by adding water to dilute the H* and HSO4 species in the
battery? Justify your answers.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5710f6d1-3a7e-447a-ae07-d8e6fb165081%2F9c452ae2-2a1b-4240-b6ed-ba62f75385cf%2F4mmmmnv.jpeg&w=3840&q=75)
Transcribed Image Text:4. Lead-acid batteries are used in automobiles. The oxidation and reduction half-reactions are:
Pb(s) + HSO4 → PbSO4(s) + H* + 2 e
PbO2(s) + 3 H* + HSO4 + 2 e → PBSO4(s) + 2 H2O(1)
E° = +0.356 V
E° = +1.685 V
%3D
a.
Write out the complete balanced redox equation and calculate its standard potential (E°).
b. Write out the reaction quotient expression (Q) for this system.
c. Calculate the actual voltage (E) generated by the battery at 100.0 °C when [H*]= [HSO4]
= 18.1 M
%3D
%3D
d. If a higher (positive) voltage is desired, can this be accomplished by lowering the
operational temperature? ... by adding water to dilute the H* and HSO4 species in the
battery? Justify your answers.
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 2 steps with 2 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