Mercuric oxide dry-cell batteries are often used where aflat discharge voltage and long life are required, such asin watches and cameras. The two half-cell reactions thatoccur in the battery areHgO(s) + H2O(l) + 2 e---->Hg(l) + 2 OH-(aq)Zn(s) + 2 OH-(aq)----->ZnO(s) + H2O(l) + 2 e-(a) Write the overall cell reaction. (b) The value of E°red forthe cathode reaction is +0.098 V. The overall cell potentialis +1.35 V. Assuming that both half-cells operate understandard conditions, what is the standard reduction potentialfor the anode reaction? (c) Why is the potential of theanode reaction different than would be expected if the reactionoccurred in an acidic medium?
Mercuric oxide dry-cell batteries are often used where aflat discharge voltage and long life are required, such asin watches and cameras. The two half-cell reactions thatoccur in the battery areHgO(s) + H2O(l) + 2 e---->Hg(l) + 2 OH-(aq)Zn(s) + 2 OH-(aq)----->ZnO(s) + H2O(l) + 2 e-(a) Write the overall cell reaction. (b) The value of E°red forthe cathode reaction is +0.098 V. The overall cell potentialis +1.35 V. Assuming that both half-cells operate understandard conditions, what is the standard reduction potentialfor the anode reaction? (c) Why is the potential of theanode reaction different than would be expected if the reactionoccurred in an acidic medium?
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
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 133CWP: Consider a galvanic cell based on the following half-reactions: a. What is the expected cell...
Related questions
Question
Mercuric oxide dry-cell batteries are often used where a
flat discharge voltage and long life are required, such as
in watches and cameras. The two half-cell reactions that
occur in the battery are
HgO(s) + H2O(l) + 2 e---->Hg(l) + 2 OH-(aq)
Zn(s) + 2 OH-(aq)----->ZnO(s) + H2O(l) + 2 e-
(a) Write the overall cell reaction. (b) The value of E°red for
the cathode reaction is +0.098 V. The overall cell potential
is +1.35 V. Assuming that both half-cells operate under
standard conditions, what is the standard reduction potential
for the anode reaction? (c) Why is the potential of the
anode reaction different than would be expected if the reaction
occurred in an acidic medium?
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 3 steps
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: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
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