Mercuric oxide dry-cell batteries are often used where a high-energy density is required, such as in watches and cameras. The two half-cell reactions that occur in the battery are HgO(s)+H2O(l)+2e−→Hg(l)+2OH−(aq) Zn(s)+2OH−(aq)→ZnO(s)+H2O(l)+2e− (a) Write the overall cell reaction. (b) The value of E∘redfor the cathode reaction is +0.098V . The overall cell potential is +1.35V . Assuming that both half-cells operate under standard conditions, what is the standard reduction potential for the anode reaction?
Mercuric oxide dry-cell batteries are often used where a high-energy density is required, such as in watches and cameras. The two half-cell reactions that occur in the battery are HgO(s)+H2O(l)+2e−→Hg(l)+2OH−(aq) Zn(s)+2OH−(aq)→ZnO(s)+H2O(l)+2e− (a) Write the overall cell reaction. (b) The value of E∘redfor the cathode reaction is +0.098V . The overall cell potential is +1.35V . Assuming that both half-cells operate under standard conditions, what is the standard reduction potential for the anode 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...
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1. Mercuric oxide dry-cell batteries are often used where a high-energy density is required, such as in watches and cameras. The two half-cell reactions that occur in the battery are
HgO(s)+H2O(l)+2e−→Hg(l)+2OH−(aq)
Zn(s)+2OH−(aq)→ZnO(s)+H2O(l)+2e−
(a) Write the overall cell reaction.
(b) The value of E∘redfor the cathode reaction is +0.098V . The overall cell potential is +1.35V . Assuming that both half-cells operate under standard conditions, what is the standard reduction potential for the anode reaction?
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