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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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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