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?

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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter18: Electrochemistry
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Problem 133CWP: Consider a galvanic cell based on the following half-reactions: a. What is the expected cell...
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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?

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