Mercuric oxide dry-cell batteries are often used where a highenergy density is required, such as in watches

Question:

Mercuric oxide dry-cell batteries are often used where a highenergy density is 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 for the cathode reaction is + 0.098. 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?