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 degree Red for the cathode reaction is +0.098V. The overall cell potential is 1.35V. Assuming that the both half-cells operate under standard conditions, what is the standard reduction potential for the anode reaction?