The cell reactions occurring in a battery are given by:

Cathode : 2MnO2 (s) + H2O (l) + 2e-→ Mn2O3 (s) + 2HO- (aq) E 0 red = +0.15 V

Anode : Zn (s) + 2HO- (aq) → Zn(OH)2 (s) + 2e- E 0 red = -1.25 V

1) What is the overall cell potential? What is the free energy change for this process?

2) During the discharge of the battery, 2.00 g of Mn2O3 is produced at the cathode. How many grams of Zn were consumed?

3) Consider this half reaction:

Cd(OH)2 + 2e- → Cd(s) + 2HO-

(aq) E°red = -0.76V

What is the overall cell potential and free energy change of the battery described above if the Zn

anode is replaced by Cd?