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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) +...
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?
