🤓 Based on our data, we think this question is relevant for Professor Gower's class at UF.
The nicad (nickel-cadmium) batteries have a slightly lower cell potential than the common alkaline value of 1.5 V normally used in flashlights. They have a cadmium anode, which is oxidized to Cd(OH)2(s) in a basic background electrolyte of concentrated OH-, and a cathode half-reaction in which NiO(OH)(s) is reduced to Ni(OH)2(s). What is the value of ΔG cell?
The standard reduction potentials of the half-reactions in nicad batteries are:
Cd (OH)2(s) + 2e- → Cd(s) + 2OH-(aq) E°red = -0.403 V
2NiO(OH)(s) + 2H2O(l) + 2e- → 2Ni(OH)2(s) + 2OH-(aq) E°red = 1.32 V