(a) Write the reactions for the discharge and charge of a nickel–cadmium (nicad) rechargeable battery. (b) Given the following reduction potentials, calculate the standard emf of the cell: Cd(OH)2(s) + 2 e-→ Cd(s) + 2 OH-(aq)E°red = -0.76 V
NiO(OH)(s) + H2O(l) + e-→ Ni(OH)2(s) + OH-(aq)E°red = +0.49 V (c) A typical nicad voltaic cell generates an emf of +1.30 V. Why is there a difference between this value and the one you calculated in part (b)? (d) Calculate the equilibrium constant for the overall nicad reaction based on this typical emf value.
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