Calculate the standard emf of the cell: `Cd| Cd^(2+) ||Cu^(2+)| Cu` and determine the cell reaction. The standard reduction potentials of `Cu^(2+)| Cu` and `Cd^(2+)|Cd` are 0.34V and -0.40 volts respectively. Predict the feasibility of the cell reaction.

Explanation

Cell reactions:
Oxidation at anode: `Cd(s) rarr Cd^(2+) (aq) +2e^(-) " " (E_("ox")^(@))_(Cd|Cd^(2+))= 0.4 V `
Reduction at cathode: `Cu^(2+) (aq) + 2e^(-) rarr Cu (s) " " (E_("red")^(@))_(Cu^(2+)|Cu)= 0.34 V `
`Cd(s) + 2e rarr Cd^(2+) (aq) + Cu (s)`
`E_("cell")^(@) = (E_("ox")^(@)) + (E_(red)^(@))_("cathode")`
`= 0.4 + 0.34 `
`= 0.74 V . `
emf is +ve , so `DeltaG ` is (-) ve the reaction is feasible