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

Explanation

Cell reactions:
`{:("Oxidation at anode":, Cd(s) to Cd^(2+)(aq) + Cu(s)`
`E_("cell")^(@) = (E_("ox")^(@)) + (E_("Red")^(@)) = 0.4 + 0.34 = 0.74 V`
emf is +ve , so `DeltaG` is (-)ve, the reaction is feasible.