Calculate the standard emf of the cell: `Cdabs(Cd^(2+))abs(Cu^(2+))Cu` and determine the cell reaction. The standard reduction potentials of `Cu^(2+)|Cu " and " Cd^(2+)|Cd`u 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+))=0.4V`
Reduction at cathode: `Cu^(2+)""_((aq))+2e^(-) rarr Cu_((s))`
`" "(E_("red")^(@))_(Cu^(2+)|Cu)=0.34V`
`E_("Cell")^(@)=(E_("ox")^(@))+(E_("red")^(@))_("cathode")`
`" "=0.4+0.34`
`" "=0.74V`.
emf is +ve, so `DeltaG` is (-)ve, the reaction is feasible.