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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+)|Cdu are 0.34V and -0.40 volts respectively. Predict the feasibility of the cell reaction. |
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Answer» Solution :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. |
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