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The single electrode reactions, Cd(s) to...

The single electrode reactions,
`Cd(s) to Cd^(2+) (0.1) + 2e^(-) , E ^@ = 0.4030`
`Cu^(2+) + 2e^(-) to Cu (s), E^@ = 0.337`
can be combined to give the cell reaction, `Cd(s) + Cu^(2+) to Cu (s)`
The emf of the cell is

A

0.74

B

0.1354

C

0.66

D

0.066

Text Solution

Verified by Experts

The correct Answer is:
A
`E_((Cd^(2+))//(Cd))^@ = 0.4030` and ` E_((Cu^(2+))//(Cu))^@= 0.337`
`therefore E_(cell)^@=E_(o x idation)^@ +E_(reduction)^@= 0.4030+0.337=0.740V`
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