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Calculate the cell e.m.f. and DeltaG for...

Calculate the cell e.m.f. and `DeltaG` for the cell reaction at 298K for the cell.
`Zn(s) | Zn^(2+) (0.0004M) ||Cd^(2+) (0.2M)|Cd(s)`
Given, `E_(Zn^(2+)//Zn)^(@) =- 0.763 V, E_(Cd^(+2)//Cd)^(@) = - 0.403 V` at `298K`.
`F = 96500 C mol^(-1)`.

A

`CdrarrCd^(2+)+2e^(-)`

B

`Zn^(2+)rarrZn-2e^(-)`

C

`Cd+Zn^(2+)rarrZn+Cd^(2+)`

D

`Zn+Cd^(2+)rarrZn^(2+)+Cd`.

Text Solution

Verified by Experts

The correct Answer is:
D
The two half cell reaction for the given cells are:
`Zn(s)rarrZn^(2+)+(aq)+2e^(-)`
`Cd^(2+)(aq)+2e^(-)rarrCd(s)`
New reaction:
`Zn(s)+Cd^(2+)(aq)rarrZn^(2+)(aq)+Cd(s)`
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