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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

0.62V

B

0.56V

C

1.12V

D

0.31V

Text Solution

Verified by Experts

The correct Answer is:
B
`Zn(s)+Sn^(2+)rarrZn^(2+)(aq)+Sn(s)`
`E_("cell")=E_("cell")^(@)-(0.059)/(n)"log"([Zn^(2+)])/([Sn^(2+)])`
`=[0.14-(-0.76)]-(0.059)/(2)"log"(0.1)/(0.001)`
`=+0.62-(0.059)/(2)"log"100=+0.56V`
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