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The standard electrode potentials E^(@) ...

The standard electrode potentials `E^(@)` for the half cell reactions are as :
`ZntoZn^(2+)+2e^(-),E^(@)=0.76V`
`FetoFe^(2+)+2e^(-),E^(@)=041V`
The EMF of the cell reaction `Fe^(2+)+ZntoZn^(2+)+Fe` is :

A

`-1.20V`

B

`+1.20V`

C

`+0.32V`

D

`-0.32V`

Text Solution

Verified by Experts

The correct Answer is:
C
Given cell reaction is
`Zn+Fe^(2+)toZn^(2+)+Fe`
In the above reaction Zn is being oxidised and `Fe^(2+)` is beign reduced, thus the cell can be represented as
`Zn|Zn^(2+)||Fe^(2+)|Fe`
`E_("cell")=E_("Right")-E_("Left")=E_(Fe^(2+)|Fe)-E_(Zn^(2+)+Zn)`
`=(-0.44)-(-0.76)`
`=0.76-0.44=0.32` volts
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