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The standard electrode potential of the ...

The standard electrode potential of the half cells are given below.
`ZnrarrZn^(2+)+2e^(-):E^(@)=0.76V`
`FerarrFe^(2+)+2e^(-):E^(@)=0.44V`
The emf of the cell
`Fe^(2+)+ZnrarrZn^(2+)+Fe` is

A

`-0.32V`

B

`+0.32V`

C

`+1.20V`

D

`-1.20V`

Text Solution

Verified by Experts

The correct Answer is:
B
The given electrode are oxidation potential so reduction potential are
`E_(Za)^(+2)//Zn=-0.76V`
`E_(Fe)^(@)//Fe=-0.44V`
then `E_("cell")^(@)=E_(c)^(@)-E_(a)^(@)`
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