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What is the value of E^(@) cell in the f...

What is the value of `E^(@)` cell in the following reaction?
`Cr|Cr^(3+) (0.1 M)||Fe^(2+) (0.01 M)|Fe`
Given, `E_(Cr^(3+)//Cr)^(@)=-0.74 V, E_(Fe^(2+)//Fe)^(@)=-0.44 V`

A

`+ 0.2606 V`

B

`0.5212 V`

C

`+ 01303 V`

D

`-0.2606 V`

Text Solution

Verified by Experts

The correct Answer is:
A
The cell reaction is
`2Cr+3Fe^(2+) rarr 2Cr^(3+)+3Fe(n=6)`
from Nernst equation,
`E_("cell")=E_("cell")^(@)-0.059/n "log" ([Cr^(3+)]^(2))/([Fe^(2+)]^(3))`
`=[-0.44+0.74]- 0.059/6 xx"log" ((0.1)^(2))/((0.01)^(3))`
`=+0.2606 V`
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