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If E(Fe^(2+))^(@)//Fe = -0.441 V and E...

If `E_(Fe^(2+))^(@)//Fe = -0.441 V`
and `E_(Fe^(3+))^(@)//Fe^(2+) = 0.771 V`
The standard `EMF` of the reaction
`Fe+2Fe^(3+) rarr 3Fe^(2+)`
will be:

A

1.212 V

B

0.111 V

C

0.330 V

D

1.653 V

Text Solution

Verified by Experts

The correct Answer is:
A
For the cell reaction `Fe+ 2Fe^(3+) rarr 2Fe^(2+)`
anode: `Fe_((s)) rarr Fe_((aq))^(2+)+ 2e^(-)`
cathode: `2Fe_((aq))^(3+)+ 2e^(-) rarr 2Fe_((aq))^(2+)`
`E_("cell")^(@)= E_("cathode")^(@)- E_("anode")^(@)`
`=0.771- (-0.441)`
`E_("cell")^(@)= 1.212V`
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