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The cell in which the following reaction...

The cell in which the following reaction occurs
`2Fe^(3+)(aq)+2I^(-)(aq)to2Fe^(2+)(aq)+I_(2)(aq)+I_(2)(s)` has `E_(cell)^(0)=0.236V` at 298 K.
Calculate the stadard gibbs energy and the equilibrium constant of the cell reaction.

Text Solution

Verified by Experts

`E_(cell)^(@) = 0.236 V`
`Delta G^(Theta) = - n FE^(Theta)`
n = 2 , F = 96500 C
`Delta G^(Theta) = -2 xx (96500 C) xx (0.236 V)`
`= -45548 J or =-45.55 kJ`
`Delta G^(Theta) = - 2.303 RT log K_(c)`
or , `log K_(c) = - (Delta G^(Theta))/(2.303 RT)`
`=- (-45.55)/(2.303 xx 8.314 xx 10^(-3) xx 298)`
`= 7.983`
`K_(c) ` = antilog (7.983) = `9.62 xx 10^(7)`
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