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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

`DeltaG^(@) = -nFE^(@)`
`=-2 xx 96500 xx 0.236` J
`=-45548 J = -45.548 kJ`
`K = "Antilog" ([nE^(@)])/([0.059]) = "Antilog" (2 xx 0.2336)/0.059 = 10^(8)`
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