`E^(@)` values for `Fe^(3+) + 3e rarr Fe` and `Fe^(2+) + 2 e rarr Fe` are - 0.036V and -0.44V respectively. Calculate the `E^(0)` and `DeltaG^(0)` for the cell reaction `Fe + 2 Fe^(3+) rarr 3Fe^(2+)` .

Explanation

Given
`Fe^(3+) + 3e^(-) rarrFe" "E^(@)= - 0.036V` .....(i)
`Fe^(2+) + 2e^(-) rarr Fe" "E^(@) = -0.44V` ......(2)
`Fe+ 2Fe^(2+)rarr 3Fe^(2+)" "E^(@) = 7, Delta G^(@) = 7 ` ....(3)
On applying operation
(Eq(1) `xx` 2 Eq(2) `xx` 3) = Eq (3)
`[ - 6 xx F xx ( - 0.036]-[ -6 xx F xx ( -0.44)] = - 6 xx F xx E^(@)`
`E^(@) = 0.4364V`
now `Delta G^(@) `for Eq (3) is `- 6 xx F xx 0.4364V`
`=-6 xx 96500Cxx0.4364V`
`= 252, 675.6 J = 2526kJ`