A solution contains `Fe^(2+), Fe^(3+)` and `T^(-)` ions. This solution was treated with iodine at `35^(@)C. E^(@)` for `Fe^(3+), Fe^(2+)` is `0.77 V` and `E^(@)` for `I_(2)//2I^(-)` = 0.536 V. The favourable redox reaction is:

Options

A. `I^(-)` will be oxidised to `I_(2)`
B. `Fe^(2+)` will be oxidised to `Fe^(3+)`
C. `I_(2)` will be reduced to `I^(-)`
D. There will be no redox reaction

Answer

A

Explanation

`E_(Fe^(3+)//Fe^(2+))^(@)= 0.77V`
`E_(l_(2)//l^(-))^(@)= 0.536V`
Reduction potential of `Fe^(3+)` is more than `l_(2)`. So `Fe^(3+)` will reduce to `Fe^(2+) and I^(-)` will oxidize to `I_(2)`.
`Fe^(3+) + I^(-) rarr Fe^(2+) + I_(2)`