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

Answer

C

Explanation

Since the reduction potential of `Fe^(3+) | Fe^(2+)` is greater than that of `I_(2) | I^(-) , Fe^(3+)` will be reduced and `I^(-)` will be oxidised .