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

Answer

D

Explanation

We arc given
`Fe^(3+)(aq.)+e^(-) rarr Fe^(2+)(aq.)," "E^(@) = +0.77 V`
`I^(s)+2e^(-) rarr 2I^(-)(aq.)," "E^(@) = +0.536 V`
The higher the reducation potential, the greater the finding to get reduced. Thus, when the solution containing `Fe^(2+), Fe^(3+)` and `I^(-)` ions is treated with iodine, then `Fe^(3+)` ions will be reduced while `l^(-)` ions will be oxidized to `I_(2)`.