A solution contains Fe2+, Fe3+ and I ions. This solution was treated with iodine at 35C. E for Fe3+/Fe2+ is +0.77 V and E for I2/2I = 0.536 V.The favorable redox reaction is:
(1) I− will be oxidized to I2
(2) Fe2+ will be reduced to Fe3+
(3) I2 will be reduced to I−
(4) there will be no redox reaction takes place
Please explain
The explanation for the correct option
Option(1)I− is oxidized to I2
E0cell=E0cathode−E0anode
=(0.77−0.536)V
=0.234V
The possible redox reaction is:
Fe3++2I−⟶I2+Fe2+
That is I− is oxidized to I2 and Fe3+ is reduced to Fe2+
Hence, Option(1) I− is oxidized to I2 is correct