Question

A solution contains $F{e}^{2+},F{e}^{3+}$ and $I^{-}$ ions. This solution was treated with iodine at $35^{\circ }C.E^{\circ }$ for $F{e}^{3+}/F{e}^{2+}$ is $+0.77V$ and $E^{\circ }$ for $I_2/2I^{-}=0.536V.$
The favourable redox reaction is-

• A. $F{e}^{2+}$ will be oxidized to $F{e}^{3+}$
• B. $I_2$ will be the reduced to $I^{-}$
• C. There will be no redox reaction
• D. $I^{-}$ will be oxidized to $I_2$

Answer 1

Answer: (D)

$2F{e}^{=3}+2I^{-}\to I_2+2F{e}^{=2}$