Question

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

• A. $Fe^{2+}$ will be oxidized to $ Fe^{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)

$2Fe^{=3} + 2I^- \rightarrow I_2 + 2Fe^{=2}$