Question

Find out the compounds that will disproportionate in their aqueous solution.

$\left(I\right)ClO_{4}^{-} \overset{+ 0.36 V}{ \rightarrow }ClO_{3}^{-} ⁡ \overset{+ 0.33 V}{ \rightarrow }ClO_{2}\overset{+ 0.66 V}{ \rightarrow }OCl^{-}\overset{+ 0.40 V}{ \rightarrow }\frac{1}{2}Cl_{2}\overset{+ 1.36 V}{ \rightarrow }Cl^{-}$

$\left(I I\right)MnO_{4}^{-} \overset{+ 0.56 V}{ \rightarrow }MnO_{4}^{2 -} ⁡ \overset{+ 2.22 V}{ \rightarrow }MnO_{2}\overset{+ 0.95 V}{ \rightarrow }Mn^{3 +}\overset{+ 1.55 V}{ \rightarrow }Mn^{2 +}\overset{- 0.19 V}{ \rightarrow }Mn$

(I)	(II)
$ClO_{2}, Cl_2$	$MnO^{2-}_{4}, Mn^{3+}$
$ClO^{-}_{3}, OCl^{-}$	$MnO_{2}, Mn^{2+}$
$OCl^{-}$ only	$MnO_{2}, Mn^{2+}$
$ClO^{-}_{3}$ only	$MnO_{2}$ only

• A. A
• B. B
• C. C
• D. D

Answer 1

Answer: (A)

If the reaction sequence is written in reduction order then if right side reduction potential is higher than left side reduction potential then that compound will disproportionate.