Find out the compounds that will disproportionate in their aqueous solution. I ClO 4 - ⁡ → + 0.36 V ClO 3 - ⁡ → + 0.33 V C l O 2 → + 0.66 V O C l - → + 0.40 V 1 2 C l 2 → + 1.36 V C l - I I MnO 4 - ⁡

Question

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

$(I) {ClO}_{4}^{-} \overset{+ 0.36 V}{\to} {ClO}_{3}^{-} \overset{+ 0.33 V}{\to} C l O_{2} \overset{+ 0.66 V}{\to} O C l^{-} \overset{+ 0.40 V}{\to} \frac{1}{2} C l_{2} \overset{+ 1.36 V}{\to} C l^{-}$

$(I I) {MnO}_{4}^{-} \overset{+ 0.56 V}{\to} {MnO}_{4}^{2 -} \overset{+ 2.22 V}{\to} M n O_{2} \overset{+ 0.95 V}{\to} M n^{3 +} \overset{+ 1.55 V}{\to} M n^{2 +} \overset{- 0.19 V}{\to} M n$

TestHub · Accepted Answer

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.

(I)	(II)
${C l O}_{2}, {C l}_{2}$	$M n O_{4}^{2 -}, M n^{3 +}$

(I)	(II)
$C l O_{3}^{-}, O C l^{-}$	$M n O_{2}, M n^{2 +}$

(I)	(II)
$O C l^{-}$ only	$M n O_{2}, M n^{2 +}$

(I)	(II)
$C l O_{3}^{-}$ only	${M n O}_{2}$ only

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