An example of a disproportionation reaction is

Disproportionation reaction: In this type of reaction, same elemental species gets oxidised as well as reduced.

\overset{+ 1}{\text{Na}}\overset{- 1}{\text{Br}} + \overset{0}{{\text{Cl}_{2}} \to 2\overset{+ 1}{\text{Na}}\overset{- 1}{\text{Cl}} + \overset{0}{{\text{Br}_{2}} -not disproportionate,

\left[2K\overset{+ 7}{Mn}{O}_{4} \to {K}_{2}\overset{+ 6}{Mn}{O}_{4} + \overset{+ 4}{Mn}{O}_{2} + {O}_{2}\right] -$not disproportionate,</p><p>$2\overset{+ 7}{Mn}{O}_{4}^{-} + 10{J}^{-} + 16{H}^{+} \to 2\overset{+ 2}{Mn} + S{I}_{2} + 8{H}_{2}O -not disproportionate

-It is disproportionate.