JEE Main 2024 — Redox Reactions Question with Solution

A disproportionation reaction is a reaction in which the same element is simultaneously oxidized and reduced. In this type of reaction, a single substance gives two products, one is oxidized while the other is reduced.

${\mathrm{S}}_1:{\mathrm{S}}_8+12{\mathrm{OH}}^{⊝}\to 4{\mathrm{S}}^{2-}+2{\mathrm{S}}_2{\mathrm{O}}_3^{2-}+6{\mathrm{H}}_2\mathrm{O}$

${\mathrm{S}}_2:{\mathrm{ClO}}_4^{⊝}$ cannot undergo disproportionation reaction as chlorine is present in its highest oxidation state.

Hence, statement $\mathrm{I}$ is correct and $\mathrm{II}$ is incorrect.