Chemistry - Redox Reactions Question with Solution | TestHub

The balanced chemical equation is: $2{\mathrm{MnO}}_4^{-}+6{\mathrm{H}}^{+}+5{\mathrm{SO}}_3^{--}⟶2{\mathrm{Mn}}^{++}+5{\mathrm{SO}}_4^{--}+3{\mathrm{H}}_2\mathrm{O}$ From the equation it is clear that Moles of ${\mathrm{MnO}}_4^{-}$ require to oxidise 5 moles of ${\mathrm{SO}}_3^{--}$are 2 Moles of ${\mathrm{MnO}}_4^{-}$ require to oxidise 1 mole of ${\mathrm{SO}}_3^{--}$are $2/5$.