Chemistry - Redox Reactions Question with Solution | TestHub

As in$\mathrm{H}\mathrm{N}{\mathrm{O}}_2$,$\text{N}$is in$\text{+3}$oxidation state but nitrogen can have oxidation states from$-\text{3}$to$+5$so it is in between the maximum and minimum oxidation state hence it can either get reduced or oxidized, depending on the conditions. It means it can act both as an oxidizing and a reducing agent. It can work both as oxidising as well as reducing agent.
(I) As an oxidising agent:
$\mathrm{H}\mathrm{N}{\mathrm{O}}_2+2{\mathrm{H}}^{+}+{\mathrm{e}}^{-}\to \mathrm{N}\mathrm{O}+{\mathrm{H}}_2\mathrm{O}$
(II) As reducing agent:
$\mathrm{H}\mathrm{N}{\mathrm{O}}_2+{\mathrm{H}}_2\mathrm{O}\to \mathrm{N}{\mathrm{O}}_3^{-}+3{\mathrm{H}}^{+}+2{\mathrm{e}}^{-}$