Question

\[\ce{H2O2}\] is a better oxidising agent than water. Explain.

Answer 1

\[\ce{H2O2}\] is a better oxidizing agent than water. \[\ce{H2O2}\] acts as an oxidizing agent in acid as well as in alkaline medium.

\[\ce{H2O2 + 2H^{+} + 2e^{-} ->[Acid] 2H2O; E^Θ = 1.77 V}\]

\[\ce{H2O2 + OH^{-} + 2e^{-} ->[Alkaline] 3OH-; E^Θ = 0.88 V}\]

Oxidation state of oxygen changes from – 1 to – 2. Oxidising nature of \[\ce{H2O2}\] can be interpreted on account of possession of labile oxygen.

\[\ce{H2O2 -> H2O + O}\]

When water acts as an oxidizing agent, it is reduced to \[\ce{H2}\]. Water reacts with number of active metals whose electrode potential is less than – 0.83 V.

\[\ce{\underset{Reduction}{2Na} + \underset{Oxidant}{2H2O} -> 2NaOH + H2}\]