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Question
\[\ce{H2O2}\] is a better oxidising agent than water. Explain.
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Solution
\[\ce{H2O2}\] 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.
\[\ce{\underset{Reduction}{2Na} + \underset{Oxidant}{2H2O} -> 2NaOH + H2}\]
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