Question

Which of the following equations depict the oxidising nature of \[\ce{H2O2}\]?

Options

• \[\ce{2MnO^{-}4 + 6H^{+} + 5H2O2 -> 2Mn^{2+} + 8H2O + 5O2}\]

• \[\ce{2Fe^{3+} + 2H^{+} + H2O2 -> 2Fe^{2+} + 2H2O + O2}\]

• \[\ce{2I^{-} + 2H^{+} + H2O2 -> I2 + 2H2O}\]

• \[\ce{KIO4 + H2O2 -> KIO3 + H2O + O2}\]

Answer 1

\[\ce{2I^{-} + 2H^{+} + H2O2 -> I2 + 2H2O}\]

Explanation:

\[\ce{2\overset{-1}{I^{-}} + 2\overset{+1}{H^{+}} + \overset{+1}{H2}\overset{-1}{O2} -> \overset{0}{I2} + 2\overset{+1}{H2}\overset{-2}{O}}\]

\[\ce{I-}\] ions are oxidized to \[\ce{I2}\] (increase in O.N. from –1 to 0), Hence, \[\ce{H2O2}\] acts as an oxidizing agent.