Which of the following equation depicts reducing nature of `H_(2)O_(2)`?

Options

A. `2[Fe(CN)_(6)]^(4-)+2H^(+)+H_(2)O_(2)rarr2[Fe(CN)_(6)]^(3-)+2H_(2)O`
B. `I_(2)+H_(2)O_(2)+2OH^(-)rarr 2I^(-)+2H_(2)O+O_(2)`
C. `Mn^(2+)+H_(2)O_(2)rarr Mn^(4+)+2OH^(-)`
D. `PbS+4H_(2)O_(2)rarr PbSO_(4)+4H_(2)O`

Answer

B

Explanation

Reducing nature of `H_(2)O_(2)` means it reduces other substance and itself gets oxidised. In such reactions `O_(2)` is evolved.
In (a), `Fe^(2+)` gets oxidised to `Fe^(3+)`.
In (b), `I_(2)` gets reduced to `I^(-)`.
In (c ), `Mn^(2+)` gets oxidised to `Mn^(4+)`
In (d), `PbS^((2-))` gets gets oxided to `overset((+6))(PbSO_(4))`.