Question

Which of the following equation depict the reducing nature of $H_{2}O_{2}?$

• A. $2MnO_{4}^{-}+6H^{+}+5H_{2}O_{2} \rightarrow 2Mn^{+ 2}+8H_{2}O+5O_{2}$
• B. $I_{2}+H_{2}O_{2}+2OH^{-} \rightarrow 2I^{-}+2H_{2}O+O_{2}$
• C. $Mn^{+ 2}+H_{2}O_{2} \rightarrow Mn^{+ 4}+2OH^{-}$
• D. $Pbs+4H_{2}O_{2} \rightarrow PbSO_{4}+4H_{2}O$

Answer 1

Answer: (B)

Reducing nature of $H_{2}O_{2}$ means it reduces other substance and itself gets oxidised by evolving $O_{2}$ .
In (a), $Mn^{+ 7}$ gets oxidised to $Mn^{+ 3}$ .
In (b), $I_{2}$ gets reduced to $I^{-}$ .
In (c), $Mn^{2 +}$ gets oxidised to $Mn^{4 +}$
In (d), $Pb^{+ 6}$ gets oxidised to $Pb^{2 +}$