The following reactions show the H2O2 behaviour in A and B reactions as (1) PbS(. s .)+4H2O2 (a q) arrow PbSO4 (s)+4H2O(l) (2) HOCl+H2O2 arrow H3O++Cl-+O2

Question

The following reactions show the H2O2 behaviour in A and B reactions as (1) PbS(. s .)+4H2O2 (a q) arrow PbSO4 (s)+4H2O(l) (2) HOCl+H2O2 arrow H3O++Cl-+O2 (A) oxidising in acidic medium and reducing in basic medium (B) reducing in acidic medium and oxidising in basic medium (C) oxidising in acidic medium and reducing in acidic medium (D) reducing in acidic medium and oxidising in acidic medium

Tardigrade Admin · Accepted Answer

Hydrogen peroxide oxidise lead sulphide to lead sulphate and itself gets reduced. Thus,

H_{2} O_{2}

acts as an oxidising agent in acidic medium.
Hydrogen peroxide reduces hypochlorous acid to chloride ion in acidic medium and itself gets oxidised.
Thus,

H_{2} O_{2}

acts as a reducing agent in acidic medium.

Q. The following reactions show the H2​O2​ behaviour in A and B reactions as (1) PbS(s)​+4H2​O2(aq)​→PbSO4(s)​+4H2​O(l)​ (2) HOCl+H2​O2​→H3​O++Cl−+O2​

oxidising in acidic medium and reducing in basic medium

reducing in acidic medium and oxidising in basic medium

oxidising in acidic medium and reducing in acidic medium

reducing in acidic medium and oxidising in acidic medium

Q. The following reactions show the $H_{2} O_{2}$ behaviour in A and B reactions as
(1) $P b S_{(s)} + 4 H_{2} O_{2 (a q)} \to P b S O_{4 (s)} + 4 H_{2} O_{(l)}$
(2) $H OCl + H_{2} O_{2} \to H_{3} O^{+} + C l^{-} + O_{2}$