$\mathrm{PbS}+4{\mathrm{H}}_2{\mathrm{O}}_2\to {\mathrm{PbSO}}_4+4{\mathrm{H}}_2\mathrm{O}$

In the above reaction lead sulphide oxidised to lead sulphate. Hence, hydrogen peroxide acts as oxidising agent.

$2{\mathrm{Fe}}^{2+}+{\mathrm{H}}_2{\mathrm{O}}_2\to 2{\mathrm{Fe}}^{3+}+2{\mathrm{OH}}^{-}$

In the above reaction ${\mathrm{Fe}}^{2+}$ oxidised to ${\mathrm{Fe}}^{3+}$. Hence, hydrogen peroxide acts as oxidising agent.

${\mathrm{Mn}}^{2+}+{\mathrm{H}}_2{\mathrm{O}}_2\to {\mathrm{Mn}}^{4+}+2{\mathrm{OH}}^{-}$

In the above reaction ${\mathrm{Mn}}^{2+}$ oxidised to ${\mathrm{Mn}}^{4+}$. Hence, hydrogen peroxide acts as oxidising agent.

$\mathrm{HOCl}+{\mathrm{H}}_2{\mathrm{O}}_2\to {\mathrm{H}}_3{\mathrm{O}}^{+}+{\mathrm{Cl}}^{-1}+{\mathrm{O}}_2$

In the above reaction ${\mathrm{Cl}}^{+1}$ reduced to ${\mathrm{Cl}}^{-}$, hence, hydrogen peroxide acts as a reducing agent.