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In which of the following reactions, $\mathrm{H}_{2} \mathrm{O}_{2}$ is acting as a reducing agent?
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$\mathrm{Ag}_{2} \mathrm{O}+\mathrm{H}_{2} \mathrm{O}_{2} \rightarrow 2 \mathrm{Ag}+\mathrm{H}_{2} \mathrm{O}+\mathrm{O}_{2}$
$\mathrm{SO}_{2}$ changes to $\mathrm{H}_{2} \mathrm{SO}_{4}$ (O.N. changes from +4 to +6 oxidation $)$ $2 \mathrm{KI} \rightarrow \mathrm{I}_{2}(\mathrm{O} . \mathrm{S} .$ changes from -1 to 0
oxidation) $\mathrm{PbS} \rightarrow \mathrm{PbSO}_{4}(\mathrm{O} . \mathrm{S}$. changes from -2 to +6
oxidation) $\mathrm{Ag}_{2} \mathrm{O} \rightarrow 2 \mathrm{Ag}(\mathrm{O} . \mathrm{S} .$ changes from +1 to 0
reduction)
oxidation) $\mathrm{PbS} \rightarrow \mathrm{PbSO}_{4}(\mathrm{O} . \mathrm{S}$. changes from -2 to +6
oxidation) $\mathrm{Ag}_{2} \mathrm{O} \rightarrow 2 \mathrm{Ag}(\mathrm{O} . \mathrm{S} .$ changes from +1 to 0
reduction)
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