Which one of the following reactions represents the reducing...

Which one of the following reactions represents the reducing property of $\mathrm{H}_{2} \mathrm{O}_{2} ?$ (a) $2 \mathrm{NaI}+\mathrm{H}_{2} \mathrm{SO}_{4}+\mathrm{H}_{2} \mathrm{O}_{2} \rightarrow \mathrm{Na}_{2} \mathrm{SO}_{4}+\mathrm{I}_{2}+2 \mathrm{H}_{2} \mathrm{O}$ (b) $\mathrm{PbO}_{2}+\mathrm{H}_{2} \mathrm{O}_{2} \rightarrow \mathrm{PbO}+\mathrm{H}_{2} \mathrm{O}+\mathrm{O}_{2}$ (c) $2 \mathrm{KMnO}_{4}+3 \mathrm{H}_{2} \mathrm{SO}_{4}+5 \mathrm{H}_{2} \mathrm{O}_{2} \rightarrow \mathrm{K}_{2} \mathrm{SO}_{4}+8 \mathrm{H}_{2} \mathrm{O}$ $+5 \mathrm{O}_{2}+2 \mathrm{MnO}_{2}$ (d) $2 \mathrm{~K}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{2}+2 \mathrm{KOH}+\mathrm{H}_{2} \mathrm{O}_{2} \rightarrow 2 \mathrm{~K}_{4}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]$ $+2 \mathrm{H}_{2} \mathrm{O}+\mathrm{O}_{2}$

Which one of the following reactions represents the reducing property of $\mathrm{H}_{2} \mathrm{O}_{2} ?$
(a) $2 \mathrm{NaI}+\mathrm{H}_{2} \mathrm{SO}_{4}+\mathrm{H}_{2} \mathrm{O}_{2} \rightarrow \mathrm{Na}_{2} \mathrm{SO}_{4}+\mathrm{I}_{2}+2 \mathrm{H}_{2} \mathrm{O}$
(b) $\mathrm{PbO}_{2}+\mathrm{H}_{2} \mathrm{O}_{2} \rightarrow \mathrm{PbO}+\mathrm{H}_{2} \mathrm{O}+\mathrm{O}_{2}$
(c) $2 \mathrm{KMnO}_{4}+3 \mathrm{H}_{2} \mathrm{SO}_{4}+5 \mathrm{H}_{2} \mathrm{O}_{2} \rightarrow \mathrm{K}_{2} \mathrm{SO}_{4}+8 \mathrm{H}_{2} \mathrm{O}$
$+5 \mathrm{O}_{2}+2 \mathrm{MnO}_{2}$
(d) $2 \mathrm{~K}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{2}+2 \mathrm{KOH}+\mathrm{H}_{2} \mathrm{O}_{2} \rightarrow 2 \mathrm{~K}_{4}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]$
$+2 \mathrm{H}_{2} \mathrm{O}+\mathrm{O}_{2}$

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Key Concepts

Hydrogen Peroxide's Dual Redox Behavior

Hydrogen peroxide (H2O2) is a unique chemical species that can function both as an oxidizing agent and as a reducing agent. This dual redox ability means that, under different reaction conditions, it can either accept electrons from another substance or donate electrons to it. Understanding this behavior is key to analyzing reactions in which H2O2 participates.

Reducing Agent

A reducing agent is a compound that donates electrons in a chemical reaction, thereby reducing another species while being itself oxidized. In the context of hydrogen peroxide, when it acts as a reducing agent, it donates electrons to an oxidizing substrate, leading to a decrease in the oxidation state of that substrate and converting H2O2 into higher oxidation state products such as oxygen.

Redox Reactions

Redox reactions, short for oxidation-reduction reactions, involve the transfer of electrons between chemical species. One substance undergoes oxidation (loses electrons) and another undergoes reduction (gains electrons). This framework is essential for understanding the electron-donating (reducing) or electron-accepting (oxidizing) behaviors of compounds like hydrogen peroxide.

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