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Hydrogen peroxide \left(\mathrm{H}_2 \mathrm{O}_2\right) acts as both a reducing agent and an oxidizing agent. Which of the following reactions represents its role as a reducing agent?

Option: 1

\mathrm{H}_2 \mathrm{O}_2+2 \mathrm{H}^++2 \mathrm{e}^{-} \rightarrow 2 \mathrm{H}_2 \mathrm{O}


Option: 2

2 \mathrm{KMnO}_4+5 \mathrm{H}_2 \mathrm{O}_2+3 \mathrm{H}_2 \mathrm{SO}_4 \rightarrow \mathrm{K}_2 \mathrm{SO}_4+5 \mathrm{O}_2+2 \mathrm{MnSO}_4+8 \mathrm{H}_2 \mathrm{O}


Option: 3

\mathrm{H}_2 \mathrm{O}_2 \rightarrow \mathrm{O}_2+2 \mathrm{H}^{+}


Option: 4

None of the above


Answers (1)

In this reaction, hydrogen peroxide \left(\mathrm{H}_2 \mathrm{O}_2\right) is acting as a reducing agent as it causes the oxidation of the oxygen in \mathrm{H}_2 \mathrm{O}_2 to form \mathrm{O}_2  in the 0 oxidation state.

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Kshitij

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