In the reaction 2 Fe2+(aq) + H2O2(aq) → 2 Fe3+(aq) + 2 OH−(aq), which species is the oxidizing agent?

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Multiple Choice

In the reaction 2 Fe2+(aq) + H2O2(aq) → 2 Fe3+(aq) + 2 OH−(aq), which species is the oxidizing agent?

Explanation:
In redox terms, the oxidizing agent is the species that gets reduced. Here, Fe2+ is oxidized to Fe3+ (it loses an electron), so Fe2+ acts as the reducing agent. Hydrogen peroxide, on the other hand, is reduced to hydroxide ions (oxygen goes from -1 in H2O2 to -2 in OH−, gaining electrons). Because H2O2 accepts electrons, it is the oxidizing agent. The two electrons released by the two Fe2+ ions balance the two electrons gained by H2O2, forming 2 OH−. The iron(III) and hydroxide aren’t the electron acceptors, so the oxidizing agent is hydrogen peroxide.

In redox terms, the oxidizing agent is the species that gets reduced. Here, Fe2+ is oxidized to Fe3+ (it loses an electron), so Fe2+ acts as the reducing agent. Hydrogen peroxide, on the other hand, is reduced to hydroxide ions (oxygen goes from -1 in H2O2 to -2 in OH−, gaining electrons). Because H2O2 accepts electrons, it is the oxidizing agent. The two electrons released by the two Fe2+ ions balance the two electrons gained by H2O2, forming 2 OH−. The iron(III) and hydroxide aren’t the electron acceptors, so the oxidizing agent is hydrogen peroxide.

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