In the reaction; $4 F e + 3 O_{2} ⇌ 4 F e^{3 +} + 6 O^{2 -}$ .

Which of the following statements is incorrect?

It is a redox reaction

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Metallic iron is a reducing agent

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F e^{3 +}

is an oxidising agent

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Metallic iron is reduced to

F e^{3 +}

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Solution

The correct option is A Metallic iron is reduced to $F e^{3 +}$
$4 F e + 3 O_{2} ⇋ 4 F e^{3 +} + 6 O^{2 -}$

As it is clearly evident from the reaction that metallic iron is oxidised to $F e^{3 +}$ . So, option D is incorrect.

Also, since both oxidation and reduction processes are taking place simultaneously so it is a redox reaction.

$∵$ Metallic iron is undergoing oxidation, therefore it is a reducing agent. Also, $F e^{3 +}$ is an oxidizing agent as it is in its highest oxidation state.

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4 F e + 3 O_{2} \to 4 F e^{3 +} + 6 O^{2 -}

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