In the reaction,4Fe + 3O_2 to 4Fe^{3+} + 6O^{ | vedclass

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(D) In the given reaction: $4Fe^{0} + 3O_2^{0} 	o 4Fe^{3+} + 6O^{2-}$.$Fe$ is oxidized from $0$ to $+3$ state,so it acts as a reducing agent.$O_2$ is

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$D$. Metallic iron is reduced to $Fe^{3+}$

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(D) In the given reaction: $4Fe^{0} + 3O_2^{0} 	o 4Fe^{3+} + 6O^{2-}$.$Fe$ is oxidized from $0$ to $+3$ state,so it acts as a reducing agent.$O_2$ is reduced from $0$ to $-2$ state,so it acts as an oxidizing agent.Since both oxidation and reduction occur,it is a redox reaction.Statement $D$ is incorrect because metallic iron is oxidized to $Fe^{3+}$,not reduced.

In the reaction,$4Fe + 3O_2 \to 4Fe^{3+} + 6O^{2-}$,which of the following statements is incorrect?

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