(B) The given reaction is $4Fe + 3O_2 \to 4Fe^{3+} + 6O^{2-}$.In this reaction,the oxidation state of $Fe$ increases from $0$ to $+3$,which means $Fe$

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

(B) The given reaction is $4Fe + 3O_2 \to 4Fe^{3+} + 6O^{2-}$.In this reaction,the oxidation state of $Fe$ increases from $0$ to $+3$,which means $Fe$ is oxidised.Since $Fe$ is oxidised,it acts as a reducing agent.Conversely,the oxidation state of $O$ decreases from $0$ to $-2$,meaning $O_2$ is reduced.Statement $B$ is incorrect because metallic iron is oxidised to $Fe^{3+}$,not reduced.

Class 11 Chemistry Redox Reactions Mix Examples-Redox Reactions

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The following reaction describes the rusting of iron:
$4Fe + 3O_2 \to 4Fe^{3+} + 6O^{2-}$
Which one of the following statements is incorrect?

AIIMS 1998 All AIIMS

A
This is an example of a redox reaction
B
Metallic iron is reduced to $Fe^{3+}$
C
$Fe^{3+}$ is an oxidising agent
D
Metallic iron is a reducing agent

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Mix Examples-Redox Reactions

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The following reaction describes the rusting of iron:$4Fe + 3O_2 \to 4Fe^{3+} + 6O^{2-}$Which one of the following statements is incorrect?

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