Question

Why is rusted iron an example of an oxidation–reduction reaction? electrons are exchanged?

Answer 1

Electrons are exchanged, yes.

Answer 2

Answer : The rusted iron is an example of an oxidation–reduction reaction because electrons are exchanged.

Explanation :

Iron rusting : It is a chemical process in which the an iron nail react with water and oxygen to give iron oxide as a product. Rusting of iron is an oxidation-reduction reaction in which iron losses electrons to oxygen atom.

Oxidation-reduction reaction : It is a reaction in which oxidation and reduction reaction occur simultaneously.

Oxidation reaction : It is the reaction in which a substance looses its electrons. In this oxidation state increases.

Reduction reaction : It is the reaction in which a substance gains electrons. In this oxidation state decreases.

The balanced chemical reaction for rusting of irons is,

$4Fe(s)+3O_2(g)\rightarrow 2Fe_2O_3(s)$

Half reactions of oxidation and reduction are :

Oxidation : $Fe(s)\rightarrow Fe^{3+}+3e^-$

Reduction : $\frac{1}{2}O_2+2e^-\rightarrow O^{2-}$

From this reaction we conclude that the electrons are getting transferred from iron to oxygen.

Hence, the rusted iron is an example of an oxidation–reduction reaction because electrons are exchanged.