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,
[tex]4Fe(s)+3O_2(g)\rightarrow 2Fe_2O_3(s)[/tex]
Half reactions of oxidation and reduction are :
Oxidation : [tex]Fe(s)\rightarrow Fe^{3+}+3e^-[/tex]
Reduction : [tex]\frac{1}{2}O_2+2e^-\rightarrow O^{2-}[/tex]
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.
