Question

Why is rusted iron an example of an oxidation-reduction reaction

Answer 1

Electrons are exchanged.

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Answer 2

Answer: Because electrons are getting transferred from iron to oxygen.

Explanation:

Oxidation-reduction reaction or redox reaction is defined as the reaction in which oxidation and reduction reaction occur simultaneously.

Oxidation reaction is defined as the reaction in which a substance looses its electrons. The oxidation state of the substance is increasing.

Reduction reaction is defined as the reaction in which a substance gain electrons. The oxidation state of the substance gets reduced.

For the reaction of rusting of iron, the equation follows:

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

On reactant side:

Oxidation state of iron = 0

Oxidation state of Oxygen = 0

On product side:

Oxidation state of iron = +3

Oxidation state of Oxygen = -2

Half reactions of oxidation and reduction are:

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

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

As, oxidation state of iron is increasing from 0 to +3, so it is getting oxidized and undergoes oxidation reaction. And, oxidation state of oxygen is getting decreased from ) to -2, so it is getting reduced and is considered as a reduction reaction.

Here, electrons are getting transferred from iron to oxygen. Hence, rusted of iron is an example of a redox reaction