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

User Reema
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2 Answers

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Electrons are exchanged.

hope i helped

can i have branest
User Anthony Budd
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Answer: Because electrons are getting transferred from iron to oxygen.

Step-by-step 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:
(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

User Rob Kovacs
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