For the reaction 4Fe + 3O_2 to 4Fe^{3+} + 6O^ | vedclass

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(D) In the reaction $4Fe + 3O_2 	o 4Fe^{3+} + 6O^{2-}$,the oxidation state of $Fe$ changes from $0$ to $+3$ (oxidation).The oxidation state of $O$ ch

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

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(D) In the reaction $4Fe + 3O_2 	o 4Fe^{3+} + 6O^{2-}$,the oxidation state of $Fe$ changes from $0$ to $+3$ (oxidation).The oxidation state of $O$ changes from $0$ to $-2$ (reduction).Since both oxidation and reduction occur,it is a redox reaction.$Fe$ acts as a reducing agent because it gets oxidized.$Fe^{3+}$ is the product of oxidation,not an oxidizing agent.Therefore,the statement that metallic iron is reduced to $Fe^{3+}$ is incorrect,as it is actually oxidized.

For the reaction $4Fe + 3O_2 \to 4Fe^{3+} + 6O^{2-}$,which of the following statements is incorrect?

Similar Questions

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