Question

Ferric oxide reacts with aluminum to produce aluminum oxide and iron. The balanced chemical equation for the given reaction is:

${\mathrm{Fe}}_2{\mathrm{O}}_3+2\mathrm{AI}\to {\mathrm{Al}}_2{\mathrm{O}}_3+2\mathrm{Fe}$

Which of the following substances is oxidized in the given reaction?

• A. ${\mathrm{Al}}_2{\mathrm{O}}_3$
• B. ${\mathrm{Fe}}_2{\mathrm{O}}_3$
• C. $\mathrm{Al}$
• D. $\mathrm{Fe}$

Answer 1

The correct option is C

$\mathrm{Al}$

The explanation for the correct option

(C) $\mathrm{Al}$

Oxidation

The addition of oxygen$\left(\mathrm{O}\right)$ atoms or the removal of hydrogen$\left(\mathrm{H}\right)$ atoms from an element is known as oxidation.

${\mathrm{Fe}}_2{\mathrm{O}}_3+2\mathrm{AI}\to {\mathrm{Al}}_2{\mathrm{O}}_3+2\mathrm{Fe}$

In this reaction, aluminum$\left(\mathrm{Al}\right)$ gains oxygen and hence is oxidized.

The explanation for the incorrect options

(A) ${\mathrm{Al}}_2{\mathrm{O}}_3$

${\mathrm{Al}}_2{\mathrm{O}}_3$ is the end product hence the concept of oxidation or reduction becomes irrelevant.

(B) ${\mathrm{Fe}}_2{\mathrm{O}}_3$

${\mathrm{Fe}}_2{\mathrm{O}}_3$ as a whole is not oxidized or reduced just $\mathrm{Fe}$ is reduced.

(D) $\mathrm{Fe}$

$\mathrm{Fe}$ is reduced in this reaction.

Therefore, in the given reaction only$\left(\mathrm{Al}\right)$ is oxidized and hence, option (C) is correct.