Question

Identify the correct statements regarding the following reaction:

$Fe\left(s\right)+O_2\left(g\right)\to F{e}_2{O}_3\left(g\right)$

• A. Iron undergoes oxidation
• B. Iron undergoes reduction
• C. Oxygen undergoes oxidation
• D. Oxygen undergoes reduction

Answer 1

Answer: (A), (D)

The correct options are
A

Iron undergoes oxidation

D

Oxygen undergoes reduction

In the reaction,

$Fe\left(s\right)+O_2\left(g\right)\to F{e}_2{O}_3\left(g\right)$

Left side has $Fe$ and $O_2$ has oxidation number 0 since they are stable elements.

We know that the oxidation number of oxygen is -2 in compounds.

Since the compound $F{e}_2{O}_3$ is a stable compound, the sum of the oxidation number of its element is zero.

From that we get, the oxidation number of Fe is +3.

Since the oxidation number of iron increased from 0 to +3 $\Rightarrow$ Iron undergoes oxidation.

Similarly, the oxidation number of oxygen decreased from 0 to -2 $\Rightarrow$ Oxygen undergoes reduction.