Question

consider the following reaction and identify the substance that is being oxidized.
4 fe(s) + 3 o₂(g) → 2 fe₂o₃(s)
o₂(g)
o in fe₂o₃(s)
fe(s)
fe in fe₂o₃(s)

Explanation:

Step1: Determine oxidation states

Oxidation state of \(Fe\) in \(Fe(s)\) is \(0\) (element in free state). In \(Fe_2O_3\), let oxidation state of \(Fe\) be \(x\). For \(Fe_2O_3\), using rule that sum of oxidation states is zero (\(2x+3\times(- 2)=0\), so \(x = +3\)). Oxidation state of \(O\) in \(O_2(g)\) is \(0\), in \(Fe_2O_3\) it is \(-2\).

Step2: Identify oxidation

Substance being oxidized is the one that loses electrons (oxidation state increases). \(Fe\) goes from \(0\) (in \(Fe(s)\)) to \(+3\) (in \(Fe_2O_3\)). \(O_2\) is reduced (oxidation state of \(O\) decreases from \(0\) to \(-2\)). \(O\) in \(Fe_2O_3\) and \(Fe\) in \(Fe_2O_3\) are products, not reactants being oxidized.

Answer:

\(\text{Fe}(s)\)