Answer
$4Fe (s) + 3O_{2} (g) → 2Fe_{2}O_{3}$
Oxidation numbers in reactants: Fe = 0, O2 = 0
Oxidation number in products: Fe = +3, O = -2
From above, we observe that oxygen is reduced (0 to -2), and Iron is oxidized (0 to +3)
Work Step by Step
$4Fe (s) + 3O_{2} (g) → 2Fe_{2}O_{3}$
Oxidation numbers in reactants: Fe = 0, O2 = 0
Oxidation number in products: Fe = +3, O = -2
From above, we observe that oxygen is reduced (0 to -2), and Iron is oxidized (0 to +3)
