# Iron rusts when exposed to oxygen. Iron(II) is produced in the reaction. How many moles of oxygen oxide will react with 2.4 mol of iron in the rusting reaction?

$F e \left(s\right) + \frac{1}{2} {O}_{2} \rightarrow F e O \left(s\right)$
This is a very simplified representation of the oxidation of iron metal. But if there are $2.4 \cdot m o l$ of iron metal, it should react with $1.2 \cdot m o l$ of dioxygen gas to give $2.4 \cdot m o l$ of iron oxide, as per the stoichiometric equation.