# How many moles of carbon dioxide are recovered after reduction of a 1000*g mass of Fe_2O_3 by CO?

$F {e}_{2} {O}_{3} \left(s\right) + 3 C O \left(g\right) \rightarrow 2 F e \left(s\right) + 3 C {O}_{2} \left(g\right)$
Moles of haematite: $\frac{1000 \cdot g}{159.69 \cdot g \cdot m o {l}^{-} 1}$ $=$ ?? $\text{moles}$
Given the stoichiometry of the equation, it is a fact that each mole of $F {e}_{2} {O}_{3}$ requires $3$ $\text{mol}$ carbon monoxide gas for reduction of the oxide. And of course the oxidation product is carbon dioxide gas, $3$ $m o l$ for every $2$ mole of iron that is reduced. So all I have to do is calculate the number of moles of oxide, and multiply this figure by 3, to give the number of moles of carbon dioxide product.