How much iron metal can be prepared from an 100*kg mass of "ferric oxide", and excess carbon monoxide?

Sep 30, 2016

$F {e}_{2} {O}_{3} \left(s\right) + 3 C O \left(g\right) \rightarrow 2 F e \left(s\right) + 3 C {O}_{2} \left(g\right)$
Approx $70 \cdot k g$ of iron metal can be produced.
$\text{Moles of ferric oxide}$ $=$ $\frac{100 \cdot \cancel{k g} \times {10}^{3} \cdot \cancel{g} \cdot \cancel{k {g}^{-} 1}}{159.69 \cdot \cancel{g} \cdot m o {l}^{-} 1}$ $=$ $626.2 \cdot m o l$.
And clearly, from the stoichiometry of the reaction, $2 \times 626.2 \cdot \cancel{m o l} \times 55.85 \cdot \cancel{g} \cdot \cancel{m o {l}^{-} 1} \times {10}^{-} 3 k g \cdot \cancel{{g}^{-} 1}$ $=$ ??