# Iron metal reacts with oxygen to produce iron (lll) oxide. If you have 12.0 moles of iron for a complete reaction, what do you need?

Feb 5, 2017

$2 F e \left(s\right) + \frac{3}{2} {O}_{2} \left(g\right) \rightarrow F {e}_{2} {O}_{3} \left(s\right)$

#### Explanation:

We need a stoichiometric equation:

$2 F e \left(s\right) + \frac{3}{2} {O}_{2} \left(g\right) \rightarrow F {e}_{2} {O}_{3} \left(s\right)$

And thus if $12.0 \cdot m o l$ of metal oxidize, then CLEARLY, by the given stoichiometry, $18.0 \cdot m o l$ of dioxygen gas are required.

What masses of gas and metal are required for the given reaction?