# What molar quantity of carbon monoxide is required to reduce a 160*g mass of Fe_2O_3?

## We follow the stoichiometric equation... $F {e}_{2} {O}_{3} \left(s\right) + 3 C O \left(g\right) \stackrel{\Delta}{\rightarrow} 2 F e \left(s\right) + 3 C {O}_{2} \left(g\right)$

Oct 1, 2017

#### Answer:

Look at the stoichiometry of your equation....

#### Explanation:

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

And this explicitly tells me that heating $160 \cdot g$ $\text{ferric oxide}$ in the presence of $84 \cdot g$ $\text{carbon monoxide gas}$ results in the formation of $112 \cdot g$ of (molten) iron and $152 \cdot g$ of $\text{carbon dioxide gas}$. As is always observed in any chemical reaction, MASS is conserved. Is it conserved here?

So you gots $2.4 \cdot m o l$ of iron....$3 \times 2.4 \cdot m o l$ of carbon monoxide were necessary, and clearly $1.2 \cdot m o l$ of $\text{ferric oxide}$ were required. You will have to fill in the appropriate masses. Can you do so?