# What mass of "ferric oxide" would result from oxidation of a 58.7*g iron metal. What mass of dioxygen is required?

Sep 28, 2017

Approx....$81 \cdot g$.....

#### Explanation:

$F {e}_{2} {O}_{3}$ has a molar mass of $159.69 \cdot g \cdot m o {l}^{-} 1$..

We work from a molar quantity with respect to iron of $\frac{58.7 \cdot g}{55.8 \cdot g \cdot m o {l}^{-} 1} = 1.05 \cdot m o l$, and thus with respect to oxygen, there are is $1.05 \cdot m o l \times \frac{3}{2} \times 16 \cdot g \cdot m o {l}^{-} 1 = 25.25 \cdot g$ mass.

And so we just sum the masses, i.e. 55.8*g+25.25*g=??*g