# How do we represent the oxidation of a 31.7*g mass of iron by chlorine gas? What mass of FeCl_3(s) results?

$F e \left(s\right) + \frac{3}{2} C {l}_{2} \left(g\right) \rightarrow F e C {l}_{3} \left(s\right)$
Moles of iron: $\frac{31.7 \cdot g}{55.85 \cdot g \cdot m o {l}^{-} 1}$ $=$ ??*mol
This molar quantity of iron requires $\frac{3}{2}$ molar equivalents of chlorine gas for complete reaction. What is oxidized, and what is reduced in the reaction? How do you know?