# Question 6b172

We're asked to find the liters of ${\text{Cl}}_{2}$ occupied by $6.7$ ${\text{g Cl}}_{2}$.
What we can do here is calculate the number of moles of chlorine using the molar mass of ${\text{Cl}}_{2}$, $70.90 \text{g"/"mol}$:
$6.7$ cancel("g Cl"_2)((1"mol Cl"_2)/(70.90cancel("g Cl"_2))) = 0.0945 ${\text{mol Cl}}_{2}$
At standard temperature and pressure, one mole of any gas occupies a volume of $22.41$ $\text{L}$. (from Avogadro's law). We can use this fact to convert from moles to liters:
0.0945cancel("mol Cl"_2)((22.41"L Cl"_2)/(1cancel("mol Cl"_2))) = color(red)(2.1)# $\textcolor{red}{{\text{L Cl}}_{2}}$