# Chlorine gas occupies a volume of 1.20 liters at 720 torr pressure. What volume will it occupy at 1 atm pressure? Assume that temperature remains the same.

Jun 11, 2018

Well, $\text{1 Torr = 1 mm Hg}$...

#### Explanation:

And $1 \cdot a t m \equiv 760 \cdot m m \cdot H g$ or rather $1 \cdot a t m$ will support a column of mercury that is $760 \cdot m m$ high...and I truly hope you have seen such a column because the health and safety commissars at my establishment have declared the mercury column counter-revolutionary.

And we simply apply old $\text{Boyles' Law..}$ ${P}_{1} {V}_{1} = {P}_{2} {V}_{2}$

We solve for ${V}_{2} = \frac{{P}_{1} {V}_{1}}{P} _ 2 = \frac{1.20 \cdot L \times \frac{720 \cdot m m \cdot H g}{760 \cdot m m \cdot H g \cdot a t {m}^{-} 1}}{\frac{760 \cdot m m \cdot H g}{760 \cdot m m \cdot H g \cdot a t {m}^{-} 1}}$

$\equiv 1.14 \cdot L$...the VOLUME has reduced because we INCREASED the PRESSURE....