# What volume will 500 mL of gas at 20°C and a pressure of 420 mm Hg occupy if the temperature is reduced to -80°C and the pressure is increased to 650 mm Hg?

Jul 27, 2018

Approx. $200 \cdot m L$...…...

#### Explanation:

The combined gas law holds that $\frac{{P}_{1} {V}_{1}}{T} _ 1 = \frac{{P}_{2} {V}_{2}}{T} _ 2$...we use terms of absolute temperature...we also KNOW that $1 \cdot a t m$ will support a column of mercury that is $760 \cdot m m$ high...

And so we solve for...${V}_{2} = \frac{{P}_{1} {V}_{1}}{T} _ 1 \times {T}_{2} / {P}_{2}$

$= \frac{\frac{420 \cdot m m \cdot H g}{760 \cdot m m \cdot a t {m}^{-} 1} \cdot 500 \cdot m L}{293.15 \cdot K} \times \frac{193.15 \cdot K}{\frac{650 \cdot m m \cdot H g}{760 \cdot m m \cdot a t {m}^{-} 1}}$

=??*mL