# A nitrogen gas occupies a volume of 500 ml at a pressure of 0.971 atm. What volume will the gas occupy at a pressure of 1.50 atm, assuming the temperature remains constant?

Dec 7, 2014

The answer is $324 m L$.

This is a simple application of Boyle's law

${P}_{1} {V}_{1} = {P}_{2} {V}_{2}$,

which states that a gas' pressure and volume are proportional to eachother. It can be derived from the combined gas law,
$P V = n R T$, by keeping $T$ constant.

So, we have ${V}_{2} = {P}_{1} / {P}_{2} \cdot {V}_{1} = \frac{0.971}{1.50} \cdot 500 m L = 324 m L$ -> pressure increases, volume decreases and vice versa.