Question

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?

Answer 1

The answer is `324 mL`.

This is a simple application of Boyle's law

`P_1V_1 = P_2V_2`,

which states that a gas' pressure and volume are proportional to eachother. It can be derived from the combined gas law,
`PV = nRT`, by keeping `T` constant.

So, we have `V_2 = P_1/P_2 * V_1 = 0.971/1.50 * 500 mL = 324 mL` -> pressure increases, volume decreases and vice versa.