Question

What is the mass of butane needed to occupy a volume of 22.4 L at STP.

Answer 1

Using the ideal gas law, we can assume that

\[\frac{ PV }{RT}=n \] where n = number of moles of butane

You can do a simple dimensional analysis to get the mass of butane. Simply multiply the number of moles by the molar mass of butane. The answer would be in grams.

Answer 2

22.4L at STP is a special number when it comes to gases.