What is the density of methyl chloride gas, CH3Cl, at STP?

1 Answer
May 17, 2016

If you assume it behaves as an ideal gas, then 0.00225 g/ml at STP.

Explanation:

If you assume that it behaves as an ideal gas then it's simple enough, and will give you a fair estimate:

One mole of an ideal gas at STP occupies 22.4 L. Molar mass of methyl chloride is 50.49 g/mol.

Then simply divide the molar mass by the molar volume which gives you a density in g/l.

i.e. Density=Molar massMolar volume

= 50.4922.4 = 2.25 g/L = 0.00225 g/ml.

If you want a more accurate figure you will need to use the full form of the gas equation incorporating a virial expansion, but that's a lot more complicated!