What is the density of methyl chloride gas, #CH_3Cl#, at STP?

1 Answer
May 17, 2016

Answer:

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 mass"/"Molar volume"#

= #50.49 / 22.4# = #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!