An unknown gas at 49.1 °C and 1.10 atm has a molar mass of 16.04 g/mol. Assuming ideal behavior, what is the density of the gas?

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Answer 1 · 2016-11-17T13:46:55

#PV=w/MxxRT#

#=>PM=w/VxxRT#

#=>PM=DxxRT#

#=>D=(PM)/(RT)#

Here

#D->"Density of the gas"#

#P->"Pressure of the gas"=1.1atm#

#M->"Molar mass of gas"=16.04" g/"mol"#

#T->"Temperature of the gas"=49.1+273=322.1K#

#R->"Ideal gas constant"=0.082Latmmol^-1K^-1#

So

#D=(PM)/(RT)#

#=>D=(1.1xx16.04)/(0.082xx322.1)g/L=0.67g/L#