Question
what is the molar mass of a gaseous organic compound with a density of 3.38 g/L at 40oC and a pressure of 1.97 atm?
I got 4.41M, is this correct?
I got 4.41M, is this correct?
Answers
righteous dude
Start with the ideal gas law, and turn it into your desired answer.
PV=nRT
PV=(g/M)RT-------M being molar mass, that is why g/M= amount of moles
MPV=gRT
M=(gRT)/ (PV)
Plug in all the values.
M= (3.38g x 0.0821 L atm x 313 K) / (1.97 atm x 1 L K) = 44 g
PV=nRT
PV=(g/M)RT-------M being molar mass, that is why g/M= amount of moles
MPV=gRT
M=(gRT)/ (PV)
Plug in all the values.
M= (3.38g x 0.0821 L atm x 313 K) / (1.97 atm x 1 L K) = 44 g