Question
Here is the question:
A sample of an unknown volatile liquid was injected into a Dumas flask (mflask=27.0928g. Vflask=.104L) and heated until no visible traces of the liquid could be found. The flask and its contents were then rapidly cooled and reweighed (mflask+vapor=27.4593g) The atmospheric pressure and temperature during the experiment were 0.976 atm and 18.0 °C, respectively. The unknown volatile liquid's molecular mass was __________.
I have not got any concrete homework done on this outside of guessing and checking can someone set up this equation for me or explain how this can be done?
A sample of an unknown volatile liquid was injected into a Dumas flask (mflask=27.0928g. Vflask=.104L) and heated until no visible traces of the liquid could be found. The flask and its contents were then rapidly cooled and reweighed (mflask+vapor=27.4593g) The atmospheric pressure and temperature during the experiment were 0.976 atm and 18.0 °C, respectively. The unknown volatile liquid's molecular mass was __________.
I have not got any concrete homework done on this outside of guessing and checking can someone set up this equation for me or explain how this can be done?
Answers
Use n = PV/RT to get the number of moles in sample used.
Divide the grams of sample used by the number of moles to get the grams/mole which is the same as the molar mass. That is numerically the same as the molar mass.
Divide the grams of sample used by the number of moles to get the grams/mole which is the same as the molar mass. That is numerically the same as the molar mass.
Thank you that was exactly what I was looking for.