A #0.5090g# mass of gas exerts a pressure of #746mmHg#, and occupies a volume of #0.1294L# at a temperature of #364*K#? What is its molecular mass?

Question

1470 views around the world

You can reuse this answer
Creative Commons License

Answer 1 · 2017-04-17T20:38:40

#"Molecular mass"<=120*g*mol^-1#

From the Ideal Gas Equation:

#n=(PV)/(RT)#

i.e. #"mass"/"molar mass"=(PV)/(RT)#

i.e. #"molar mass"=("mass"xxRT)/(PV)#

#=(0.5090*gxx0.0821*L*atm*K^-1*mol^-1xx364*K)/((746*mm*Hg)/(760*mm*Hg*atm^-1)xx0.1294*L)#

#??*g*mol^-1#

A #0.5090*g# mass of gas exerts a pressure of #746*mm*Hg#, and occupies a volume of #0.1294*L# at a temperature of #364*K#? What is its molecular mass?