What is the molar mass of a pure gas if a 12.0 g sample of has a pressure of 1.1 atm at 250 C in a 2.00 L flask? (R = 0.0821 L atm/mol K)?

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n = PV/RT = (1.1)(2) / (0.08206)(273.16+250) = _____ mol

MM = 12/mol = 12(0.08206)(273.16+250) / (1.1)(2)
MM = 6(0.08206)(273.16+250) / (1.1) = ____ g/mol


Ideal gas law
PV = nRT
n = number of moles
R = gas constant = 0.08206 (atm∙L)/(mol∙K)
                   8.314 L∙kPa/mol∙K
                   0.08314 L∙bar/mol∙K
                   62.36 L∙torr/mol∙K
                   62.36 L∙mmHg/mol∙K
T = temperature in kelvins
P = absolute pressure in atm, kPa, bar, torr
V = volume in liters...Show more