What is the molar mass of 81.50g of gas exerting a pressure of 1.75atm on the walls of a 4.92L container at 307K?
2 answers:
M = 81.50g, mm = m/n
n = ???
PV = nRT --> n = PV/RT
n = (1.75)(4.92)/(.0821)(307)
n = 8.61/25.20 = .342
--> mm = m/n = 81.5/.342 = 238.58
Answer: Molar mass of gas is 238.6 g/mol
Explanation:
Using ideal gas equation:
PV = nRT
P= pressure = 1.75 atm
V= volume = 4.92 L
n = no of moles =
R= gas constant =0.0821 Latm\molK
T = temperature = 307 K
R= gas constant = 8.314 J/Kmol
T= temperature = 190.7 K
M= molecular mass of gas = ?g/mol


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