According to the ideal gas law, a 0.9575 mol sample of methane gas in a 1.064 L container at 273.0 K should exert a pressure of 20.16 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For CH4 gas, a = 2.253 L2atm/mol2 and b = 4.278×10-2 L/mol.
According to the ideal gas law, a 0.9575 mol sample of methane gas in a 1.064 L container at 273.0 K should exert a pressure of 20.16 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For CH4 gas, a = 2.253 L2atm/mol2 and b = 4.278×10-2 L/mol.
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter10: Solids, Liquids, And Phase Transitions
Section: Chapter Questions
Problem 6P
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