According to the ideal gas law, a 1.048 mol sample of xenon gas in a 1.042 L container at 273.4 K should exert a pressure of

Question

According to the ideal gas law, a 1.048 mol sample of xenon gas in a 1.042 L container at
273.4 K should exert a pressure of 22.56 atm. What is the percent difference between the
pressure calculated using the van der Waals' equation and the ideal pressure? For Xe gas, a =
4.194 L²atm/mol² and b=5.105x10-2 L/mol.

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