Question

According to the ideal gas law, a 10.08 mol sample of krypton gas in a 0.8488 L container at 496.7 K should exert a pressure of 484.0 atm. By what percent does the pressure calculated using the van der Waals' equation differ from the ideal pressure? For Kr gas, a = 2.318 L²atm/mol² and b = 3.978×10^-2 L/mol.

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Hint: % difference = 100 × (P _ideal - P_{van der Waals}) / P _ideal