Question

If 1.00mol of argon is placed in a 0.500- container at 28.0 degree Celsius, what is the difference between the ideal pressure (as predicted by the ideal gas law) and the real pressure (as predicted by the van der Waals equation)?
For argon,a=1.345(L square. atm)/mol square and b=0.03219L/mol .

You know the ideal PV = nRT equation, and you know van der Waals equation. Plug and chug.

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