Please help?

Question

If 1.00 mol of argon is placed in a 0.500-L container at 23.0 degrees C, 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^2 X atm)/mol^2 and b = 0.03219 L/mol

Answer 1

Ideal gas law: PV = nRT P = nRT/V

n=1.00 V=0.500L T=296K R=0.082 L-atm/K-mol

V = (1.0)(0.082)(296)/(0.500) = 48.5 atm

To get the real P, plug the values above into the van der Waals equation together with values for a and b.