If 1.00 molmol of argon is placed in a 0.500-LL container at 20.0 ∘C∘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(L2⋅atm)/mol2a=1.345(L2⋅atm) /mol2 and b=0.03219L/molb=0.03219L/mol .