Using the van der Waals equation, find the pressure exerted by 1 mole of Ar gas stored in a 1.42-liter container at 300 K. Given: a = 1.35L2 · atm/mol2, b = 0.0322 L/mol, and R = 0.08205 L · atm/K · mol

I’m writing this equation by memory, so I hope I’m correct. It’s been about four months since we used in in my chem class:

(P - (n^2•a) / V^2) (V-nb) = nRT

Plugging in values given:

(P - (1•1.35) / (1.42^2)) (1.42 - (1•0.0322)) = (1) (0.0821) (300)

(P - (1.35/2.016)) (1.42-0.0322) = 24.63

(P - (1.35/2.016)) = 17.75

P=18.42 atm

The pressure exerted by the Argon would be 18.42 atmospheres.