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For CO2 the van der Waals constants are a=3.59 atm • L2/mol2 and b=0.0427 L/mol. Calculate the pressure exerted by 2.50 moles of CO2 confined in a volume of 5.00 L at 450 K.

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The pressure is 17.97 atm;

[P + a\((\frac{n}{V}) ^{2}\)](V-nb) = nRT;

[P + 3.59 atm·L²mol⁻²\((\frac{2.50 mol}{5.00 \text L}) ^{2}\)](5.00 L - 2.50 mol × 0.0427 mol·L⁻¹) = 2.50 mol × 0.08206 L·atm·K⁻¹mol⁻¹ × 450 K;

(P + 0.898 atm)(5.00 L - 0.107 L) = 92.3 L·atm;

(P + 0.898 atm)(4.89) = 92.3 atm;

P + 0.898 atm = \(\frac{92.8 atm}{4.89}\) = 18.87 atm;

P = 18.87 atm - 0.898 atm = 17.97 atm

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