Question

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.

Answer 1

The pressure is 17.97 atm; [P + a
`((n)/(V)) ^(2)`](V-nb) = nRT; [P + 3.59 atm·L²mol⁻²
`((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 =
`(92.8 atm)/(4.89)` = 18.87 atm; P = 18.87 atm - 0.898 atm = 17.97 atm