Question

Question 34 of 34 > Use the van der Waals equation of state to calculate the pressure of 3.60 mol of Xe at 469 K in a 5.30 L vessel. Use this list of van der Waals constants. 900 Use the ideal gas equation to calculate the pressure under the same conditions. rect

Answer 1

No of moles of the Xe gas, n = 3.60 mol Temperature, T = 469 K Gas constant, R= 0.0821 L. atm K-'mol-? Volume of the gas, V = 5.30 L Vanderwalls constants for Xe a=4.137 L.atm/ mol? b = 0.0516 L/mol According to Vanderwalls equation, (P+ amit (v – nb) = nRT nRT an V-nb 72 (3.60 mol x 0.0821 L.atm K 'mol-469K (5.30 L -3.60 molx0.0516 L/mol) 4.137 L'atm/mo12 (3.60 mol) (5.30 L) (3.60 mol x 0.0821 L.atm K 'molx469K 5.111 4.137 L.atm/m012 (3.60 mol) (5.30 L) = 27.1 atm -1.91 atm = 25.19 atm = 25.2 atm No of moles of the Xe gas, n = 3.60 mol Temperature, T = 469 K Gas constant, R= 0.0821 L.atm K-mol-1 Volume of the gas, V = 5.30 L According to ideal gas equation, PV = nRT Pressure of the Xe gas, P = nRT (3.60 mol)(0.0821 L.atm.K+mo1^)(469K) 5.30 L = 26.2 atm