Use the virial equation to calculate the pressure that one mole of dme (dimethyl ether) exerts when it occupies a volume of 4.0 l at a temperature of 303.15 k. the second virial3
coefficient, b for dme is -461.34 cm /mol. (hint: use only the first two terms of the virial equation). (6 pts)
(b) compare this result with the pressure calculated using the perfect gas equation and determine which is more dominant, the attractive forces or the repulsive forces. (you must provide an explanation to receive credit)
2) a mixture of oxygen and ammonia at 273.15 k and 1.00 atm has a volume of 150.0 cm .this mixture is cooled to the temperature of liquid nitrogen at which ammonia freezes out
and the remaining gas is removed from the vessel. the vessel is allowed to warm to 273.15 k and 1 atm, and the volume is now 85.0 cm . calculate the mole fraction of ammonia in the
original mixture.
3) (a) use the van der waals equation to calculate the volume occupied by one mole of xe gas at 400 k and 20.0 atm pressure. the van der waals constants are a = 4.19 atm l2 mol-2 and b= 0.051 l mol-1 .
(b) determine which is more dominant, the attractive forces or repulsive forces under these conditions. (you must provide an explanation to receive credit).
4) (a) calculate the critical constants (pc, tc, vc) for co2 if the van der waals constants are a = 22.8 dm6 bar mol-2 and b = 0.146 dm3 mol-1
(b) calculate the reduced pressure and the reduced temperature when co2 is found at 1.25 atm and 145c.