In order to appreciably influence the vapor pressure of a liquid mixture a substance must form a
A) true solution
B) colloidal dispersion
C) coarse suspension
D) inanimate solution
E) animate solution
Colloidal dispersions have been observed to affect the vapor pressures most significantly as compared to other types of mixtures. Hence the right answer is B) Colloidal disperion
In order to appreciably influence the vapor pressure of a liquid mixture a substance must form...
Cornmeal will mix with water to form a A) true solution B) colloidal dispersion C) coarse suspension D) inanimate solution E) animate solution
Liquid C and D form a real solution at 25 °C. The vapor pressure of pure liquid C and D is 0.75 and 1.50 atm, respectively. At the composition of solution XC = 0.5, the liquid pressure of C is 0.25 atm. Determine the activity of liquid C and the vapor pressure of liquid D at the above mentioned composition in the solution.
5. Liquid C and D form a real solution at 25 °C. The vapor pressure of pure liquid C and D is 0.75 and 1.50 atm, respectively. At the composition of solution Xc 0.5, the liquid pressure of C is 0.25 atm. Determine the activity of liquid C and the vapor pressure of liquid D at the above mentioned composition in the solution.
Part A Two liquids, labeled A and B, form an ideal mixture with total vapor pressure P = 324.4 torr at a certain composition. At the same temperature, pure liquid A has a vapor pressure of 230 torr, while pure liquid B has a vapor pressure of 380 torr. What is the mole fraction XA of liquid A in this mixture. O 0.183 O 0.420 0.556 O 0.037 0.371
At 100 ?C the vapor pressures of hexane and octane are 1836 and 354 torr, respectively. A certain liquid mixture of these two compounds has a vapor pressure of 666torr at 100 ?C. Find the mole fractions in the liquid mixture and in the vapor phase. Assume an ideal solution.
1. At 241.95 K, the vapor pressure of liquid propane and n-butane are 160.0 kPa and 26.7 kPa, respectively.) a) Calculate the total pressure above a solution that contains 0.2 moles of propane and 0.6 moles of n-butane. Assume that the two components form an ideal solution. b) What is the composition of the vapor phase in equilibrium with the liquid phase? c) Calculate AmiG and AmixS for the formation of this mixture.
At 300 K, the vapor pressure of pure liquid A and B is 200 mmHg and 450 mmHg, respectively. If the total pressure of the mixture A and B is 350 mmHg and the assumption that the solution is ideal, calculate: (a) Mole fraction of A and B in liquid phase and vapor phase, (b) The activity and activity coefficient of A and B in the solution, and (c) The mixing free energy, Agm, and the mixing entropy, Asm, of...
Benzene, C6H6, and octane, C8H14, form an ideal solution. At 60°C the vapor pressure of pure benzene is 0.507 atm, and the vapor pressure of pure octane is 0.103 atm. A solution is composed of 3.53 g of benzene, and 40.2 g of octane. What is the mole fraction of benzene in the vapor phase above the liquid? In order to receive full credit, your work should clearly show the following: a) the calculation of the partial pressure of benzene...
6. At 60°C, pure substance A has a vapor pressure of 380 mmHg and pure substance B of 140 mmHg. The mole fraction XB=0.15 is in the range of validity of Henry's law. The partial pressure of B at XB=0.1 is 20 mmHg. (a) What is the vapor partial pressure PB at XB=0.15? Answer: PB=30 mmHg. (b) What would PB be at XB=0.15 if the solution were ideal? Answer: PB=21 mmHg. (c) What is the activity coefficient of B, γB,...
4. At 300 K, the vapor pressure of pure liquid A and B is 200 mmHg and 450 mmHg, respectively. If the total pressure of the mixture A and B is 350 mmHg and the assumption that the solution is ideal, calculate: (a) Mole fraction of A and B in liquid phase and vapor phase, (b) The activity and activity coefficient of A and B in the solution, and (c) The mixing free energy, Agm, and the mixing entropy, Asm,...