3. Liquids A and B form an ideal solution. At 25 °C, the vapor pressure of liquid A and B is 13.0 kPa and 26.0 kPa,...
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
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.
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.
The vapor pressure of liquid C4H10 is 324.1 mmHg at a temperature of 251.0 K. The enthalpy of vaporization, ΔHvap, for this liquid is 22.4 kJ/mol. What is the vapor pressure of C4H10 at a temperature of 269.2 K, in mmHg?
The vapor pressure of a liquid is 300 torr at 51.0 °C, and its enthalpy of vaporization is 37.66 kJ/mol. Calculate the normal boiling point of this liquid in °C?
The vapor pressure of a liquid is 405 torr at 69.0 °C, and its enthalpy of vaporization is 45.34 kJ/mol. Calculate the normal boiling point of this liquid in °C? Only provide the numerical value below.
Two liquids A and B have vapor pressures of 70.3 and 131 mmHg, respectively, at 25°C. What is the total vapor pressure of the ideal solution made up of: (a) 1.00 mole of A and 1.00 mole of B (b) 2.00 moles of A and 5.00 moles of B
Calculate the vapor pressure of 3-pentanone (b.p. 102.0 °C) at the gas chromatography column temperature of 96.0"C using the form of the Clausius-Clapeyron equation shown below, P1 P. vap where R is the ideal gas constant, ???? is the enthalpy of vaporization, T1 and T2 are two different temperatures, and P1 and P2 are the vapor pressures at the respective temperatures. The enthalpy of vaporization can be estimated using Trouton's rule, ??'vap-(88 J mol-1 K-1), Tp. Number Torr Calculate the...
5. Ethanol and methanol are form an ideal solution at 20 °C. Vapor pressure of pure ethanol and pure methanol at 20 °C is 44.5 and 88.7 mmHg, respectively. If 100 g of ethanol and 100 g of methanol are mixed into a solution, calculate: (a) the mol fractions of ethanol and methanol in the solution, (b) the partial pressures of ethanol and methanol and total pressure of the solution, and (c) the mol fraction of methanol in a vapor...