PHASE DIAGRAMS The vapour pressure of pure liquid CCl4 is 23 kPa and its Henry's law constant in liquid Br2 is 73 kPa at 20°C. Calculate the vapour pressure of each component, the total pressure, and the composition of the vapour phase (y and y B) when the mole fraction of CC₁ is 0.066.
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- At 25°C the vapour pressure of pure pentane is 511 torr and that of hexane is 150. torr.What is the mole fraction of pentane in a pentane-hexane solution that has a vapour pressure of 346 torr at 25°C? What is the mole fraction of hexane in the vapour that is in equilibrium with this solution?(Assume ideal gas behaviour.)Hexane and perfluorohexane show partial miscibility below 22.70 °C. The critical concentration at the upper critical temperature is x = 0.355, where x is the mole fraction of C6F14. At 22.0 °C the two solutions in equilibrium have x = 0.24 and x = 0.48, respectively, and at 21.5 °C the mole fractions are 0.22 and 0.51. Sketch the phase diagram. Describe the phase changes that occur when perfluorohexane is added to a fixed amount of hexane at (i) 23 °C, (ii) 22 °C.An ideal-dilute solution of chloroform and ethanol with a mole fraction of ethanol in the liquid phase Xeth = 0.9900 has a total vapour pressure of p = 17795 Torr. The vapour pressure of pure ethanol at this temperature is p*eth = 172.76Torr. (a) Use Raoult's law to calculate the partial pressure of ethanol in the vapour phase. (b) Hence determine the partial pressure of chloroform in the vapour phase . (c) Also calculate the mole fractions of chloroform and ethanol in the vapour phase. (d) Calculate the Henry's law constant for chloroform, Kchl at this temperature.
- Two liquids, A and B, show partial miscibility below 52.4 °C. The critical concentration at the upper critical temperature is x = 0.459, where x is the mole fraction of A. At 40.0 °C the two solutions in equilibrium havex = 0.22 and x = 0.60, respectively, and at 42.5 °C the mole fractions are 0.24 and 0.48. Sketch the phase diagram. Describe the phase changes that occur when B is added to a fixed amount of A at (i) 48 °C, (ii) 52.4 °C.A solvent (molar mass = 98.2 g mol-¹) has a vapour pressure of 4930 Pa at 20 °C; at 50 °C this increases to 1.94 x 104 Pa. A mass of 12.8 g of an unknown solute is dissolved in 100.0 g of the solvent. Assume the solute has negligible vapour pressure. Estimate the normal boiling point of the solution.(b) At 80 °C, ethylene dibromide and propylene dibromide mixture forms an ideal solution. Given that the pure vapour pressures of ethylene dibromide and propylene dibromide are 22.9 and 16.9 kPa, respectively. Using the plots of partial vapour pressures of ethylene dibromide and propylene dibromide, and total vapour pressure of the mixture against the mole fraction of ethylene dibromide, determine (i) the composition of the vapour in equilibrium with a solution containing 0.75 mole fraction of ethylene dibromide. (ii) the composition of the liquid phase in equilibrium with ethylene dibromide- propylene dibromide containing 0.5 mole fraction each.
- At 100 degrees celcius the vapour pressures of hexane and octane are 1836 and 354 torr,respectively. A certain liquid mixture of these two compounds (that is both totallymiscible) has a vapour pressure of 0.88 atm at 100 degrees celcius. Calculate the compositions inboth the liquid and the vapour phases.A and B form ideal solution. If mole fraction of A in the solution is xĄ, what will be its mole fraction in vapour state? (vapour pressure of pure A and B are respectively P° and P) BAt 90°C, the vapor pressure of methylbenzene is 53.3 kPa and that of 1,2-dimethylbenzene is 20.0 kPa. What is the composition of a liquid mixture that boils at 90°C when the pressure is 0.50 atm? What is the composition of the vapor produced?
- (Please answer both) A binary solution of A and B with xA = 0.6589 has a boiling point of 88 °C. At this temperature the vapour pressures of A and B are 127.6 kPa and 50.60 kPa, respectively. Is the solution ideal? What is the composition of the vapour (in terms of yA) above the solution?The vapour pressure of 2-propanol, C3 H8 O, is 50.00 kPa at 338.8°C, but it fell to 49.62 kPa when 8.69 g of an involatile organic compound was dissolved in 250 g of 2-propanol. Assuming that 2-propanol is ideal and it obeys Raoult’s Law, calculate the molar mass of the compound in gram per mole. (molar mass: C = 12 g/mol; O = 16 g/mol; H = 1 g/mol) Choices a = 670 b = 272 c = 544 d = 98 e = 160At 25 °C the saturated vapour pressure of water is 3.165 kPa (23.75 mm Hg). Find the saturated vapour pressure of a 5% aqueous solution of urea (carbamide) at the same temperature. (Molar mass of urea = 60.05 g mol-1)