Molar fraction of ethanol in a solution is 0.2. Calculate the total vapour pressure of the vapour phase. The vapour pressure of pure water and ethanol at a given temperature is 4 Kpa and 8 Kpa. a. 4.8 b.3.2 c. 1.6 d. 5.2
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- A mixture of organic solvent (nitrobenzene) and water boils at 363K. The vapour pressure of water at 363K is 733mm. Calculate the weight percentage of the organicsolvent in the distillate.At 300 K, the vapour pressures of dilute solutions of HCI in liquid GeCI4 are as follows: x(HCI) 0.005 0.012 0.019p/kPa 320 76.9 121 .8 Show that the solution obeys Henry's law in th is range of mole fractions and calculate Henry's law constant at 300 K.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.
- A vapour solution with a mole percentage of 10% benzene is cooled gradually. At what temperature does liquid first appear?A dilute solution of bromine in carbon tetrachloride behaves as an ideal dilute solution. The vapour pressure of pure CCl4 is 33.85 Torr at 298 K. The Henry’s law constant when the concentration of Br2 is expressed as a mole fraction is 122.36 Torr. Calculate the vapour pressure of each component, the total pressure, and the composition of the vapour phase when the mole fraction of Br2 is 0.050, on the assumption that the conditions of the ideal dilute solution are satisfied at this concentration.An open vessel containing water stands in a laboratory measuring 5.0 m × 5.0 m × 3.0 m at 25 °C; the vapour pressure of water at this temperature is 3.2 kPa. When the system has come to equilibrium, what mass of water will be found in the air if there is no ventilation? Repeat the calculation for open vessels containing benzene (vapour pressure 13.1 kPa) and mercury (vapour pressure 0.23 Pa).
- At 25 °C, the vapour pressure of pure benzene is 12.8 kPa and the vapour pressure of pure methylbenzene (toluene) is 3.8 kPa. Consider a liquid mixture with mole ratio 30% benzene-70% methylbenzene, which you can treat as an ideal liquid mixture, in a closed container. a) Calculate the mole ratio of benzene and methylbenzene in the vapour.At 90°C, the vapour pressure of methylbenzene is 54kPa and that of 1,3-dimethylbenzene is 18.0 kPa. What is the molar fraction of methylbenzene in the gas phase above the mixture containing 1 mol of methylbenzene and 2mol of 1,3-dimethylbenzene at this temperature (assume that these solvents form ideal solutions).The vapour pressure of pure liquids A and B at 400 K are 450 and 700 mmHg respectively. Find out the composition of liquid mixture if total vapour pressure at this temperature is 600 mmHg.
- 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.The pure vapour pressure of benzene (C6H6) is 745 torr; the pure vapour pressure to toluene(C7H8) is 290 torr. What is the mole fraction of benzene in a benzene/toluene mixture whose total vapour pressure is 500 torr? Give answer to 3dp.The vapor pressures of 1,2-dibromoethane (M = 187.9 g mol-1and 1,2-dibromopropane (M =201.9 g mol-1), both measured at 343 K, are 12.90 and 9.17 kPa, respectively. Assuming thatthese two liquids form an ideal mixture, calculate the pressure of the vapor phase which is inequilibrium at 343 K with a liquid containing 50 % by mass of each of these components