Liquids and form an ideal solution in the entire composition range. At the vapour pressure of pure A and pure B are and , respectively. The composition of the vapour in equilibrium with a solution containing 40 mole percent of A at this temperature is:
The vapour pressures of pure liquids and are and respectively at On mixing the two liquids, the sum of their volumes is equal to the volume of the final mixture. The mole fraction of liquid is in the mixture. The vapour pressure of the final solution, the mole fractions of components and in the vapour phase, respectively are
A solution at is composed of 1.5 mol of benzene and 3.5 mol of toluene. If the vapour pressure of pure benzene and pure toluene at this temperature are 74.7 torr and 22.3 torr respectively, then the total vapour pressure of the solution and the benzene mole fraction in equilibrium with it will be, respectively:
A of solution was made by dissolving of protein at The osmotic pressure of the resulting solution is torr. The molecular weight of the protein is approximately (in )
Solution contains acetone dissolved in chloroform and solution contains acetone dissolved in carbon disulphide. The type of deviations from Raoult’s law shown by solutions and , respectively are
At , the vapour pressure of a solution containing mole of -hexane and moles of -heptane is of . At the same temperature, if one more mole of -heptane is added to this solution, the vapour pressure of the solution increases by of . What is the vapour pressure in of - heptane in its pure state______?
Liquids and form ideal solution for all compositions of and at . Two such solutions with and mole fractions of have the total vapor pressures of and bar, respectively. What is the vapor pressure of pure liquid in bar?
Which of the following statements about the composition of the vapour over an ideal 1 : 1 molar mixture of benzene and toluene is correct? Assume that the temperature is constant at . (Given vapour pressure data at , benzene = 12.8 kPa, toluene = 3.85 kPa)
A solution of urea (molar mass ) boils at at the atmospheric pressure. if and for water are and respectively. The freezing point of the solution will be