The liquids X and Y from ideal solution having vapour pressures 200 and 100mm Hg respectively. Calculate the mole fraction of component X in vapour phase in equilibrium with an equimolar solution of the two.

Benzene and toluene form ideal solution over the entire range of composition. The vapour pressure of pure benzene and toluene at 300 K are 50.71 mm Hg and 32.06 mm Hg respectively. Calculate the mole fraction of benzene in vapour phase if 80 g of benzene is mixed with 100 g of toluene.

Two liquids A and B have vapour pressure of 0.658 bar and 0.264 bar respectively. In an ideal solution of the two, calculate the mole fraction of A at which the two liquids have equal partial pressures.

Vapour pessure of a liquid or a solution is the pressure exerted by the vapour in equilibrium with the liquid or solution at a particular temperature. It depends upon the nature of the liquid and temperature. It depends upon the nature of the liquid and temperature. According to Raoult's law in a solution, the vapour pressure of a component at a given temperature is equal to the mole fraction of that component in solution multiplied by the vapour pressure of that component in hte pue state. this solution in which each component obeys Raoult's law are called ideal solutions. there are two types of non ideal solutions, showing positive deviations and negative deviations from ideal behaviour. If liquid A and B form ideal solution, then

Two liquids A and B have P_A^(@)" and P_B^(@) in the ratio of 1 : 3 and the ratio of number of moles of A and B in liquid phese are 1 : 3 then mole fraction of 'A' in vapour phase in equilibrium with the solution is equal to :

Benzene and toluene form nearly ideal solution . At 313 K the vapour pressure of benzene and toluene are 160 mm and 60 mm of Hg respectively. Calculate the total pressure of the solution made by mixing their equal masses at 313 K.

P_A and P_B are the vapour pressure of pure liquid components A and B respectively of an ideal binary solution. If X_A represent the mole fraction of component A, then the total pressure of the solution will be