Home
Class 12
CHEMISTRY
At 70^@C vapour pressure of pure benezen...

At `70^@C` vapour pressure of pure benezene and pure toluene are 500 torr and 200 torr, respectively. In a homogeneous mixture of toluene with benzene at `70^@C`, the mole fraction of benezene is 0.4. Calculate the vapour pressure of the mixture.

Text Solution

Verified by Experts

Vapour pressure of the mixture (P) is the sum of the total partial pressures of the components.
`P = p_1 X_1 + p_2X_2 = 500 xx 0.4 + 200 xx 0.6`
Vapour pressure of mixture = `200 + 120 = 320` torr .
Promotional Banner

Similar Questions

Explore conceptually related problems

The vapour pressure of pure benzene and toluene are 160 and 60 torr respectively. The mole fraction of toluene in vapour phase in contact with equimolar solution of benzene and toluene is:

The vapour pressure of benzene and toluene are 150 mm and 50 mm respectively. A solution is prepared by mixing equal weights of benzene and toluene. Assuming the solution to be ideal, calculate the vapour pressure of the solution.

Benzene (C_(6)H_(6), 78 g//mol) and toluene (C_(7)H_(8),92g//mol) form an ideal solution. At 60^(@)C the vapour pressure of pure benzene and pure toluene are 0.507 atm and 0.184 atm, respectively. The mole fraction of benezen in a solution of these two chemicals that has a vapour preesure of 0.350 atm at 60^(@)C , will be :

Vapour pressure of beneze and toluene are 160 are 60 torr. What will be the vapour pressure of a mixture of equal masses of benezene and toluene.

A solution at 20^(@)C 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:

The vapour pressures of benzene and toluene at 293 K are 75 mm and 22 mm Hg respectively. 23.4g of benzene and 64.4 g of toluene are mixed. If the two form and ideal solution, calculate the mole fraction of benzene in the vapour phase assuming that the vapours are in equilibrium with the liquid mixture at this temperature.

The vapour pressure of pure components A and B are 200 torr and 160 torr respectively. The total pressure of the solutions obtained by mixing 2 moles of A and 3 B moles of B is.....

The vapour pressures of pure liquid A and pure liquid B at 20^(@)C are 22 and 75 mm of Hg respectively. A solution is prepared by mixing equal moles of A and B. Assuming the solution to be ideal, calculate the vapour pressure of the solution.

The vapour pressure of two pure liquids, A and B that form an ideal solution are 300 and 800 torr respectively, at temperature T. A mixture of the vapour of A and B for which the mole fraction of A is 0.25 is slowly compressed at temperature T, Calculate (a) the composition of the first drop of the condesate, (b) the total pressure when this drop is formed, (c) the composition of the solution whose normal boiling point is T, (d) the pressure when only the last bubble of vapour remains, and (e) the composition of the last bubble.

The vapour pressure of two pure liquids A and B are 50 and 40 torr respectively. If 8 moles of A is mixed with x moles of B , then vapour pressure of solution obtained is 48 torr. What is the value of x.