Raoult's law and vapour pressure

At 300 K, the ratio of the molar volume of pure B in vapour phase to its molar volume in liquid phase is ____.

The mole fraction of B in vapour phase which is in equilibrium with this solution is ____.

A non-volatile, non-electrolyte solid solute when dissolved in 40 g of a solvent, the vapour pressure of the solvent decreased from 760 mm Hg to 750 mm Hg. If the same solution boils at 320 K, then the number of moles of the solvent present in the solution is ________. (Nearest integer)
[Given: boiling point of the pure solvent = 319.5 K, $K_b$ of the solvent = 0.3 K kg mol$^{-1}$]

When 0.25 moles of a non-volatile, non-ionizable solute was dissolved in 1 mole of a solvent the vapor pressure of solution was $x$ % of vapor pressure of pure solvent. What is $x$ %?

An aqueous solution is prepared by dissolving 0.1 mol of an ionic salt in 1.8 kg of water at 35 ºC. The salt remains 90% dissociated in the solution. The vapour pressure of the solution is 59.724 mm of Hg. Vapor pressure of water at 35 ºC is 60.000 mm of Hg. The number of ions present per formula unit of the ionic salt is ________.

The vapour pressures of two volatile liquids A and B at 25°C are 50 Torr and 100 Torr, respectively. If the liquid mixture contains 0.3 mole fraction of A, then the mole fraction of liquid B in the vapour phase is $\frac x{17}$. The value of $x$ is ______.

A box contains 0.90 g of liquid water in equilibrium with water vapour at 27°C. The equilibrium vapour pressure of water at 27°C is 32.0 Torr. When the volume of the box is increased, some of the liquid water evaporates to maintain the equilibrium pressure. If all the liquid water evaporates, then the volume of the box must be ______ litre. [nearest integer]

(Given: R = 0.082 L atm K$^{-1}$ mol$^{-1}$)

(Ignore the volume of the liquid water and assume water vapours behave as an ideal gas.)

When a certain amount of solid A is dissolved in 100 g of water at 25°C to make a dilute solution, the vapour pressure of the solution is reduced to one-half of that of pure water. The vapour pressure of pure water is 23.76 mmHg. The number of moles of solute A added is ______. (Nearest Integer)

A gaseous mixture of two substances A and B, under a total pressure of 0.8 atm is in equilibrium with an ideal liquid solution. The mole fraction of substance A is 0.5 in the vapour phase and 0.2 in the liquid phase. The vapour pressure of pure liquid A is ______ atm. (Nearest integer)

Liquids A and B form ideal solution for all compositions of A and B at 25 °C. Two such solutions with 0.25 and 0.50 mole fractions of A have the total vapor pressures of 0.3 and 0.4 bar, respectively. What is the vapor pressure of pure liquid B in bar?

On dissolving 0.5 g of a non-volatile non-ionic solute to 39 g of benzene, its vapor pressure decreases from 650 mm Hg to 640 mm Hg. The depression of freezing point of benzene (in K) upon addition of the solute is ______

(Given data: Molar mass and the molal freezing point depression constant of benzene are 78 g mol⁻¹ and 5.12 K kg mol⁻¹, respectively)

Liquids A and B form ideal solution over the entire range of composition. At temperature T, equimolar binary solution of liquids A and B has vapour pressure 45 Torr. At the same temperature, a new solution of A and B having mole fractions $x_A$ and $x_B$, respectively, has vapour pressure of 22.5 Torr. The value of $x_A/x_B$ in the new solution is ______.

(given that the vapour pressure of pure liquid A is 20 Torr at temperature T)

For a solution formed by mixing liquids L and M, the vapour pressure of L plotted against the mole fraction of M in solution is shown in the following figure. Here $x_\mathrm{L}$ and $x_\mathrm{M}$ represent mole fractions of L and M, respectively, in the solution. The correct statement(s) applicable to this system is(are)

Pure water freezes at 273 K and 1 bar. The addition of 34.5 g of ethanol to 500 g of water changes the freezing point of the solution. Use the freezing point depression constant of water as $2\ \mathrm{K\,kg\,mol^{-1}}$. The figures shown below represent plots of vapour pressure (V.P.) versus temperature (T). [molecular weight of ethanol is $46\ \mathrm{g\,mol^{-1}}$]

Among the following, the option representing change in the freezing point is

A solution is prepared by mixing 8.5 g of $\ce{CH2Cl2}$ and 11.95 g of $\ce{CHCl3}$. If vapour pressure of $\ce{CH2Cl2}$ and $\ce{CHCl3}$ at 298 K are 415 and 200 mmHg respectively, the mole fraction of $\ce{CHCl3}$ in vapour form is :

(Molar mass of Cl = 35.5 g mol$^{-1}$)

18 g glucose ($\ce{C6H12O6}$) is added to 178.2 g water. The vapor pressure of water (in torr) for this aqueous solution is :

The solubility of $\ce{N2}$ in water at 300 K and 500 torr partial pressure is 0.01 g L$^{-1}$. The solubility (in g L$^{-1}$) at 750 torr partial pressure is :

The vapour pressure of acetone at 20°C is 185 torr. When 1.2 g of a non-volatile substance was dissolved in 100 g of acetone at 20°C, its vapour pressure was 183 torr. The molar mass (g mol$^{-1}$) of the substance is :

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 :

Choose the correct statement with respect to the vapour pressure of a liquid among the following :