Two liquids A and B form an ideal solution. At a certain temperature, the vapor pressure of pure A is 400 mm Hg and that of pure B is 700 mm Hg. If the mole fraction of A in the liquid phase is 0.4, what is the mole fraction of A in the vapor phase?

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

A solution of liquids A and B shows no change in volume and no heat exchange upon mixing. This indicates that:

The partial pressure of ethane over a saturated solution containing $6.56 imes {10^{ - 2}} g$ of ethane is 1 bar. If the solution contains $5.0 imes {10^{ - 2}}\;g$ of ethane, the partial pressure of ethane will be :

At 25°C, an equimolar mixture of benzene (vapor pressure = 12.8 kPa) and toluene (vapor pressure = 3.85 kPa) forms an ideal solution. If the total pressure above the solution is 8.325 kPa, which component has a higher partial pressure in the vapor phase?

Benzene and toluene form nearly ideal solutions. At $25^\circ C$, the vapour pressure of benzene is 75 torr and that of toluene is 22 torr. The partial vapour pressure of benzene at $20^\circ C$ for a solution containing 78 g of benzene and 46 g of toluene in torr is

When attraction between $A - B$ is more than that of $A - A$ and $B - B$, the solution will show…..deviation from Raoult’s law

The ratio of vapour pressure over solution phase on mixing two immiscible liquids is equal to :

According to Raoult's law, the relative lowering of vapour pressure for a solution is equal to:

On mixing $10\,ml$ of acetone with $40\,ml$ of chloroform, the total volume of the solution is

A solution containing components $A$ and $B$ follows Raoult’s law