A solution showing a large positive deviation from Raoult's law forms a:

At 25°C, the vapor pressures of pure benzene and toluene are 12.8 kPa and 3.85 kPa, respectively. If an ideal solution is prepared with 2 moles of benzene and 1 mole of toluene, what is the total vapor pressure above the solution?

The vapour pressure $(VP)$ of a dilute solution of non-volatile solute is $P$ and the $VP$ of pure solvent is ${P_0}$, the lowering of the $VP$ is :

An aqueous solution of glucose was prepared by dissolving 18 g of glucose in 90 g of water. The relative lowering in vapour pressure is

Which of the following mixtures exhibits a positive deviation from Raoult's law?

A liquid is kept in a closed vessel. If a glass plate (negligible mass) with a small hole is kept on top of the liquid surface, then the vapour pressure of the liquid in the vessel is :

The vapour pressure of pure liquid A is $0.80\;atm$. When a non-volatile B is added to A its vapour pressure drops to $0.60\;atm$. The mole fraction of B in the solution is

The azeotropic mixture of water (b. pt.100℃) and HCl (b.pt. 85℃) boils at 108.5℃.When this mixture is distilled it is possible to obtain

Among the following mixtures, dipole-dipole as the major interaction is present in :

A solution of benzene and toluene at 25°C has a total vapor pressure of 7.0 kPa. The vapor pressures of pure benzene and toluene at this temperature are 12.8 kPa and 3.85 kPa, respectively. Assuming ideal behavior, what is the mole fraction of benzene in the liquid phase?

Relative lowering of vapour pressure of a dilute solution is 0.2. What is the mole fraction of the non-volatile solute ?