Vapour Pressure of Liquid - Vapour Pressure of Solutions of Solids in Liquids

A solution containing 10 g per dm³ of urea (molecular mass = 60 g mol^–1) is isotonic with a 5% solution of a non-volatile solute. The molecular mass of this non-volatile solute is:

The vapour pressures of pure liquids A and B are 400 and 600 mm Hg, respectively at 298 K On mixing the two liquids, the sum of their initial volumes is equal to the volume of the final mixture. The mole fraction of liquids B is 0.5 in the mixture. The vapour pressure of the final solution, the mole fractions of components A and B in vapour phase, respectively are ______.

Why is the vapour pressure of an aqueous solution of glucose lower than that of water?

The solubility of a solid in a liquid is significantly affected by temperature changes.

$$\mathrm{Solute}+\mathrm{Solvent}⟶\mathrm{Solution}$$

The system being in a dynamic equilibrium must follow Le-chatelier’s principle.

Considering the Le-chatelier’s principle which of the following is correct?

The vapour pressure of pure benzene at a certain temperature is 0.850 bar. A non-volatile, nonelectrolyte solid weighing 0.5 g is added to 39.0 g of benzene (molar mass 78 g/mol). The vapour pressure of the solution then is 0.845 bar. What is the molecular mass of the solid substance?

State Raoult's law for the solution containing volatile components. What is the similarity between Raoult's law and Henry's law?

The vapour pressure of a 5% aqueous solution of non-volatile organic substance at 373 k is 745 mm. calculated the molecular mass of the solute

The vapour pressure of a solvent decreases by 10 mm of Hg when a non-volatile solute was added to the solvent. The mole fraction of the solute in the solution is 0.2. What should be the mole fraction of the solvent if the decrease in the vapour pressure is to be 20 mm of Hg?