Raoult's Law

Under what condition Henry's law becomes special case of Raoult's Law?

For a binary ideal liquid solution, the variation in total vapour pressure versus composition of solution is given by which of the curves?

An aqueous solution is made by dissolving $10\mathrm{g}$ of glucose $\left({\mathrm{C}}_6{\mathrm{H}}_{12}{\mathrm{O}}_6\right)$ in $90\mathrm{g}$ of water at $300 \mathrm{K}$. If the vapour pressure of pure water at $300 \mathrm{K}$ is $32.8 \mathrm{mm} \mathrm{Hg}$, what would be the vapour pressure of the solution?

What changes occurs in the vapour pressure as a non-volatile solute is added to a pure liquid solvent?

Two liquids are mixed together to form a mixture which boils at same temperature and their boiling point is higher than the boiling point of either of them, so they show _____ from Raoult's law.

The vapour pressure of the solution is affected by adding the _____ solute.

When will the vapour pressure of the volatile liquid lowered?

The vapour pressure of water is $12.3\mathrm{kPa}$ at $300 \mathrm{k}$. Now, calculate the vapour pressure of $1$ molar solution of a solute in it.

_____ law which states that for a solution of volatile liquids, the partial vapour pressure of each component of the solution is directly proportional to its mole fraction present in solution.

The following is a graph plotted between the vapour pressure of two volatile liquids against their respective mole fractions.

Which of the following statement is correct ?

For a dilute solution containing$2.5 \mathrm{g}$ of a non-volatile non-electrolyte solution in $100 \mathrm{g}$of water, the elevation in boiling point at $1$$\mathrm{atm}$ pressure is$2°\mathrm{C}.$ Assuming the concentration of solute is much lower than the concentration of the solvent, the vapor pressure of the solution is (${\mathrm{K}}_{\mathrm{b}} = 0.76 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}$)

Two liquids $\mathrm{X}$ and $\mathrm{Y}$ form an ideal solution. At $300 \mathrm{K}$, vapour pressure of the solution containing $1$ mole of $\mathrm{X}$ and $3$ mole of $\mathrm{Y}$ is $550 \mathrm{mm} \mathrm{Hg}$. At the same temperature, if$1$  mole of $\mathrm{Y}$ is further added to this solution, vapour pressure of the solution increases by$10 \mathrm{mm} \mathrm{Hg}$ . Vapour pressure (in $\mathrm{mm} \mathrm{Hg}$) of $\mathrm{X}$ and $\mathrm{Y}$ in their pure states will be, respectively

The vapours pressure of pure components $\mathrm{X}$ and $\mathrm{Y}$ are $200$ $\mathrm{torr}$ and $100$$\mathrm{torr}$ respectively. Assuming a solution of these components obeys Raoult's law, the mole fraction of component $\mathrm{X}$ in the vapours phase in equilibrium with a solution containing equimolecular of $\mathrm{X}$ and $\mathrm{Y}$ is

$30$ $\mathrm{g}$ of urea $\left(\mathrm{M}=60 \mathrm{g} {\mathrm{mol}}^{-1}\right)$ is dissolved in $846$ $\mathrm{g}$ of water. Calculate the vapour pressure of water for this solution if vapour pressure of pure water at $298$ $\mathrm{K}$ is $23.8$ $\mathrm{mmHg}$.

Which of the following units is most useful in relating concentration of solution with its vapour pressure?

When partial pressure of solvent in solution of non-volatile solute is plotted against its mole fraction, nature of graph is

Partial pressure of solvent (mole fraction$={\mathrm{x}}_1$) in solution of non-volatile solute (mole fraction$={\mathrm{x}}_2$) is given by equation,

Explain the determination of molar mass of a solute from relative lowering in vapour pressure.

In an equilibrium at ${30}^0\mathrm{C}$ with a benzene-toluene solution, the mole fraction of benzene is 0.400, then, what is the mole fraction of toluene in vapour phase?

$\left({\mathrm{P}}_{\mathrm{B}}^0=119\mathrm{ }\mathrm{t}\mathrm{o}\mathrm{r}\mathrm{r}\mathrm{ }\mathrm{a}\mathrm{n}\mathrm{d}\mathrm{ }{\mathrm{P}}_{\mathrm{r}}^0=37.0\mathrm{ }\mathrm{t}\mathrm{o}\mathrm{r}\mathrm{r}\right)$

Maximum boiling azeotrope will be formed by-