Raoult's Law

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

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.

A mixture of toluene and benzene forms a nearly ideal solution. Assume ${\mathrm{P}}_{\mathrm{B}}°$ and ${\mathrm{P}}_{\mathrm{T}}°$ to be the vapor pressures of pure benzene and toluene, respectively. The slope of the line obtained by plotting the total vapor pressure to the mole fraction of benzene is:

In the pressure vs. the mole fraction of benzene curves/lines shown below, the total vapour pressure of an ideal mixture of benzene and toluene will follow the curve/line.

Vapour pressure of benzene is $200 \mathrm{mm} \mathrm{Hg}$. When $2\mathrm{g}$ of non-volatile solute is dissolved in $78\mathrm{g}$ benzene, benzene solution has vapour pressure $\text{195 mm Hg}$. Calculate the molar mass of the solute in ${\mathrm{gmol}}^{-1}$( molar mass of benzene = $78{\mathrm{gmol}}^{-1}$).

Raoult's law 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.

_____ 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 (${\mathrm{K}}_{\mathrm{b}} = 0.76 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}$)

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-

Mark the correct statement(s) from the following.

Select the correct option from the following colligative effect: