Raoult's Law

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

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:

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.

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:

Two liquids $A$ and $B$ form an ideal solution at temperature $T$. When the total vapour pressure above the solution is $600$ Torr, then mole fraction of $A$ in the vapour phase is $0.35$ and in the liquid phase is $0.70$.

If vapour pressure pure 'A' and pure 'B' are ${p_A}^0 \& {p_B}^0$ then find the value of $\frac{{p_B}^0-2{p_A}^0}{10}$ (in torr).

An ideal binary liquid solution of A and B has a vapour pressure of 900 mm of Hg. It is distilled at constant temperature till $\frac{2}{3}$ of the original amount is distilled. If the mole fraction of 'A' in residue and mole fraction of B in condensate is 0.3 and 0.4 respectively and vapour pressure of residue is 860 mm of Hg then select the correct option(s).

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

Total vapour pressure of mixture of
1 mol volatile component $\mathrm{A}({\mathrm{P}}_{\mathrm{A}}^{\circ }=\mathrm{100 }\mathrm{m}\mathrm{m}\mathrm{H}\mathrm{g})$ and $\mathrm{3 }\mathrm{}\mathrm{m}\mathrm{o}\mathrm{l}$ of volatile component $\mathrm{B}({\mathrm{P}}_{\mathrm{B}}^{\circ }=\mathrm{60 }\mathrm{m}\mathrm{m}\mathrm{H}\mathrm{g})$ is $\mathrm{75 }\mathrm{}\mathrm{m}\mathrm{m}$ . For such case-

Partial pressure of a solution component is directly proportional to its mole fraction. This is known as

Two solutes $A$ and $B$ have vapour pressures, $P_A^0=400 mm$ of $Hg$ and $P_B^0=600 mm$ of $Hg$. Total volume after mixing remains the same $(∆V_{mix}=0)$. The mole fraction of $A$ in liquid phase $=0.5,$ what is the total pressure and mole fraction of $A$ and $B$ in the vapour phase?