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?

Raoult's law becomes a special case of Henry's law when ${\mathrm{K}}_{\mathrm{H}}$$=$${\mathrm{p}}^0$. In this equation, ${\mathrm{K}}_{\mathrm{H}}$ is 

At $298 \mathrm{K}$, the vapour pressure of an ideal solution containing $1 \mathrm{mol}$ of liquid $\mathrm{L}1$ and $2 \mathrm{mol}$ of liquid $\mathrm{L}2$ is $500 \mathrm{mm}$ Hg. When $2 \mathrm{mol}$ of $\mathrm{L}1$ is added to this solution, the vapour pressure of the solution increases by $5\%$. What are the respective vapour pressures (in mm $\mathrm{Hg}$ ) of $\mathrm{L}1$ and $\mathrm{L}2$ in their pure states at $298 \mathrm{K}$ ?

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.

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

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,

If Two liquids A and B which form a non-ideal solution which obey the  below equation as ${\mathrm{P}}_{\mathrm{T}}={\mathrm{P}}_{\mathrm{A}}^0+3({\mathrm{P}}_{\mathrm{B}}^0-{\mathrm{P}}_{\mathrm{A}}^0){\mathrm{X}}_{\mathrm{B}}+2({\mathrm{P}}_{\mathrm{A}}^0-{\mathrm{P}}_{\mathrm{B}}^0){\mathrm{X}}_{\mathrm{B}}^2\mathrm{.}$

Calculate the exact composition (by mole) when this mixture boils without change in composition at a definite temperature of an equimolar mixture of A and B is distilled, Where ${\mathrm{P}}_{\mathrm{A}}^0 \mathrm{and} {\mathrm{P}}_{\mathrm{B}}^0$ , $({\mathrm{P}}_{\mathrm{B}}^0>{\mathrm{P}}_{\mathrm{A}}^0)$ are vapour pressures of A and B respectively ${\mathrm{X}}_{\mathrm{B}}=$ mole fraction of B in liquid phase

Maximum boiling azeotrope will be formed by-

Two volatile liquids $\mathrm{A}$ and $\mathrm{B}$ are mixed in a molar ratio of $1:4$. The value of ${\mathrm{P}}_{\mathrm{A}}^{\circ }$ and ${\mathrm{P}}_{\mathrm{B}}^{\circ }$ are $440 \mathrm{mm} \mathrm{Hg}$ and $120 \mathrm{mm} \mathrm{Hg}$, respectively. What is the total vapour pressure of the solution?

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

A mixture of liquid $\mathrm{A}$ and $\mathrm{B}$ is formed which boils at $80 °\mathrm{C}$ and $1 \mathrm{atm}$pressure, then calculate the amount of $\mathrm{A}$ in the above mixture if vapour pressure of pure liquid $\mathrm{A}$ and $\mathrm{B}$ is $520 \mathrm{mm} \mathrm{Hg}$ and $1000 \mathrm{mm} \mathrm{Hg}$, respectively, at $80 °\mathrm{C}$
($1 \mathrm{atm} = 760 \mathrm{mm} \mathrm{of} \mathrm{Hg}$)

In a solution of ${\mathrm{CS}}_2$ and acetone, the mole fraction of ${\mathrm{CS}}_2$ is $0.25$ and the total vapor pressure is $600 \text{mm Hg}$. Which of the following statements about the solution is true?

[Given: At $35°\mathrm{C}$, the vapor pressure of ${\mathrm{CS}}_2$ is $512 \text{mm Hg}$ and of acetone is $344 \text{mm Hg}$.]

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:

If ${\mathrm{P}}^0$ and ${\mathrm{P}}_{\mathrm{S}}$ are the vapour pressures of the solvent and solution respectively, ${\mathrm{n}}_1$ and ${\mathrm{n}}_2$ are the mole fractions of the solvent and solute respectively, then

A solution is prepared containing a 2:1 mol ratio of dibromo ethane $\left({\mathrm{C}}_2{\mathrm{H}}_4\mathrm{B}{\mathrm{r}}_2\right)$ and dibromo propane $\left({\mathrm{C}}_3{\mathrm{H}}_6\mathrm{B}{\mathrm{r}}_2\right)$. What is the total vapour pressure over the solution assuming ideal behaviour?