Lowering of Vapour Pressure

Hoar frost is -

An ideal solution is made up of two volatile liquids $\mathrm{A} \mathrm{and} \mathrm{B}$ ($\mathrm{p}=125 \mathrm{torr}, \mathrm{P} = 46.3 \mathrm{torr}$) As the pressure is reduced, first vapour appears at $70$ torr. Thus, mole fraction of the liquid A in the mixture is?

Which of the following plots does not represent the behaviour of an ideal binary liquid solution?

$6 \mathrm{g}$ of urea is dissolved in $90 \mathrm{g}$ of water. The relative lowering of vapour pressure is equal to 

$80$ mole percent of ${\mathrm{MgCl}}_2$ is dissociated in aqueous solution. The vapour pressure of $1.0$ molal aqueous solution of ${\mathrm{MgCl}}_2$ at ${38}^{\mathrm{o}}\mathrm{C}$ is _____ $\mathrm{mm} \mathrm{Hg}$. (Nearest integer)

Given: Vapour pressure of water at ${38}^{\mathrm{o}}\mathrm{C}$ is $50 \mathrm{mm} \mathrm{Hg}$

What weight of glucose must be dissolved in $100 \mathrm{g}$ of water to lower the vapour pressure by $0.20 \mathrm{mm} \mathrm{Hg}$?
(Assume dilute solution is being formed)
Given: Vapour pressure of pure water is $54.2 \mathrm{mm} \mathrm{Hg}$ at room temperature.Molar mass of glucose is $180 \mathrm{g} {\mathrm{mol}}^{-1}$

Mass of Urea $\left({\mathrm{NH}}_2{\mathrm{CONH}}_2\right)$ required to be dissolved in $1000 \mathrm{g}$ of water in order to reduce the vapour pressure of water by $25\%$ is $\mathrm{\_\_\_\_\_\_\_} \mathrm{g}.$ (Nearest integer)

Given : Molar mass of $\mathrm{N}, \mathrm{C}, \mathrm{O}$ and $\mathrm{H}$ are $14, 12, 16$ and $1 \mathrm{g} {\mathrm{mol}}^{-1}$ respectively.

Lowering of vapour pressure of $30\%$ of aqueous solution of glucose (in mm Hg)

Given: ${\mathrm{P}}_{{\mathrm{H}}_2\mathrm{O}}= 760 \mathrm{mm} \mathrm{of} \mathrm{Hg}$

Some amount of urea is added to $1000 \mathrm{gm}$of ${\mathrm{H}}_2\mathrm{O}$ due to which the vapour pressure decreases by the $25\%$ of the original vapour pressure. Find out the mass of urea added 

The relative lowering of vapour pressure of $1\%$ solution of aniline in ether was $0.007$. Calculate the molecular weight of aniline.

If $8 \mathrm{g}$ of a non-electrolyte solute is dissolved in $114 \mathrm{g}$of n-octane to reduce its vapour pressure to$80\%$, the molar mass (in $\mathrm{g} {\mathrm{mol}}^{-1}$) of the solute is [Given that molar mass of n-octane is $114 \mathrm{g} {\mathrm{mol}}^{-1}$].

What is Raoult's law?

Vapour pressure of water is $360 \mathrm{mm} \mathrm{Hg}$, how much urea should be added to $200 \mathrm{ml}$. water to reduce its vapour pressure by $0.5\%$? (Molecular weight of urea$=60$)

$30 \mathrm{g}$ of non volatile solute is dissolved in $360 \mathrm{g}$ of water at $100°\mathrm{C}$, if the vapour pressure of solution is $570 \mathrm{mm}$ of mercury then calculate molar mass of solute​.

$2 \mathrm{g}$ of each solute $\mathrm{A}$ and $\mathrm{B}$ (molar mass $\mathrm{A}>\mathrm{B}$) are dissolved separately in $20 \mathrm{g}$ each of the same solvents. Which will show the greater lowering in vapour pressure and why?

Derive the relationship between the relative lowering of vapour pressure and the mole fraction of the volatile liquid.

The vapour pressure of ethanol is $115$ torr at $34.9°\mathrm{C}$. if ${\mathrm{\Delta H}}_{\mathrm{vap} }$ of ethanol is $38.6 \mathrm{kJ}/\mathrm{mol}$. Calculate the temp. $\left({}^{\circ }\mathrm{C}\right)$ when then vapour pressure is $760$ torr.

The vapour pressure of ethanol is $115 \mathrm{torr}$ at $34.9°\mathrm{C}$ if $∆{\mathrm{H}}_{\mathrm{vap}}$ of ethanol is $38.6 \mathrm{kJ}/\mathrm{mol}$. Calculate the temperature $\left(°\mathrm{C}\right)$ when the vapour pressure is $760 \mathrm{torr}$. [Use relation $\mathrm{T} \mathrm{K} ={\mathrm{t}}^{°}\mathrm{C}+273$]

Show that relative lowering of vapour pressure for a solution is equal to the mole fraction of the solute when solvent alone is volatile.

Derive the relationship between the relative lowering of vapour pressure and the mole fraction of the non-volatile solute.