The vapour pressure of two pure liquids $(A)$ and $(B)$ are $100 \ torr$ and $80 \ torr$ respectively. The total pressure of the solution obtained by mixing $2 \ mole$ of $(A)$ and $3 \ mole$ of $(B)$ would be ........ $torr$.

Write the formula which expresses the relationship between the total pressure of a solution $(P_{total})$ and the mole fraction $(x_2)$ of the components,according to Raoult's law.

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

When a certain amount of solid $A$ is dissolved in $100 \ g$ of water at $25^{\circ} \ C$ to make a dilute solution,the vapour pressure of the solution is reduced to one-half of that of pure water. The vapour pressure of pure water is $23.76 \ mm \ Hg$. The number of moles of solute $A$ added is $...........$ (Nearest Integer).

Vapour pressure of $CCl_4$ at $25 \text{ }^\circ\text{C}$ is $143 \text{ mm Hg}$. If $0.5 \text{ g}$ of a non-volatile solute is dissolved in $100 \text{ cm}^3$ of $CCl_4$, find the vapour pressure of the solution. (Density of $CCl_4 = 1.58 \text{ g/cm}^3$ and molar mass of solute = $65 \text{ g/mol}$) (in $\text{ mm Hg}$)

The vapor pressure of a liquid mixture of $X$ and $Y$ is given by the equation $P = 160X_x + 50$,where $X_x$ is the mole fraction of $X$. The ratio of the vapor pressures of pure liquids $X$ and $Y$ is: