Mixtures and Alligation

100 mL aqueous solution of glucose with osmotic pressure 1.2 atm at $25^oC$ is mixed with 300 mL aqueous solution of urea at 2.4 atm at $25^oC$. Calculate the osmotic pressure of mixture.

At $300\ K$, two pure liquids $A$ and $B$ have vapour pressures $150\ mm\ Hg$ and $100\ mm\ Hg$ respectively. In an equimolar liquid mixture of $A$ and $B$, the mole fraction of $B$ in the vapour mixture at this temperature is:

Two liquids a and b are mixed in 1: 4-mole ratio to form an ideal solution if pure liquid and a b exert a vapour pressure of 75 mmHg and 22 mmHg, the vapour pressure of liquid a in vapour phase would be

A gaseous mixture contains $56\ g\ N_{2}. 44\ g\ CO_{2}$ and $16\ g\ CH_{4}$. The total pressure of the mixture is $720\ mm\ Hg$. The sum of individual pressures of the gases is:

Equal mass of $H_2$, $He$ and $CH_4$ are mixed in empty container at $300$K, when total pressure is $2.6$ atm. The partial pressure of $H_2$ in the mixture is:

The vapour pressure of pure liquid $A$ at $300\ K$ is $577\ Torr$ and that of pure liquid $B$ is $390\ Torr$. These two compounds form ideal liquid and gaseous mixtures. Consider the equilibrium composition of a mixture in which the mole fraction of $A$ in the vapour is $0.35$. Find the mole % of $A$ in liquid.

The vapour pressure of the solution of two liquids $A(p^o = 80 mm)$ and $B(p^o = 120 mm)$ is found to be 100 mm when $x_A = 0.4$. The result shows that:

The vapour pressure of $C_6H_6$ and $C_7H_8$ mixture at $50^{\circ}C$ is given by $p=179X_B+92$ where $X_B$ is the mole fraction of $C_6H_6$. Calculate (in mm) Vapour pressure of liquid mixture obtained by mixing $936 \, g\ C_6H_6 \, $ and $736\ g$ toluene is:

Vapour Pressure of a mixture of benzene and toluene is given by $P= 179X_{B} + 92$, Where $X_{B}$ is mole fraction of benzene. If Vapours are removed and condensed in to liquid then what will be the ratio of mole fraction of benzene and toluene in first condensate :

A mixture of chlorobenzene and wate (immiscible) boils at $90.3^oC$ at an external pressure of 740.2 mm. The vapour pressure of pure water at $90.3^oC$ is 530.1 mm. Calculate the % composition of distillate :

A solution containing 30 g of a non-volatile solute in exactly 90 g water has a vapour pressure of 21.85 mm of Hg at $25^oC$. Further 18 g of water is then added to the solution, the new vapour pressure becomes 22.15 mm Hg at $25^oC$. Calculate : (a) Molar mass of solute (b) Vapour pressure of water at $25^oC$