17. The vapour pressure of a solution in benzene is 722mm and that of solvent is 760mm. What is the Molality of the solution

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Q. The vapour pressure of a solution in benzene is 722 mm and that of pure solvent (benzene) is 760 mm. The molality of solution is :

Q. The vapour pressure of pure benzene is 639.7 mm Hg and the vapour pressure of a solution of a solute in benzene at the temperature is 631.9 mm Hg. If the molality of the solution is

156 \times 10^{- x}

, then what is the value of

x

The vapour pressure of Benzene at $25^{\circ}$ is 639.7mm of Hg. The vapour pressure of a solution of benzene at same temperature is 631.9 mm of Hg. The molality of solution is:

Q. Vapour pressure of pure benzene is

640 m m

and its mol. wt. is

78

. When

2.175 g

of a non-volatile substance is dissolved in

39 g

benzene the vapour pressure of the solution becomes

600 m m

. Calculate mol. wt. of solute.

Q. A very small mass of a non-volatile solute (that does not dissociate) is dissolved in

56.8 c m^{3}

of benzene (density is

0.889 g c m^{- 3})

. At room temperature, vapour pressure of this solution is 98.88 mm Hg, while that of benzene is 100 mm Hg. Find the molality of this solution. If the freezing temperature of this solution is 0.73 degree lower than that of benzene, what is the value of molal depression constant of benzene?

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