A small amount of a non-volatile solute is dissilved in `64.5 cm^(3) ` of acetone ( density `0.791 g//cm^(3) )` the vapour pressure of this solution at room temperature is 260 mm Hg , while that of acetone is 285 mm Hg . What is the molality of the solution ?

A very small amount of a non-volatile solute (that does not dissociate) is dissolved in 56.8 cm^(3) of benzene (density 0.889 g cm^(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 the freezing point depression constant of benzene?

A very small amount of a non-volatile solute (that does not dissociate) is dissolved in 56.8 cm^(3) of benzene (density 0.889 g cm^(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 the freezing point depression constant of benzene?

A very small amount of a non-volatile solute (that does not dissociate) is dissolved in 56.8 cm^(3) of benzene (density 0.889 g cm^(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 the freezing point depression constant of benzene?

A very small amount of a non-volatile solute (that does not dissociate) is dissolved in 56.8 cm^(3) of benzene (density 0.889 g cm^(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 the freezing point depression constant of benzene?

A very small amount of a nonvolatile solute (that does not dissociate) is dissolved in 56.8 cm^3 of benzene (density 0.889 g cm^-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 molar freezing point depression constant of benzene ?

A very small amount of non-volatile solute, non-electrolyte is dissolved in 50 cm^(3) of benzene (d=0.9 g cm^(-3)) . At room temperature, vapour prssure of this solution is 99 mm Hg while that of benzene is 100 Hg. If DeltaT_(f) is the 0.73 What is value of K_(f)?

The vapour pressure of water at room temperature is 30 mm of Hg. If the mole fraction of the water is 0.9, the vapour pressure of the solution will be :

The vapour pressure of water at room temperature is 30 mm of Hg. If the mole fraction of water in a solution of non volatile solute is 0.9, the vapour pressure of the solution will be :-