The amount of solute (molar mass 60 g `mol^(-1)`) that must be added to 180 g of water so that the vapour pressure of water is lowered by `10%` is

The amount of solute (molecular mass 60 gmol^-1 ) that must be added to 180g water so that the vapour pressure of water is lowered by 10% is

The amount of solute (mol. Mass=60) that must be added to 180 g of water so that the vapour pressure of water is lowered by 10% is

How mich urea ("molar mass"=60 g mol^(-1)) must be dissolved in 50 g of water so that the vapour pressure at room temperature is reduced by 25% ? Also calculate the molality of the solution obtained.

What mass of solute ("molar mass=60 g mol"^(-1)) should be dissolved in 180 g water to reduce the vapour pressure to 4/5 th of pure water :

What is the mass of a non-volatile solute (molar mass 60) that needs to be dissolved in 100 g of water in order to decrease the vapour pressure of water by 25%. What will be the molality of the solution?

Calculate the amount of CaCl_(2) (molar mass = 111g "mol"^(-1) ) which must be added to 500 g of water of lower its freezing point by 2K, assuming CaCl_(2) is completely dissociated. (Kf for water = 1.86 k kg "mol"^(-1) ).

Six grams of urea ( molar mass = 60 ) are dissolved in 90 g of water. The relative lowering of vapour pressure is equal to