When a non volatile solute is added to a solvent, the vapour pressure of the solution decreases. Let xA be the mole fraction of the solvent, xB be the mole fraction of the solute and pAo be the vapour pressure of the pure solvent and p be the vapour pressure of the solution.
Since solute is non volatile, there will be no contribution of the solute to the vapour pressure and the vapour pressure of the solution will only be due to the solvent. Therefore, the vapour pressure of the solution p will be equal to the vapour pressure of the solvent pA, over the solution.
Thus lowering in vapour pressure is given as,
pA = pAo - pA = pAo - pAo xA (from Raoult's Law)
Since, xA = 1 - xB
So that,
pA = pAo - pAo (1-xB)
Rearranging terms we get,
Thus, the relative lowering in vapour pressure of an ideal solution containing the non volatile solute is equal to the mole fraction of the solute at a given temperature.