n moles of a non volatile solute are dissolved in wg of water. If `K_(f)` is the molal depression constant of water, the freezing point of the solution will be

One mole on non-volatile solute is dissolved in two mole of water. The vapour pressure of the solution relative to that of water is:

One mole of non-volatile solute is dissolved in two moles of water. The vapour pressure of the solution relative to that water of

One mole of non-volatile solute is dissolved in two mole of water. The vapour pressure of the solution relative to that of water is:

A solution of 1.25 g of a non-electrolyte in 20 g of water freezing at 271.9K with its molal depression constant , then the molecular wt. of the solute is:

The freezing point of a solution prepared from 1.25 g of non-electrolyte and 20 g of water is 271.9 K . If the molal depression constant is 1.86 K mol^(-1) , then molar mass of the solute will be

If molality of the dilute solution is doubled, the value of molal depression constant K_f will be