The boiling point of benzene is 353.23 K. When 1.809 of a non-volatile solute was dissolved in 90 g of benzene, the boiling point is raised to 354.11K. Calculate the molarmass of the solute. `K_b` for benzene is `2.53 K kg mol^(-1)`.

When 10 of a non-volatile solute is dissolved in 100 g of benzene . It raises boiling point by 1^(@)C then moler mass of the solute is ______. (if K_b = 2.53 ""^(@)C kg // mol )

The normal boiling point of ethyl acetate is 77.06^@C . A solution of 50 g of a nonvolatile solute in 150 g of ethyl acetate boils at 84.27^@C . Evaluate the molar mass of solute if K_b for ethyl acetate is 2.77^@C Kg Mol^(-1)

1.00 g of a non-electrolyte solute dissolved in 50 g of benzene lowered the freezing point of benzene of 0.40K. The freezing point depression constant of benzene is 5.12K kgmol^(-1) . Find the molar mass of the solute .

0.440 g of a substance dissolved in 22.2 g of benzene lowered the freezing point of benzene by 0.567 ^(@)C . The molecular mass of the substance is _____ (K_(f) = 5.12 ^(@)C kg mol ^(-1))

1.02 g of urea when dissolved in 98.5 g of certain solvent decreases its freezing point by 0.211K. 1.609 g of unknown compound when dissolved in 86 g of the same solvent depresses the freezing point by 0.34 K. Calculate the molar mass of the unknown compound.(molar mass of urea = 60 g/mol )

IF 10 g of solute was dissolved in 250 mL. of water and osmotic pressure of the solution was found to be 600 mm of Hg at 300 K, then molecular weight of the solute is _______. g mol ^(-1)