The boiling point of benzene is 353.23K. When 1.80g of a non-volatile solute was dissolved in 90g of benzene, the boiling point is raised to 354.11K. Calculated the molar mass of the solute `k_b` for benzene is 2.53K kg `mol^(-1)`

The boiling point of a pure liquid is 353.23 K. When 1.80 g of a non-volatile solute is dissolved in 90 g of this pure liquid, the boiling point becomes 354.11 K. The molar mass of the solute is (given that the boiling point elevation constant function of the pure liquid is 2.53 K. kg. mol^-1 )

0.48g of a substance was dissolved in 10.6 g C_6H_6. The freezing point of benzene was lowered by 1.8^@C. Calculate molar mass of the substance. Molecular depression constant for benzene is "5K kg mol"^(-1) .

1.00g of a non-electrolyte solute dissolved in 50g of benzene lowered by 0.40K. The freezing point depression constant of benzene is 5.12K kg//mol . Find the molar mass of solute.

An aqueous solution of '2 %' non-volatile sol ute exerts a pressure of 1.004 bar at the nor mal boiling point of the solvent. What is the molar mass of the solute?

1.00g of a non-electrolyte solute dissolved in 50g of benzene lowered the freezing point of benzene by 0.40K. Freezing point depression constant of benzene is 5.12K g//mol . Find the molar mass of solute. .

A solution containing 0.1 g of a non-volatile organic substance P (molecular mass 100) in 100 g of benzene raises the boiling point of benzene by 0.2^@C, while a solution containing 0.1 gof another non-volatile subistance Q in the same amount of benzene raises the boiling point of benzene by 0.4^@C . What is the ratio of molecular masses of P and Q?

When 1 mole of a solute is dissolved in 1 kg of H_(2)O , boilling point of solution was found to be 100.5^(0)C . K_(b) for H_(2)O is

The vapour pressure of a 10% aqueous solution of a non volatile substance at 373K is 740 mm of Hg. Calculate the molecular mass of the solute.