3.0 g of non-volatile solute when dissolve in 1 litre water, shows an osmotic pressure of 2 atmosphere at 300 K. Calculate the molar mass of the solute. (R = 0.0821 litre atm `K^(-1)"mol"^(-1)`).

Decinormal solution of NaCl developed an osmotic pressure of 4.6 atm at 300K. Calculate the degree of dissociations.

Boiling point of benzene is 353.23 K . When 1 . 80 g of non-volatile solute was dissolved in 90 g of benzene the boiling point is raised to 354. 11 K? Calculate molar mass of solute . ( K_(b) for benzene is 2 . 53 K kg mol^(-1) )

10g of non-volatile solute when dissolved in 100g of benzene raises its boiling point by 1^@ C. What is the molecular mass of the solute. ( k_b for benzene=2.53 K kg mol^-1 )

The boiling point of Benzene (C_(6) H_(6)) is 353.23 K. When 1 . 80 g of a non - volatile solute was dissolved in 90 g of C_(6) H_(6) the boiling point is raised to 354 . 11 K. Calculate the molar mass of solute . (Given K_(b) for benzene is 2 . 53 K kg mol^(-1) )

200 cm^3 of an aqueous solution of a protein contains 1.26g of the protein . The osmotic pressure of such a solution at 300K is found to be 2.7 xx 10^-3 bar. Calculate the molar mass of the protein (R=0.083 L bar mol^-1 K^-1 )

Calculate the molar concentration of urea solution if it exerts an osmotic pressure of 2.45 atmosphere at 300K . (R=0.0821L atm mol^-1 K^-1 )

An aqueous solution of 2% non-volatile solute exerts a pressure of 1.004 bar at the normal boiling point of the solvent. What is the molar mass of the solute?

The osmotic pressure of 0.2 molar solution of urea at 27^@C (R=0.082 litre atm "mol"^(-1) K^(-1)) is

Calculate the osmotic pressure at 273K of a 5% solution of compound A. (molecular mass-60) (Given R= 0.0821 L atm K^-1mol^-1 )