At 300K, 10 gm of a solute dissolved in 100gm of benzene showed a lowering of 8.8 mm in benzene. Calculate the mass of solute [Vapour pressure of pure Benzene is 121.8 mm at 300K]

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

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

2.0 g of a non-electrolyte solute dissovled in 100 g of benezene lowered the freezing point of benzene by 0.4^@C . If the freezing point depression constant of benezene is 5.12 K kg mol^(-1) . Calculate the molar mass of solute.

2.0g of a non-electrolyte dissolved in 100g of benzene lowers the freezing point of benzene by 1.2K. The freezing pont depression constant of benzene is 5.12 K kg mol^(-1) . The molar mass of the solute is

A solution containing 25. 6 gm of sulphur dissolved in 1000 gm of napthalene gave a freezing point lowering of 0.680, then molecular formula of sulphare is (K_(f) for naphthalene=6.8K kg mol^(-1) )

When 25 g of a non-volatile solute is dissolved in 100g of water, the vapour pressure is lowered by 2.25 xx 10^(-1)mm . If the vapour pressure of water at 20^(@)C is mm, what is the molecular weight of the solute?

At 273K, 100cm^(3) of a solution contaning 3gm of an unidentified solute exhibits an osmotic pressure of 2.24 atm , them molar mass of the solute is

Calculate the vapour pressure of a solution containing 10gm of non-volatile solute in 80gm of ethanol of at 298K [The vapour pressure of pure ethanol at 298K is 22.45 mm and Molecular weight of solute is 120]