A solution containing 28 g phosphorus in 315 g `CS_2` (b. pt. `46.3^@C`) boils at `47.98^@C.K_b` for `CS_2` is 2.34 K `mol^-1` kg. Calculate m.wt. of phosphorus and deduce its molecular formula. Assume its complete association.

2.56 g of sulphur in 100 g of CS_2 has depression in freezing point of 0.010^@ . K_(f)=0.1^(@) kg (mol)^(-1) . Hence atomicity of sulphur in the solution is

A solution containing 2.5 g of a non-volatile solute in 100 gm of benzene boiled at a temperature 0.42K higher than at the pure solvent boiled. What is the molecular weight of the solute? The molal elevation constant of benzene is "2.67 K kg mol"^(-1) .

A solution of 1.25 g of 'P' in 50g of water lowers freezing point by 0.3^@C . Molar mass of 'P' is 94. K_f(water) is 1.86 K kg mol^(-1). The degree of association of 'P' in water is [Assume dimerisation of P]

At a temperature of 273K and 1 atm pressure 1L of a gas weighs 2.054g. Calculate its molecular mass.

For a dilute solution containing 2.5 g of a non-volatile non-electrolyte solute in 100 g water, the elevation of boiling point at 1 atm pressure is 2°C. Assuming concentration of solute is much lower than the concentration of solvent, determine the vapour pressure (mm Hg) of the solution. [Given: k_b for water = 0.76K-kg- mol^(- 1) ]

0.900g of a solute was dissolved in 100 ml of benzene at 25^(@)C when its density is 0.879 g/ml. This solution boiled 0.250^(@)C higher than the boiling point of benzene. Molal elevation constant for benzene is "2.52 K.Kg.mol"^(-1) . Calculate the molecular weight of the solute.

The mole fraction of a solute in a binary solution is 0.1. At 298 K, molarity of this solution is same as its molality. Density of this solution at 298 K is 2.0 g cm^(-3) . The ratio of molecular weights of the solute and the solvent (M_("solute")//M_("solvent")) is

The boiling point of a solution containing 1.5 g of dichlorobenzene in 100 g of benzene was higher by 0.268^@C . Calculate the molar mass of dichlorobenzene. K_b forbenzene = 2.42 K kg mol^-1