When one mole of solute is dissolved in `"1kg"` of water,the boiling point of water is determined as `100.5^(@)C` .Then `"Kb"` of water is

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

Solute when dissolved in water:

0.1 gram mole of urea dissolved in 100 g of water. The molality of the solution is

One mole of non-volatile solute is dissolved in two mole of water. The vapour pressure of the solution relative to that of water is:

Elevation in boiling point was 0.52^(@)C when 6 g of a compound X was dissolved in 100 g of water. Molecular weight of X is ( K_(b) of water is 5.2^(@)C per 100 g of water)

The boiling point of a glucose solution containing 12 g of glucose in 100 g of water is 100.34^@C . Boiling point of water is 100^@C . The molal elevation constant of water is

One moles of strem is compressed reversibly of water at boiling point 100^(@)C . The heat of vapourisation of water at 100^(@)C and 1atm is 540cal g^(-1) . Calculate DeltaU and DeltaH .