A solution containing 7g of a solute (molar mass `210 "g mol"^(-1)`) in 350g of acetone raised the boiling point of acetone from `56^(@)C` to `56.3^(@)C`. The value of ebullioscope contant of acetone in `"K kg bol"^(-1)` is :

A solution containing 0.73 g of camphor ( molar mass 152 g "mol"^(-1) ) in 36.8 g of acetone ( boiling point 56.3^(@)C) boils at 56* 55^(@)C . A solution of 0.564 g of unknown compound in the same weight of acetone boils at 56.46^(@)C . Calculate the molar mass of the unknown compound .

10 g of solute with molecular mass 100 g mol^(-1) dissolved in 100 g of solvent to show 0. 3^@ elevation in boiling point. The value of molal ebullioscopic constant will be

A solution contains 0.524 g of camphor ( molar mass = 152 g/ mol dissolved in 36.8 g of ether (boiling point =34.6^(@) C) . The molal elevation constant per 100 g of ether is 19.4 K kg mol ^(-1) . The boiling point of the solution is _______.

If 1 g of solute (molar mass = 50 g mol^(-1) ) is dissolved in 50 g of solvent and the elevation in boiling point is 1 K. The molar boiling constant of the solvent is

If 1 g of solute (molar mass = 50 g mol^(-1) ) is dissolved in 50 g of solvent and the elevation in boiling point is 1 K. The molar boiling constant of the solvent is

Calculate the boiling point of solution containing 0.456g of camphor (molar mass =152 ) dissolved in 31.4g of acetone (boiling point =56.30^(@)C ), if the molar elevation constant per 100g of acetone is 17.2^(@)C.