Calculate the mass in grams of an impurity ofmolar mass `100 g mol^(-1)` which would be required to raise the boiling point of 50 g of chloroform by 0.30 K (Kb for chloroform `3.63 K kg mol^(-1))`.

Calculate the freezing point of solution prepared by dissolving 4.5 g of glucose (molar mass = 180 g mol^(-1)) in 250 g of bromoform. Given, freezing point of bromoform = 7.8^@C and K_f for bromoform = 14.4 K kg mol^(-1) .

Calculate the volume in litres of 49.8 g of HCl gas at STP (Molar mass of HCl =36.5 g mol^-1) .

The Molarity of urea ( molar mass 60 g mol ^(-1) ) solution prepared by dissolving 15 g urea in 500 cm^(3) of water is ______.

The boiling point of 0.1 molal K_4 [Fe(CN)_6 ] solution will be (given K_b for water = 0.52 k kg mol^(-1))

Calculate the volume in litres occupied by 7.4g of ammonia at STP(molar mass of NH_3 = 17 g mol^-1 ).

The depression of freezing point of a solvent (b.p:303 K) for a particular solution is 0.153 K. Calculate the molal elevation constant if the boiling point of the solution is 304.52 K .(K_(f) =1.68 K kg mol ^(-1))

Calculate the mass of potassium chlorate required to librate 6.72 dm^3 of oxygen at STP, molar mass of potassium chlorate is 122.5 g /mol .

The depression of freezing point of watar for a particular solution is 0.186 K. The boiling point of the same solution is _______. (K_(f)= 1.86K kg mol^(-1) and K_(b)= 0.512 K kg mol^(-1))

How many grams of KCI should be added to 1000 g of water , so that the freezing point reduces to - 10^(@)C? (K_(f) "for water "=1.86""^(@)C kg mol ^(-1))

3.795 g of sulphur is dissolved in 100 g of carbon disulfide. This solution boils at 319.81K. What is the molecular formula of sulphure in solution? The boiling point of the solvent is 319.45K. (Given that Kb for CS2 = 2.42 K kg mol(-1) and atomic mass of S = 32)