Addition of 0.643g of a compound to 43.95g of benzene lowers the freezing point from `5.51^@`C to `5.03^@`C. If `K_f` for benzene is 5.12K kg `mol^-1` , calculate the molar mass of the compound.

35 g of compound is added in 1 kg of water so that the resulting solution freezes at - 10^(@) C . If K_(f) for water = 1. 86 K/m . Calculate the molecular mass of the compound

18 g of a compound is dissolved in 10 kg of water so that the resulting solution freezes at - 8^(@) C . If K_(f) for water = 1 . 86 K/m . Calculate the molecular mass of the compound

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

2.1 g of non-electrolyte solute (molar mass 250 g/mol) was dissolved in 5.12 g of benzene. If the freezing point of depression constant, k_f of benzene is 5.12 K kg/mol, Calculate the freezing point of benzene.

Caculate the mass of a compound (molar mass=256g mol^-1) to be dissolved in 75g of benzene to lower its freezing point by 0.48K (K_f=5.12 K kg mol^-1)

Two elements A and B form compounds having formula AB2 and AB4. When dissolved in 20 g of benzene (C_6H_6), 1 g of AB_2 lowers the freezing point by 2.3 K whereas 1.0 g of AB_4 lowers it by 1.3 K. The molar depression constant for benzene is 5.1 K kg mol^(-1) . Calculate atomic masses of A and B.

On dissolving 3.24g of sulphur in 40g of benzene, boiling point of solution was higher than that of benzene by 0.81K. K_b value for benzene is 2.53K kg mol^-1 . What is the molecular formula of sulphur? (Atomic mass of sulphur=32 g mol^-1) .

1 g of non - electrolyte solute (molar mass 250 g/mol) was dissolved in 5.12g of benzene. If the freezing point of depression constant, k_f of benzene is 5.12 K kg/mol, the freezing point of benzene will be lowered by