The cryoscopic constant and freezing point of benzene is `"5.12 K kg mol"^(-1)` and 278.6 K respectively. At what temperature will one molal solution of benzene containing a nonelectrolyte `(i=1)` freeze? 

A molal solution is one that contains 1 mol of a solute in

The ebullioscopic constant for benzene is 2.52 K Kg mol^(-1) . A solution of an organic substance in benzene boils at 0.125^(@)C higher than benzene. Calculate the molality of solution?

A solution containing 0.1 mol of naphthalene and 0.9 mol of benzene is cooled out until some benzene freezes out. The solution is then decanted off from the solid and warmed upto 353 K where its vapour pressure was found to be 670 mm . The freezing point and boiling point of benzene are 278.5 K and 353 K respectively, and its enthalpy of fusion is 10.67 KJ "mol"^(-1) . Calculate the temperature to which the solution was cooled originally and the amount of benzene that must have frozen out. Assume ideal behaviour.

The freezing point of a 0.05 molal solution of a non-eletrolyte in water is ( K_(f)=1.86Km^(-1) )

The molal freezing point depression constant of benzene (C_(6)H_(6)) is 4.90 K kg mol^(-1) . Selenium exists as a polymer of the type Se_(x) . When 3.26 g of selenium is dissolved in 226 g of benzene, the observed freezing point is 0.112^(@)C lower than pure benzene. Deduce the molecular formula of selenium. (Atomic mass of Se=78.8 g mol^(-1) )

The freezing point of 0.02 mole fraction acetic acid in benzene is 277.4 K . Acetic acid exists partly as dimer. Calculate the equilibrium constant for dimerization. The freezing point of benzene is 278.4 K and the heat the fusion of benzene is 10.042 kJ mol^(-1) . Assume molarity and molality same.

(a) 10 g of non-electrolyte solute dissolved in 50 g of benzene lowered the freexing point of benzene by 0.4 K. Find the molar mass of the solute.[Given : Freezing point depression constant of benzene = 5.12 K. kg mor^(-1)] (b) How solubility of a gas in liquid varies with (i) Temperature and (ii) pressure?

A very small amount of a non-volatile solute (that does not dissociate) is dissolved in 56.8 cm^(3) of benzene (density 0.889 g cm^(3)) . At room temperature, vapour pressure of this solution is 98.88 mm Hg while that of benzene is 100 mm Hg . Find the molality of this solution. If the freezing temperature of this solution is 0.73 degree lower than that of benzene, what is the value of molal the freezing point depression constant of benzene?