Question

`1.0 g` of non-electrolyte solute dissolved in `50.0 g` of benzene lowered the freezing point of benzene by `0.40 K`. The freezing point depression constant of benzene is `5.12 kg mol^(-1)`. Find the molecular mass of the solute.

Answer 1

Substituting the values of various terms involved in equation we get ,
`M_(2)=(5.12" K kg "mol^(-1)xx1.00gxx1000" g "kg^(-1))/(0.40xx50g)=256" g "mol^(-1)`
Thus, molar mass of the solute`=256" g "mol^(-1)`