1.00 g of a non-electrolyte dissolved in 50.5g of benzene lowered its freezing point by 0.40K. The freezing point depression constant of benzene is "5.12K.kg mol"^(-1). Find the molecular mass of the solute.

1.00 g of a non-electrolyte dissolved in 50.5g of benzene lowered its

1.	1.00 g of a non-electrolyte dissolved in 50.5g of benzene lowered its freezing point by 0.40K. The freezing point depression constant of benzene is "5.12K.kg mol"^(-1). Find the molecular mass of the solute.
Answer» Solution :`DeltaT_(f)=0.40K` `K_(f)="5.12 kg mol"^(-1)` `W_(2)=1G` `W_(1)="50.5 GM "=(50.5)/(1000)kg` `M_(2)=(K_(f))/(DeltaT_(f))xx(W_(2))/(W_(1))` `therefore""M_(2)=(5.12)/(0.40)xx(1)/(50.5)xx1000` `="2.56 g mol"^(-1)` Thus, the molecule mass of the solute `=" 256 g mol"^(-1)`.