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» <html><body><p></p>Solution :`DeltaT_(f)=0.40K` <br/> `K_(f)="5.12 kg mol"^(-1)` <br/> `W_(2)=<a href="https://interviewquestions.tuteehub.com/tag/1g-282964" style="font-weight:bold;" target="_blank" title="Click to know more about 1G">1G</a>` <br/> `W_(1)="50.5 <a href="https://interviewquestions.tuteehub.com/tag/gm-1008640" style="font-weight:bold;" target="_blank" title="Click to know more about GM">GM</a> "=(50.5)/(1000)kg` <br/> `M_(2)=(K_(f))/(DeltaT_(f))xx(W_(2))/(W_(1))` <br/> `therefore""M_(2)=(5.12)/(0.40)xx(1)/(50.5)xx1000` <br/> `="2.56 g mol"^(-1)` <br/> Thus, the molecule mass of the solute `=" 256 g mol"^(-1)`.</body></html>