$1.00 \text{ g}$ of a non-electrolyte solute dissolved in $50 \text{ g}$ of benzene lowered the freezing point of benzene by $0.40 \text{ K}$. The freezing point depression constant of benzene is $5.12 \text{ K kg mol}^{-1}$. Find the molar mass of the solute.
- A$280 \text{ g mol}^{-1}$
- B$356 \text{ g mol}^{-1}$
- C$562 \text{ g mol}^{-1}$
- D$256 \text{ g mol}^{-1}$
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Similar Questions
The freezing point of a $0.01 \ m$ aqueous glucose solution is $-0.18^\circ C$. If an equal volume of $0.002 \ m$ glucose solution is added to it,the freezing point of the resulting solution will be ...... $^\circ C$.
Medium
View Solution$A$ solvent freezes at $17^{\circ} C$ and it has a latent heat of fusion of $180 \ J \ g^{-1}$. The molal depression constant $(K_{f})$ of the solvent is (in $K \ kg \ mol^{-1}$):
What is the relation between the depression in freezing point and the molar mass of a non-volatile solute?
Give the formula which shows the relation between the freezing point and the fusion enthalpy of a solvent.
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View SolutionDuring the depression in freezing point experiment, an equilibrium is established between the molecules of
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