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?

A very small amount of a non-volatile solute (that does not dissociate

1.	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?
Answer» `(Deltap)/(p_(0))=x_(B)` `(100-98.8)/(100)=x_(B)` `x_(B)=0.012` Molality `= (x_(B)xx1000)/((1-x_(B))m_(A))=(0.012xx1000)/(0.988xx78)=0.1557` `DeltaT=K_(f)xx` Molality `0.73=K_(f)xx0.1557` `K_(f)=4.688`.

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