calculate the freezing point of a solution of a 3.46g of a compound, X, in 160g of benzene. when a separate of X was vaporised, its density was found to be 3.27g/L at 116 degree Celsius and 773 torr. The freezing point of pure benzene is 5.45 degree Celsius, and kf is 5.12 degree Celsius kg/mol

Answer 1

I assume comound X is not polar.
Use P*molar mass = dRT to find molar mass.
Then dT = Kf*m
m = mols/kg solvent. You know kg solvent and mols is g/molar mass.
That gives dT. Subtract from normal freezing point to find new f.p.
Post your work if you get stuck.

Answer 2

12

Answer 3

Calculate the freezing point of a soulution of 3.46 of a compoun

Answer 4

Student

Answer 5

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