Asked by Ethio

Calculate the freezing point of a solution of 3.46 g of a compound,X,in 160 g of benzene. When separate sample of X was vaporised, its density was found 3.27 g/L at 116 c and 773 torr. The freezing point of pure benzen is 5.45 c, and kf is 5 .12 c/m.
Answered by DrBob222
First determine molar mass from
P*molar mass = density*R*T
Solve for molar mass. Then

moles = grams/molar mass
Solve for moles

molality = moles/kg solvent
Solve for molality

delta T = Kf*m
Solve for delta T, then convert to freezing point
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Calculate the freezing point of a solution of 3.46 g of a compound, X, in 160 g of benzene. When a separate sample of X was vaporised, its density was found to be 3.27 g/Lat 116°C and 773 torr. The freezing point of pure benzene is 5.45°C, and Kis 5.12°C kg/mol.
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