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A solutionof 2.50g of a compound having the empirical formula C7H6O2 in 25.0g of benzene is observed to freeze at 4.3 degree C.Calculate the molar mass of the solute and its Molecular formula
College Chemistry2 -
Look up normal freezing point benzene.
Look up freezing point constant for benzene (Kf = ?).
delta T = Kf*molality
Solve for molality.
molality = moles/kg solvent
Solve for moles
moles = grams/molar mass
Solve for molar mass.
Find the mass of the empirical formula.
(molar mass/empirical mass) = ?? and round to the nearest whole number and call that number n. The molecular formula is (empirical formula)n.