Asked by niki
A 7.85 g sample of a compound with the empirical formula C5H4 is dissolved in 301 g of benzene. The freezing point of the solution is 1.05C below that of pure benzene. what are the molar mass and molecular formula of this compound?
Answers
Answered by
DrBob222
delta T = Kf*m
You know delta T and Kf, solve for molality.
Then molality = mols/kg solvent. You know m and kg solvent, solve for mols.
Then mols = grams/molar mass. You know mols and grams, solve for molar mass.
The empirical formula is C5H4. Calculate the empirical formula mass.
empirical formula mass x n = molar mass.
The molecular formula then is
(emprical formula)<sub>n</sub>
You know delta T and Kf, solve for molality.
Then molality = mols/kg solvent. You know m and kg solvent, solve for mols.
Then mols = grams/molar mass. You know mols and grams, solve for molar mass.
The empirical formula is C5H4. Calculate the empirical formula mass.
empirical formula mass x n = molar mass.
The molecular formula then is
(emprical formula)<sub>n</sub>
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.