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Problem 48 Hard Difficulty

A compound with the empirical formula $\mathrm{CH}_{4} \mathrm{O}$ was found in a subsequent experiment to have a molar mass of approximately 192 g. What is the molecular formula of the compound?

Answer

$\mathrm{C}_{6} \mathrm{H}_{24} \mathrm{O}_{6}$

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Top Chemistry 101 Educators
TD
Theodore D.

Carleton College

Nadia L.

Rice University

KS
Karli S.

Numerade Educator

Jake R.

University of Toronto

Video Transcript

in this question, we're asked to find a compound with the empirical formula ch 40 given that the compound has a molar mass of around 192 grams per mole. So again, I'll just go to this one more time. A good way to find this is if we know the molecular weights of them likely formula. We can divide it by the empirical weights of the empirical formula to find a whole number. Now, if you multiply this number by the empirical formula, we should find at the end the molecular formula. So let's go ahead and run through this real quickly. First, we want to find E W. The molecular weights of the empirical formula, so we know carbon as 12.11 grams for more four hydrogen ins going to come out to be four games from all. Oxygen is 16 grams for more. So if we add all these up, we find that the empirical wait is 32 0.0 11 grams promote were also given that the molecular weight is 192 grams from, so let's go ahead and find that whole number and we find that the whole number is six. So we take this whole number and we multiply it by the empirical formula and we come out to C six h 24 06

Ohio State University
Top Chemistry 101 Educators
TD
Theodore D.

Carleton College

Nadia L.

Rice University

KS
Karli S.

Numerade Educator

Jake R.

University of Toronto