posted by arcos15 on .
A 0.02847 g sample of gas occupies 10.0-mL at 292.0 K and 1.10 atm. Upon further analysis, the compound is found to be 38.734% C and 61.266% F.
What is the MOLECULAR formula of the compound?
Take a 100 g sample.
61.266 g F.
38.734 g C.
mols C = 38.734/12.015 = ?
mol F = 61.266/190 = ?
Find the ratio of the two elements to each other and calculate the molar mass of the empirical formula.
Then use PV = nRT and solve for n.
From n you can calculate the molar mass by n = grams/molar mass.
Finally, empirical mass x ? = molar mass; solve for ?, and the molecular formula is (empirical formula)?
you should end up with C2F2