A 0.5438 g sample of a compound contains only C H and O was burned completely in oxygen.the products were 1.0390 g CO2 and 0.6369g H2O. Determine the empirical formula of thr compound

Answer 1

g C = 1.0390g CO2 x (atomic mass C/molar mass CO2) = ?
g H = 0.669 g H2O x (2*atomic mass H/molar mass H2O) = ?
g O = 0.5438-gC-gH = ?

Then mols C = grams C/atomic mass C = ?
mols H = grams H/atomic mass H = ?
mols O = grams O/atomic mass O = ?

Now find the whole number ratio of C:H:O
Post your work if you get stuck.

Answer 2

C6H1803

Answer 3

what is the difference between atomic mass and molecular mass? Isn't the atomic mass and molecular mass of carbon 12?