Anthracene which contains only Carbon and hydrogen, is an important source of dyes. When 250 mg of anthracene is burned in pure oxygen, 8.64 mg of CO2 and 1.26 mg of H2O are formed. What is the empirical formula of anthracene?

Answer 1

The easist, I think, but a little longer is to convert to percent.
%C = 8.64 x (12/44)/250 = %C
12 is atomic mass C. 44 is molar mass CO2.

%H = 1.26 x (2*1/18)/250 = %H.
Then take a 100 g sample, convert to mols C and mols H and find the ratio. Post your work if you get stuck and I can help you throgh.

Answer 2

molar mass