An unknown compound contains only c, h and o. combustion of 5.60g of this compound produced 11.18g of co2 and 4.58g of h2o. find the empirical formula.

Mass of CO2:
C=[11.18/(12.011+2x15.9994)]*12.011
and the moles
mass of H2O :
H=[4.58/(1.00794x2+15.9994)]/2*1.00794

Then subract: C-H=O (in grams.). O/15.9994=moles of O

11.18gCO2 x 12g/44g = 3.04gC
So 3.04C x I mol/12g = 0.254

D.na is the answer hope this