A 27.0 g sample of an unknown hydrocarbon compound (containing carbon and hydrogen only) was burned in excess oxygen to form 88.0 g of CO2 and 27.0 g of H2O. Identify which of the following is a possible molecular formula for the hydrocarbon.

A 2.554-g sample of a certain hydrocarbon is burned in excess oxygen, producing 8.635 g CO2(g) and 1.768 g H2O(l). If the molecular weight of the hydrocarbon is found to be 78.11 u, what is its molecular formula? [m.w. CO2 = 44.01 u; m.w. H2O = 18.02 u]

A 4.235 g sample of a hydrocarbon was burned in oxygen to give 3.810 g of H2O and 13.96 g of CO2. What is the empirical formula of the compound?

A 1.00 g sample of a compound containing carbon, hydrogen and oxygen undergoes complete combustion to produce 2.44 g of CO2 and 1.00 g of H2O. Determine the empirical formula of the compound.The lowest whole number ratio of atoms in the compound is:        C:  H: O:1Enter only whole numbers with one significant figure for C and H only; the number for oxygen is 1.

In an experiment, a sample of an unknown, pure gaseous hydrocarbon was analyzed. Results showed that thesample contained 6.000 g of carbon and 1.344 g of hydrogen.(a) Determine the empirical formula of the hydrocarbon.

A compound is found to contain 24.0 g carbon, 4.00 mol hydrogen and 1.204 × 1024 atoms of oxygen. What is the empirical formula of this compound? CH2OC2H4O2CH2O2C2H4O