Hi. I need help on a stoichiometry problem: When a particular hydrocarbon was burned in air, 0.467g of CO, 0.733g of CO2, and .450g of H2O were formed. The question asks me to find the empirical formula of the hydrocarbon and the number of grams of O2 used in the reaction. The answers are C2H3(empirical formula) and 1.19g of O2, but I don't understand how to get the answers. So far, I tried to find the empirical formula by finding out the number of moles of each compound. I got .017 mol Co, .017 mol CO2, and .025 mol water. So using this information, I was able to get a chemical equation of [tex]Unknown Hydrocarbon + 9O_2 \rightarrow 4CO + 4CO_2 + 6H_2O[/tex] But I don't know how to get the empirical formula from that. Is this the correct step to take? Or should I try something else? Thanks.