1. The problem statement, all variables and given/known data When a sample that is .91 grams is burned in oxygen, it produces 2.073 grams of carbon dioxide, .304 grams of water, and .0944 grams of nitrogen. What is the empirical formula of the compound? 3. The attempt at a solution I converted all of the products to moles: CO2: .0471 moles H2O: .0169 moles N2: .00337 moles. This gave me C.0471H.0338N.00674. Simplifying the ratios, I got C7H5N. My problem is that I don't have any idea of what to do with the oxygen. I don't even know if/how much of it it is present in the sample, because the sample is burned. Thanks in advance for any help.