1. The problem statement, all variables and given/known data A compound only contains C, H and O. An elemental analysis of the compound gives the result C: 40.00%; H: 6.71%. The 13C NMR, IR spectrum and mass spectrums are in the graph below. Graphs: http://s512.photobucket.com/albums/t323/antiuniverse/graphs.gif [Broken] I need to determine the name of the compound. 2. Relevant equations N/a 3. The attempt at a solution I'm not entirely sure. From the elemental analysis: If we had 100g of compound, we'd have: 40g C 6.71g H 53.29 O Work out the moles: 40g / 12 = 3.3333 moles of C 6.71g / 1 = 6.7100 moles of H 53.29g / 16 = 3.3306 moles of O Divide by smallest ratio: 2.8571 / 2.8571 = 1 atom of C 6.7100 / 2.8571 = 2 atoms of H 1.1652 / 2.8571 = 1 atom of O So the empirical formula would be H2CO (or C2H4O2?). I think the mass spectrum is telling me that the empirical formula must be H2CO (which has a molecular weight/mass of 30). From the 13C NMR spectra I believe it's either an aldehyde or ketone. I know that H2CO is formaldehyde (methanal) which is an aldehyde and correlates with what I found in the 13C NMR spectra. Could anybody look over this and let me know if it's correct?