posted by kaliegh on .
An orgnaic compound contains C, H, No, and O. Combustion of 0.1023 g of the compound in excess oxygen yielded 0.2766 g of CO2 and 0.991g of H2O. A asample of 0.4831 g of the compound was analyzed for nitrogen by the Dumas method. At STP, 27.6 mL of dry N2was obtained. In a third experiment, t he density of the compound as a gas was found to be 4.02 g/ L at 127 degrees Celsius and 256 torr. What are the empirical and molecular formulas of the compound?
I believe you should check the numbers in your problem, particularly the number for grams H2O. I don't think it can be that much. Check the other numbers while you are at it.
please someone answer!!!!
Anyone figure this one out yet?