Determine the mass of co2 and the mass of h2o produced by the combustion of 1.15 g of a compound with the empirical formula ch4o.

CO2 = 1.580 grams H2O = 0.592 grams Lookup the molar mass of each element in the compound Carbon = 12.0107 Hydrogen = 1.00794 Oxygen = 15.999 Calculate the molar mass of CH4O by adding the total masses of each element used. 12.0107 + 4 * 1.00794 + 15.999 = 32.04146 Now calculate how many moles of CH4O you have by dividing by the molar mass. m = 1.15 g / 32.04146 g/mole = 0.035891 mole Now figure out how many moles of carbon and hydrogen you have. Carbon = 0.035891 moles Hydrogen = 0.035891 moles * 4 = 0.143564 moles For Carbon Dioxide, you need 2 moles of oxygen per mole of carbon. So the mass of the carbon dioxide will be 0.035891 * 12.0107 + 2 * 0.035891 * 15.999 = 1.579516 grams For water, you need 1/2 mole of oxygen per mole of hydrogen. So the mass of H2o will be 0.035891 * 1.00794 / 2 + 0.035891 * 15.999 = 0.592308 grams

The answer is 65.3312

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