1.) In order to determine the moles of carbon in the compound, first determine the moles of carbon dioxide that were produced from the combustion. 2.) Determine the moles of carbon present in carbon dioxide. This will be the same number of moles of carbon in the original compound. 3.) In order to determine the moles of hydrogen in the compound, first determine the moles of water that were produced from the combustion. 4.) Determine the moles of hydrogen present in the water. This will be the same number of moles of hydrogen in the original compound. 5.) Calculate the mass of oxygen in the original compound. You will need to subtract the mass of the carbon that ended up in the carbon dioxide and the mass of the hydrogen that ended up in the water from the mass of the original compound. 6.) Determine the number of moles of oxygen in the original compound 7.) Determine the empirical formula of the unknown compound
A compound containing only carbon, hydrogen, and oxygen is analyzed using combustion analysis. When 80.9 g of the compound is burned, 148.2 g of carbon dioxide and 40.5 g of water are collected.
1.) In order to determine the moles of carbon in the compound, first determine the moles of carbon dioxide that were produced from the combustion.
2.) Determine the moles of carbon present in carbon dioxide. This will be the same number of moles of carbon in the original compound.
3.) In order to determine the moles of hydrogen in the compound, first determine the moles of water that were produced from the combustion.
4.) Determine the moles of hydrogen present in the water. This will be the same number of moles of hydrogen in the original compound.
5.) Calculate the mass of oxygen in the original compound. You will need to subtract the mass of the carbon that ended up in the carbon dioxide and the mass of the hydrogen that ended up in the water from the mass of the original compound.
6.) Determine the number of moles of oxygen in the original compound
7.) Determine the empirical formula of the unknown compound
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