An organic compound is composed of C, H and O. A 0.1005 g sample of this is combusted, producing 0.2829 g CO2 and 0.1159 g of H2O. What is the empirical formula of this compound? If the compound has a molar mass of 14 g/mol. What is the molecular formula?

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1. I got C10 H20 O but that makes the molar mass 156, not 146 :( am i doing something wrong?

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posted by Sim
2. Would you look at your post and confirm the molar mass of 14 g/mol. If you have the simplest formula possible of CHO, the molar mass of that is 12+1+16 = 29 so I don't believe 14.

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3. sorry, i made a typo, the question says that the compound has a molar mass of 146 g/mol

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posted by Sim
4. When you have a problem like this why don't you post your work and we tell at a glance what is wrong.
I worked the problem and obtained an empirical formula of 30 which gives a molecular formula of (CH2O)5 [or C5H10O5] for a molar mass of 150. I can help you through it if you get stuck.

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5. 5.6g of an organic compound on burning with excess of oxygen gave 17.6g of CO2 and 7.2g H2O. the formula of the compound is?

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posted by ASH

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