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?
5 answers
I got C10 H20 O but that makes the molar mass 156, not 146 :( am i doing something wrong?
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.
sorry, i made a typo, the question says that the compound has a molar mass of 146 g/mol
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.
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.
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?
2 answers