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?
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.
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?
To find the empirical formula of the organic compound, we need to determine the ratio of carbon, hydrogen, and oxygen atoms in the compound based on the given combustion data.
1. Start by calculating the moles of carbon, hydrogen, and oxygen in the given samples of CO2 and H2O.
- Moles of CO2: 0.2829 g CO2 / molar mass of CO2 (44 g/mol)
- Moles of H2O: 0.1159 g H2O / molar mass of H2O (18 g/mol)
2. Use the given molar mass of the compound (14 g/mol) to find the total moles of carbon, hydrogen, and oxygen in the compound.
- Total moles = molar mass of the compound / 14 g/mol
3. Divide the total moles by the smallest mole value obtained in step 1 to find the mole ratio between carbon, hydrogen, and oxygen.
4. Round the mole ratio to the nearest whole number to obtain the empirical formula.
To find the molecular formula, you need additional information, such as the molecular weight of the compound. Without this information, we cannot determine the molecular formula from just the empirical formula and the molar mass.