A 0.250 g sample of a hydrocarbon is burned completely in excess O2. The combustion products are passed through a dehydrating tube (gains 0.306 g) followed by a CO2 absorber (gains 0.747 g). The hydrocarbon contains only C and H.
A separate measurement gives a molar mass of 84 g/mol. What is the molecular formula?
- A
C5H10
- B
C7H14
- Ccheck_circle
C6H12
- D
CH2
Explanation
Empirical mass = 14 g/mol. 84/14 = 6 -> C6H12.