Chemistry Homework Help?
Complete combustion of 5.30g of a hydrocarbon produced 16.9g of CO2 and 6.06g of H2O. What is the empirical formula for the hydrocarbon? Insert subscripts as necessary.
The answer I got was C3H5 but it keeps telling me I am incorrect.
- pisgahchemistLv 73 weeks agoFavorite Answer
CxHy + O2 --> CO2 + H2O ............... not balanced
5.30g ............. 16.9g...6.06g
16.9g CO2 x (1 mol CO2 / 44.0g CO2) x (1 mol C / 1 mol CO2) = 0.384 mol C
6.06g H2O x (1 mol H2O / 18.0g H2O) x (2 mol H / 1 mol H2O) = 0.337 mol H
0.384 mol C / 0.337 = 1.14 mol C
0.337 mol H / 0.337 = 1.00 mol H
Either the numbers are very sloppy and the empirical formula is CH, or we need to multiply the moles by 7 to get whole numbers.
1.14 x 7 = 7.98 ~ 8 mol C
1.00 x 7 = 7 mol H
empirical formula = C8H7