Combustion analysis of a hydrocarbon produced 33.01 g CO2 and 4.84 g H2O.
I was asked to find the empirical formula of the hydrocarbon. I used these molar mass values for my calculations:
C - 12.0107
H - 1.00794
O - 15.9994
Here is my work:
Molar mass of CO_2 = 12.0107 + 2*15.9994 = 44.0095 Molar mass of H_2O = 2*1.00794 + 15.9994 = 18.01528
We now have 33.01g of CO2 and 4.84g of H2O, which means:
33.01/44.0095 = 0.750 mol CO_2 4.84/18.01528 = 0.26866 mol H_2O 0.26866*2 = 0.53732 mol H
From the calculation we know that the ratio of C to H is 0.750:0.537, which is approximately 3:2. However, the empirical formula C3H2 is not the right answer. Can anyone tell me why I am wrong? Thank you!