Question

2) A 1.000 g sample of a hydrocarbon (which is a compound that contains only carbon and hydrogen) was burned in oxygen, and the carbon dioxide and water produced were carefully collected and weighed. The mass of the carbon dioxide was 3.385 g, and the mass of the water was 0.692 g. What was the empirical formula of the hydrocarbon? A. C5H12 B. CsH6 C. CįH6 D. C H2 E. CįH star 1.00

Answer 1

given data: 19 of hydrocarbon burned in oxygen, of H₂O. of CO2 and 0.6929 g gives 3.38 i Number of moles of CO2 = mass of CO2 molar mass OSCO = 3.385 = 0.0769318 44 mass of H2O molar mass of H2O Number of moles of 20 0.692. -0.038444 18 since Imole of co no. of moles of has Imole of c. C in co2 = OV 0769318 of H in H₂O = 2x0.0384444 = 0.0768888 of moles Number Divide by Smallest: = (00055 C C: 0.0769318 0.0768888 = 1. 0.076 8888 0.0768888

c=1, H=1. i empirical formulae = C,H,