Ask Question
24 March, 01:00

When 6.270 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 19.67 grams of CO2 and 8.055 grams of H2O were produced. In a separate experiment, the molar mass of the compound was found to be 56.11 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon.

+2
Answers (1)
  1. 24 March, 03:29
    0
    6.270/56.11 = 0.1117447870 / 0.1117 ... ≈ 1

    19.67/44.01 = 0.446943876 / 0.1117 ... ≈ 4

    8.055/18 = 0.4475 / 0.1117 ... ≈ 41 mole of compound forms 4 moles of both CO2 and H2O, so the empirical formula will be C4H8

    As this gives molar mass of 56.11, this is also the molecular formula

    This could be cyclobutane, or butene
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “When 6.270 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 19.67 grams of CO2 and 8.055 grams of H2O were ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers