Ask Question
11 August, 20:34

A 10.00 g sample of a compound containing only carbon, hydrogen, and oxygen forms 23.98 g CO2 and 4.91 g H2O upon complete combustion. What is the empirical formula of the compound?

+1
Answers (1)
  1. 11 August, 21:10
    0
    There are three major steps for finding an empirical formula from a combustion reaction.

    1.) Determine the grams of carbon and hydrogen from the given data.

    C: 23.98 g x (12.011 g / 44.01 g) = 6.54 g C

    H: 4.91 g x (2.0158 g / 18.02 g) = 0.55 g H

    Determine the grams of oxygen in the sample by subtracting the mass of the compound given from the total mass solved earlier.

    O: 10.0 - (6.54 + 0.55) = 2.91 g O

    2) Convert the values in step 1 to moles.

    C: 6.54 g / 12.01 g / mol = 0.54 mol

    H: 0.55 g / 1.01 g/mol = 0.54 mol

    O: 2.91 g / 16.00 g/mol = 0.18 mol

    3) Divide each by the lowest value calculated in step 2

    C: 0.54 mol / 0.18 mol = 3

    H: 0.54 mol / 0.18 mol = 3

    O: 0.18 mol / 0.18 mol = 1

    Thus, the empirical formula is C3H3O.
Know the Answer?
Not Sure About the Answer?
Find an answer to your question ✅ “A 10.00 g sample of a compound containing only carbon, hydrogen, and oxygen forms 23.98 g CO2 and 4.91 g H2O upon complete combustion. What ...” in 📘 Chemistry if you're in doubt about the correctness of the answers or there's no answer, then try to use the smart search and find answers to the similar questions.
Search for Other Answers