When 4.673 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 16.05 grams of CO2 and 2.628 grams of H2O were produced. In a separate experiment, the molar mass of the compound was found to be 128.2 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon.
When 4.673 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 16.05 grams of CO2 and 2.628 grams of H2O were produced. In a separate experiment, the molar mass of the compound was found to be 128.2 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon.
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Question
When 4.673 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 16.05 grams of CO2 and 2.628 grams of H2O were produced.
In a separate experiment, the molar mass of the compound was found to be 128.2 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon.
Expert Solution
Step 1
Given: Mass of compound burned = 4.673 g.
Mass of CO2 produced = 16.05 g.
Mass of H2O produced = 2.628 g.
And the molar mass of compound = 128.2 g/mol.
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