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1) When 6.580 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 20.16 grams of CO2 and 9.631 grams of H2O were produced.
In a separate experiment, the molar mass of the compound was found to be 86.18 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon.
2)When 2.823 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 8.859 grams of CO2 and 3.627 grams of H2O were produced.
In a separate experiment, the molar mass of the compound was found to be 70.13 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon.
1) When 6.580 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 20.16 grams of CO2 and 9.631 grams of H2O were produced.
In a separate experiment, the molar mass of the compound was found to be 86.18 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon.
2)When 2.823 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 8.859 grams of CO2 and 3.627 grams of H2O were produced.
In a separate experiment, the molar mass of the compound was found to be 70.13 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon.
Lelia LubowitzLv2
29 Sep 2019
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