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When 3.848 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 13.21 grams of CO₂ and 2.164 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. Enter the elements in the order presented in the question. empirical formula = molecular formula =

When 3.848 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 13.21 grams of CO₂ and 2.164 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. Enter the elements in the order presented in the question. empirical formula = molecular formula =

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Sample Furnace Enter the elements in the order presented in the question. empirical formula = When 3.848 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 13.21 grams of CO₂ and 2.164 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. molecular formula = H₂O absorber CO₂ absorber
Transcribed Image Text:Sample Furnace Enter the elements in the order presented in the question. empirical formula = When 3.848 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 13.21 grams of CO₂ and 2.164 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. molecular formula = H₂O absorber CO₂ absorber
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