When 3.699 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 11.33 grams of CO2 and 5.414 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. Enter the elements in the order presented in the question. empirical formula =? molecular formula =?
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When 3.699 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 11.33 grams...
When 1.696 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 5.198 grams of CO2 and 2.483 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. Enter the elements in the order presented in the question. empirical formula = molecular formula =
When 1.860 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 5.699 grams of CO2 and 2.723 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. Enter the elements in the order presented in the question. empirical formula = molecular formula =
When 3.741 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 12.65 grams of CO2 and 2.589 grams of H2O were produced. In a separate experiment, the molar mass of the compound was found to be 78.11g/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 3.949 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 12.39 grams of CO2 and 5.073 grams of H2O were produced. In a separate experiment, the molar mass of the compound was found to be 56.11g/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 =
1) When 2.321 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 7.649 grams of CO2 and 2.088 grams of H2O were produced. In a separate experiment, the molar mass of the compound was found to be 40.06 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon. Empirical formula= molecular formula= 2) When 2.201 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 7.442 grams of CO2 and 1.524 grams of...
A. When 1.591 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 5.378 grams of CO2 and 1.101 grams of H2O were produced. In a separate experiment, the molar mass of the compound was found to be 26.04 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon. B. A 9.448 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis and 18.88 grams of CO2 and 7.729 grams...
When 4.671 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 13.67 grams of CO2 and 8.398 grams of H2O were produced. In a separate experiment, the molecular weight of the compound was found to be 30.07 amu. 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 3.061 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 9.603grams of CO2 and 3.932grams of H2O were produced. In a separate experiment, the molar mass of the compound was found to be 42.08 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon. What is the empirical formula? What is the molecular formula?
1. When 2.689 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 8.437 grams of CO2 and 3.454 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. A 21.79 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis and 21.31 grams of CO2 and 4.362 grams...
1. When 1.389 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 4.771 grams of CO2 and 0.7813 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.