When 3.061 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 9.603grams of...
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?
Homework Answers
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When 3.061 grams of a hydrocarbon,
CxHy, were burned in a combustion analysis
apparatus, 9.603grams of...
1) When 2.321 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 7.649...
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...
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...
1. When 2.689 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 8.437...
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...
When 1.696 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 5.198 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...
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 3.699 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 11.33 grams...
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 =?
1. When 1.389 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 4.771...
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.
When 3.741 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 12.65 grams...
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...
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 =
When 2.258 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 7.350 grams of CO2 and 2.257 gr...
When 2.258 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 7.350 grams of CO2 and 2.257 grams of H2O were produced. In a separate experiment, the molar mass of the compound was found to be 54.09 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon.
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