1. When 4.912 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 15.41 grams of CO2 and 6.311 grams of H2O were produced.
In a separate experiment, the molar mass of the compound was found to be 28.05 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon.
empirical formula = |
molecular formula = |
2. When 6.848 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 21.49 grams of CO2 and 8.799 grams of H2O were produced.
In a separate experiment, the molar mass of the compound was found to be 28.05 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon.
empirical formula = |
molecular formula = |
3. A 15.05 gram sample of copper is heated in the presence of excess chlorine. A metal chloride is formed with a mass of 23.45 g. Determine the empirical formula of the metal chloride.
empirical formula = |
4. A 27.81 gram sample of iron is heated in the presence of excess fluorine. A metal fluoride is formed with a mass of 46.73 g. Determine the empirical formula of the metal fluoride.
empirical formula = |
5. A compound is found to contain 50.05 % sulfur and 49.95 % oxygen by mass.
To answer the question, enter the elements in the order presented above.
QUESTION 1:
The empirical formula for this compound is | . |
QUESTION 2:
The molar mass for this compound is 64.07 g/mol.
The molecular formula for this compound is | . |
6. A compound is found to contain 3.622 % carbon and 96.38 % bromine by mass.
To answer the question, enter the elements in the order presented above.
QUESTION 1:
The empirical formula for this compound is | . |
QUESTION 2:
The molar mass for this compound is 331.6 g/mol.
The molecular formula for this compound is | . |
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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 3.699 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 3.741 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 =
A 13.56 gram sample of copper is heated in the presence of excess bromine. A metal bromide is formed with a mass of 30.60 g Determine the empirical formula of the metal bromide. ter the elements in the order C B empirical formula A 5.267 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis and 13.29 grams of CO2 and 2.332 grams of H20 are produced In a separate experiment, the molar mass...
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...
35a When 4.752 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 16.06 grams of CO2 and 3.289 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. 35 part b A 4.079 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis and 9.273 grams of CO2 and...
When 3.537 grams of a hydrocarbon, C,Hy, were burned in a combustion analysis apparatus, 11.96 grams of CO2 and 2.448 grams of H2O were produced In a separate experiment, the molar mass of the compound was found to be 78.11 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 =