Question

1. When 4.912 grams of a hydrocarbon, C_xH_y, 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.

Enter the elements in the order presented in the question.



empirical formula =





molecular formula =

2. When 6.848 grams of a hydrocarbon, C_xH_y, 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.

Enter the elements in the order presented in the question.



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.

Enter the elements in the order Cu, Cl



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.

Enter the elements in the order Fe, F



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

.