Empirical Formula Calculation:

To calculate the empirical formula, we need to determine the relative number of atoms of each element in the compound. We can assume that we have 100 g of the compound, which means we have:

- Hydrogen: 4.07 g (4.07% of 100 g)
- Carbon: 24.27 g (24.27% of 100 g)
- Chlorine: 71.65 g (71.65% of 100 g)

Next, we need to determine the moles of each element by dividing the mass by its molar mass:

- Hydrogen: 4.07 g / 1.008 g/mol = 4.04 mol
- Carbon: 24.27 g / 12.011 g/mol = 2.02 mol
- Chlorine: 71.65 g / 35.453 g/mol = 2.02 mol

We can divide each mole value by the smallest mole value to get the simplest whole-number ratio of the elements:

- Hydrogen: 4.04 mol / 2.02 mol = 2
- Carbon: 2.02 mol / 2.02 mol = 1
- Chlorine: 2.02 mol / 2.02 mol = 1

Therefore, the empirical formula of the compound is C₁H₂Cl.

Molecular Formula Calculation:

To determine the molecular formula, we need to know the molecular mass of the empirical formula. The empirical formula mass is:

- C₁H₂Cl: 1 x 12.011 g/mol + 2 x 1.008 g/mol + 1 x 35.453 g/mol = 49.48 g/mol

We can then divide the molar mass of the compound by the empirical formula mass to determine the molecular formula multiplier:

- 98.96 g/mol / 49.48 g/mol = 2

We can multiply the subscripts in the empirical formula by 2 to get the molecular formula:

- C₂H₄Cl₂

Therefore, the molecular formula of the compound is C₂H₄Cl₂.