Explanation:

- The empirical formula of a compound gives the simplest ratio of atoms in the compound. It does not necessarily represent the actual number of atoms in a molecule of the compound.
- The empirical formula CH2O2 indicates that the compound contains one carbon atom (C), two hydrogen atoms (H), and two oxygen atoms (O).
- To determine the molecular formula, we need to find the actual number of atoms in a molecule of the compound.

Calculating the molecular formula:

- The empirical formula CH2O2 has a total of 5 atoms (1 carbon + 2 hydrogen + 2 oxygen).
- To determine the molecular formula, we need to find the ratio of atoms in the empirical formula to the ratio of atoms in the molecular formula.
- For example, if the molecular formula has twice the number of atoms as the empirical formula, the molecular formula would be C2H4O4.

Comparison:

a) C2H2O2: This molecular formula has 5 atoms, which matches the number of atoms in the empirical formula. However, the ratio of atoms is not the same, so it cannot be the correct molecular formula.
b) C2H2O4: This molecular formula has 9 atoms, which is not the same as the number of atoms in the empirical formula. Therefore, it cannot be the correct molecular formula.
c) C2H4O4: This molecular formula has 10 atoms, which is the same as the number of atoms in the empirical formula. Additionally, the ratio of atoms matches the empirical formula, so this could be the correct molecular formula.
d) CH4O4: This molecular formula has 9 atoms, which is not the same as the number of atoms in the empirical formula. Therefore, it cannot be the correct molecular formula.

Conclusion:

The correct molecular formula for the compound with the empirical formula CH2O2 could be C2H4O4.