The empirical formula CH tells us the simplest whole-number ratio of carbon and hydrogen atoms in the compound. However, it doesn't tell us the actual number of atoms in the molecule.

To determine the molecular formula, we need additional information, specifically the molar mass of the compound.

Here's how we can find the molecular formula:

1. Calculate the empirical formula mass:

- C: 12.01 g/mol

- H: 1.01 g/mol

- Empirical formula mass = 12.01 + 1.01 = 13.02 g/mol

2. Divide the molar mass of the compound by the empirical formula mass:

- This will give you a whole number, which is the factor by which the empirical formula needs to be multiplied to get the molecular formula.

Example:

Let's say the molar mass of the compound is 78.12 g/mol.

- 78.12 g/mol / 13.02 g/mol = 6

This means the molecular formula is six times the empirical formula:

- Molecular formula: C6H6

Without knowing the molar mass, we can't determine the molecular formula. There are many possible molecular formulas with the empirical formula CH, such as:

* C2H2 (acetylene)

* C4H4

* C6H6 (benzene)

* C8H8

* and so on.