A compound is found to contain 24.0 g carbon, 4.00 mol hydrogen and 1.204 × 1024 atoms of oxygen. What is the empirical formula of this compound?

To find the empirical formula of the compound, we need to convert the given amounts of carbon, hydrogen, and oxygen into moles.

1. For carbon, we know that the molar mass of carbon (C) is approximately 12.01 g/mol. So, we can convert the given mass of carbon into moles by dividing the mass by the molar mass:

   Moles of C = 24.0 g / 12.01 g/mol = 2.00 mol

2. For hydrogen, we are already given the amount in moles, which is 4.00 mol.

3. For oxygen, we are given the amount in atoms. We can convert this into moles using Avogadro's number (6.022 x 10^23 atoms/mol):

   Moles of O = 1.204 x 10^24 atoms / 6.022 x 10^23 atoms/mol = 2.00 mol

Now that we have the amounts of C, H, and O in moles, we can write the empirical formula by simply combining these amounts as subscripts in the formula:

The empirical formula is C2H4O2.