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?

Sure, let's solve this step by step:

1. First, we need to convert all the given amounts into moles, because the empirical formula is based on the ratio of moles of each element in the compound.

   • For carbon (C), we have 24.0 g. The molar mass of carbon is approximately 12.01 g/mol. So, the number of moles of carbon is 24.0 g / 12.01 g/mol = 2.00 mol.

   • For hydrogen (H), we are already given that there are 4.00 mol.

   • For oxygen (O), we are given the number of atoms, not grams. We can convert this to moles using Avogadro's number (6.022 x 10^23 atoms/mol). So, the number of moles of oxygen is 1.204 x 10^24 atoms / 6.022 x 10^23 atoms/mol = 2.00 mol.

2. Now that we have the number of moles of each element, we can write the ratio of moles as the empirical formula. However, in this case, the ratio of moles of C:H:O is 2:4:2, which can be simplified to 1:2:1.

3. Therefore, the empirical formula of the compound is CH2O.