The steps to calculate the empirical formula are:
Let's say we have a compound with 40.92 g of carbon, 4.58 g of hydrogen, and 54.50 g of oxygen. Using the atomic masses (C: 12.01, H: 1.008, O: 16.00):
\[ \text{Moles of C} = \frac{40.92}{12.01} \approx 3.41 \]
\[ \text{Moles of H} = \frac{4.58}{1.008} \approx 4.54 \]
\[ \text{Moles of O} = \frac{54.50}{16.00} \approx 3.41 \]
Divide by the smallest number of moles (3.41):
\[ \text{Ratio of C} = \frac{3.41}{3.41} = 1 \]
\[ \text{Ratio of H} = \frac{4.54}{3.41} \approx 1.33 \approx 4 \]
\[ \text{Ratio of O} = \frac{3.41}{3.41} = 1 \]
So, the empirical formula is \( \text{C}_1\text{H}_4\text{O}_1 \) or simply \( \text{CH}_4\text{O} \).
The empirical formula of a compound is the simplest whole-number ratio of atoms of each element in the compound. It provides the relative number of atoms of each element in the compound.