There are specific steps to calculate the empirical formula of a compound when given a molecular formula, and vice versa. Let’s look at each process.
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To find an empirical formula from a molecular formula, divide the subscript of each element by the greatest common factor.
Let’s look at an example:
Calculate the empirical formula of the substance C6H12O6.
| Steps | Example |
|---|---|
| 1. Identify the subscripts of the substance. | C = 6 H = 12 O = 6 |
| 2. Check if the subscripts can be divided by the same numerical factor. In this case, all subscripts can be divided by 6. However, If possible, repeat the process to divide all the subscripts in the formula by the same factor. Stop when it’s no longer possible to divide subscripts. | C = 6 ÷ 6 H = 12 ÷ 6 O = 6 ÷ 6 |
| 3. Write the simplified formula. | C = 1 H = 2 O = 1 The empirical formula is CH2O |
Converting from a molecular formula to an empirical formula is relatively simple. But what about the reverse process? Well, converting from an empirical formula back to a molecular formula requires a bit more information but is still quite straightforward. You will need:
Let’s look at an example:
Determine the molecular formula of a compound that has a molar mass (Mr) of 92 and an empirical formula of NO2.
| Steps | Example |
|---|---|
| 1. Identify the relative formula mass of the compound given. | Mr of NO2 = 92 |
| 2. Identify the relative atomic mass (Ar) of each element in the compound. | Ar N = 14 Ar O = 16 |
| 3. Calculate the Mr of the compound according to its empirical formula. Remember to multiply the atomic mass by the subscript, which indicates how many times that atom is present in the compound. | Mr NO2 = 14 + (2 × 16) = 46 |
| 4. Compare the true relative formula mass (Mr) of the molecule to the Mr of its empirical formula. By dividing the true Mr by the empirical Mr, you can determine how many times the empirical formula ‘fits’ into the molecular formula. This ratio is the factor you multiply each element by to find the molecular formula. | Relative formula mass ÷ Mr NO2 = 92 ÷ 46 = 2 |
| 5. Apply the factor to the empirical formula to find the molecular formula. | Applying the factor of 2 to the empirical formula NO2 gives us N2O4 as the molecular formula. |
Last updated: December 27, 2022
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Last updated: April 27th, 2024
Please read these terms and conditions carefully before using our services.
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