Empirical Formula
- The molecular formula is the formula that
shows the number and type of each atom in a
molecule
- E.g. the molecular formula of ethanoic acid is C2H4O2
- The empirical formula is the simplest
whole number ratio of the atoms of each element present in one molecule or
formula unit of the compound
- E.g. the empirical formula of ethanoic acid is CH2O
- It can be deduced from data that give the percentage composition by mass of the elements in a compound
- Organic molecules often have different empirical and molecular formulae
- The formula of an ionic compound is always an empirical formula
Worked example
Determine the empirical formula of a compound that contains 10 g of hydrogen and 80 g of oxygen.
Answer:
| Hydrogen | Oxygen | |
| Note the mass of each element | 10 g | 80 g |
| Divide the masses by atomic masses |
10 = 10 mol |
80 = 5 mol |
| Divide by the lowest figure to obtain nearest whole number ratio |
10 =2 |
5.0
5.0 =1 |
| Empirical formula | H2O | |
Worked example
Determine the empirical formula of a compound that contains 85.7% carbon and 14.3% hydrogen.
Answer:
| Carbon | Hydrogen | |
| Note the X by mass of each element | 85.6 | 14.3 |
| Divide the X by atomic masses |
85.7 =7.14 mol |
14.3 = 14.2 mol |
| Divide by the lowest figure to obtain nearest whole number ratio |
7.14 = 1 |
14.2 = 2 |
| Empirical formula | CH2 | |
Molecular formula
- The molecular formula gives the actual numbers of each element present in the formula of the compound
- The molecular formula can be found by dividing the relative molecular mass by the relative mass of the empirical formula and finding the multiple that links the empirical formula to the molecular formula
- Multiply the empirical formula by this number to find the molecular formula
Worked example
The empirical formula of X is C4H10S and the relative molecular mass of X is 180.42.
What is the molecular formula of X?
Relative Atomic Mass Carbon: 12.01 Hydrogen: 1.01 Sulfur: 32.07
Answer:
- Step 1: Calculate the relative mass of empirical formula
Relative empirical mass = (C x 4) + (H x 10) + (S x 1)
Relative empirical mass = (12.01 x 4) + (1.01 x 10) + (32.07 x 1)
Relative formula mass = 90.21
- Step 2: Divide relative molecular mass of X by relative mass of empirical formula
The multiple between X and the empirical formula = 180.42/90.21 = 2
- Step 3: Multiply the empirical formula by 2
2 x C4H10S = C8H20S2
The molecular formula of X is C8H20S2