The empirical formula

of a compound is the simplest whole number ratio of the elements in the compound. It does not necessarily represent the actual number of atoms of each element in the compound, but rather the ratio in which they are present. The empirical formula can be determined from the percent composition of a compound or from experimental data such as mass or volume measurements. It is important to note that the empirical formula may not always be the same as the molecular formula, which represents the actual number of atoms of each element in a compound.

The empirical formula of a compound represents the simplest whole-number ratio of the elements present in the compound. It can be determined from the elemental analysis of a compound, which gives the mass percentage of each element.

To determine the empirical formula, follow these steps:

1. Convert the mass percentage of each element to grams.
2. Convert the grams of each element to moles by dividing by its molar mass.
3. Divide the moles of each element by the smallest number of moles to obtain the simplest whole-number ratio.
4. Multiply the subscripts of the elements in the empirical formula by a whole number to balance the charges if the compound is ionic.

The empirical formula is then written as the chemical symbols of the elements with their corresponding subscripts.

For example, if the elemental analysis of a compound gives the following mass percentages:

- Carbon: 40.0%
- Hydrogen: 6.7%
- Oxygen: 53.3%

1. Convert the mass percentages to grams:
- Carbon: 40.0 g
- Hydrogen: 6.7 g
- Oxygen: 53.3 g

2. Convert the grams to moles:
- Carbon: 40.0 g / 12.01 g/mol = 3.33 mol
- Hydrogen: 6.7 g / 1.01 g/mol = 6.63 mol
- Oxygen: 53.3 g / 16.00 g/mol = 3.33 mol

3. Divide the moles of each element by the smallest number of moles:
- Carbon: 3.33 mol / 3.33 mol = 1
- Hydrogen: 6.63 mol / 3.33 mol = 2
- Oxygen: 3.33 mol / 3.33 mol = 1

Therefore, the empirical formula of the compound is CH2O.

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