How can I calculate the empirical formula of butane?

1 Answer
Jul 29, 2014

It depends on the information you have.

The empirical formula tells us the simplest whole-number ratio of the different types of atoms in a compound.

FROM THE MOLECULAR FORMULA

If you know that the molecular formula of butane is C₄H₁₀, then you divide the subscripts by their highest common factor (2).

This gives you the empirical formula C₂H₅.

FROM PERCENTAGE COMPOSITION

You can calculate the empirical formula from percentage composition.

Example

Butane is 82.66 % C and 17.34 % by mass. What is its empirical formula?

Solution

Assume 100 g of butane. Then you have 82.66 g of C and 17.34 g of H.

Moles of C = 82.66 g C × 1mol C12.01g C = 6.8826 mol C

Moles of H = 17.34 g H × 1mol H1.008g H = 17.202 mol H

Moles of CMoles of H=6.8826mol17.202mol=12.4994=24.998825

∴ The empirical formula of butane is C₂H₅.

FROM COMBUSTION ANALYSIS

You can calculate the empirical formula by doing a combustion analysis.

You burn a sample of butane and measure the masses of CO₂ and H₂O produced.

Example

The combustion of a sample of butane produces 1.6114 g of carbon dioxide and 0.8427 g of water. What is the empirical formula of butane?

Solution

Moles of C = 1.6114 g CO₂ × 1mol CO44.01g CO×1mol C1mol CO = 0.036 614 mol C

Moles of H = 0.8247 g H₂O × 1mol HO18.02g HO×2mol H1mol HO = 0.091 532 mol H

Moles of CMoles of H=0.036614mol0.091532mol=12.5000=25.000025

∴ The empirical formula of butane is C₂H₅.

Very good explanation, large fond, video on this page: https://www.boundless.com/chemistry/textbooks/boundless-chemistry-textbook/atoms-molecules-and-ions-2/chemical-formulas-37/empirical-formulas-210-587/