Volume percents characterize the composition of gas mixtures. An example of a gas mixture is air that consists of primarily oxygen and nitrogen gasses. Gas mixtures obey the ideal gas law that sets the relation between the gas volume, temperature and pressure. According to this law, the volume is proportional to the number of moles of a gas, and therefore, the mole percentage is the same as the volume percents for gas mixtures. Weight percents refer to mass of gasses in the mixtures and are required for stoichiometry calculations in chemistry.

## Write Down The Chemical Composition

## Calculate the Molar Mass

## Calculate the Second Molar Mass

## Divide to Get Weight

## Find the Weight of the Second Gas

## Add Up the Weights

## Calculate the First Weight Percent

## Calculate the Second Weight Percent

Write down the composition of the gas mixture. For example, the mixture consists of oxygen O_{2} and nitrogen N_{2}, and their respective volume percents are 70 and 30.

Calculate the molar mass of the first gas in the mixture; in this example, the molar mass of oxygen, O_{2} is 2 x 16 = 32 grams per mole. Note that the atomic weight of oxygen is 16, and the number of the atoms in the molecule is 2.

Calculate the molar mass of the second gas in the mixture; in this example, the molar mass of nitrogen, N_{2} is 2 x 14 = 28 grams per mole. Note that the atomic weight of nitrogen is 14, and the number of the atoms in the molecule is 2.

Divide the volume percent of the first gas by 100, and then multiply the respective molar mass to calculate the weight of the first gass in one mole of the mixture. In this example, the mass of the oxygen is (70/100) x 32 = 22.4 grams.

Divide the volume percent of the second gas by 100, and then multiply the respective molar mass to calculate the weight of the second gass in one mole of the mixture. In this example, the mass of the oxygen is (30/100) x 28 = 8.4 grams.

Add up the weights of the gasses to compute the mass of one mole of the mixture. In this example, the mass of the mixture is 22.4 + 8.4 = 30.8 grams.

Divide the weight of the first gas by the mass of the mixture, and then multiply by 100 to calculate the weight percent. In this example, the weight percent of oxygen is (22.4 / 30.8) x 100 = 72.7.

Divide the weight of the second gas by the mass of the mixture, and then multiply by 100 to calculate the weight percent. In this example, the weight percent of nitrogen is (8.4 / 30.8) x 100 = 27.3.

#### References

- "Chemistry"; Raymond Chang; 2007
- Wolfram: Ideal Gas Law