- States that the total pressure exerted by the mixture of non-reactive gases is equal to the sum of the partial pressures of individual gases. This empirical law was observed by John Dalton in 1801 and is related to the ideal gas laws.
- Real World Example - 1. Air is a mixture of nitrogen, oxygen, CO2, H2O, etc. Each of these gases has its own partial pressure and total up to the atmospheric pressure at that location.