1) The pressure of a mixture of chemically non-interacting ideal gases is equal to the sum of the partial pressures. Approximately applicable to real gases at values of temperature and pressure far from the critical ones.
2) At constant temperature the solubility in a given liquid of each of the components of a gas mixture standing above the liquid is proportional to its partial pressure. Each gas of the mixture dissolves as though the other components were absent, that is, in accordance with Henry's law. It holds strictly for a mixture of ideal gases; it is also applicable to real gases if their solubility is small and their behaviour is close to that of an ideal gas. Dalton's laws were discovered by the English scientist J. Dalton in 1801 and 1803.
2) At constant temperature the solubility in a given liquid of each of the components of a gas mixture standing above the liquid is proportional to its partial pressure. Each gas of the mixture dissolves as though the other components were absent, that is, in accordance with Henry's law. It holds strictly for a mixture of ideal gases; it is also applicable to real gases if their solubility is small and their behaviour is close to that of an ideal gas. Dalton's laws were discovered by the English scientist J. Dalton in 1801 and 1803.