Which gas law states that the total pressure of a mixture of gases is equal to the sum of the partial pressures of each gas in the mixture?

The principle that the total pressure of a mixture of gases is equal to the sum of the partial pressures of each individual gas is known as Dalton's Law. This law is significant in understanding how gases behave in mixtures and is especially relevant in fields such as aviation and medicine, where understanding the behavior of gases at various altitudes and conditions is crucial.

Dalton's Law indicates that if you have a container filled with various gases, each gas exerts pressure independently of the others. The total pressure can be calculated by adding together the pressures that each gas would exert if it occupied the same volume by itself. This understanding is essential in aerospace physiology, where the composition of the atmosphere and the partial pressures of gases like oxygen and nitrogen can significantly affect human physiology in flight.

The other laws mentioned relate to different aspects of gas behavior. Boyle's Law deals with the relationship between pressure and volume at a constant temperature, and Henry's Law describes how gases dissolve in liquids under varying pressure. The Law of Gaseous Diffusion describes how gas molecules move from areas of higher concentration to areas of lower concentration. However, none of these directly pertain to the summation of partial pressures in a gas mixture, making Dalton's Law the correct response.