Dalton's Law of Partial Pressures helps explain the causes of which of the following?

Dalton's Law of Partial Pressures is fundamental to understanding how gases behave in a mixture and the effects of pressure in underwater environments. This law states that in a mixture of non-reacting gases, the total pressure exerted by the mixture is equal to the sum of the partial pressures of each individual gas in the mixture.

Oxygen toxicity occurs when breathing oxygen at elevated partial pressures. As a diver descends, the pressure increases which also increases the partial pressure of the gases inhaled, including oxygen. When the partial pressure of oxygen exceeds safe physiological limits (around 1.4 to 2.0 ATA in environments like diving), it can lead to toxic effects on the pulmonary system and the central nervous system. This is a direct result of the principles outlined by Dalton's Law, as it highlights the importance of understanding how the partial pressures of gases can affect physiological responses in divers.

Understanding this relationship is crucial for divers in order to avoid conditions like oxygen toxicity, particularly when utilizing gas mixtures that include a higher proportion of oxygen, such as in deep diving or technical diving scenarios. Thus, Dalton's Law provides a foundation for understanding not just the behavior of gases under pressure but also the potential risks associated with high partial pressures of oxygen.