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Dalton’s Law of Partial Pressures

1802
  • John Dalton
Gas mixing apparatus in a vintage laboratory for thermodynamics applications.

Dalton’s Law states that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of the individual gases. The partial pressure of a gas is the pressure it would exert if it occupied the entire volume alone at the same temperature. The formula is [latex]P_{text{total}} = \sum_{i=1}^{n} p_i[/latex].

John Dalton formulated this law around 1802, based on his experiments with gases. It was a crucial step in the development of his atomic theory, as it suggested that the particles of different gases in a mixture act independently of one another. The law holds true for ideal gases and is a good approximation for real gases at low pressures and high temperatures, where intermolecular interactions are minimal. The partial pressure of a single gas ([latex]p_i[/latex]) in a mixture can be calculated using its mole fraction ([latex]x_i[/latex]) and the total pressure ([latex]P_{text{total}}[/latex]): [latex]p_i = x_i cdot P_{text{total}}[/latex]. This relationship is extremely useful in many practical scenarios. For instance, in scuba diving, the partial pressure of oxygen is critical; if it becomes too high at depth, it can cause oxygen toxicity. Divers use Dalton’s law to calculate the maximum safe operating depth for a given breathing gas mixture. In physiology, the exchange of oxygen and carbon dioxide in the alveoli of the lungs is driven by differences in their partial pressures between the air and the blood. The law also explains why collecting a gas over water requires a correction, as the total measured pressure includes the partial pressure of water vapor at that temperature, which must be subtracted to find the pressure of the collected gas alone.

UNESCO Nomenclature: 2212
- Termodinámica

Tipo

Sistema abstracto

Disrupción

Sustancial

Utilización

Uso generalizado

Precursores

  • Antoine Lavoisier’s work on the composition of air
  • Robert Boyle’s experiments on the properties of gases
  • The development of the concept of a gas as a collection of particles

Aplicaciones

  • scuba diving for calculating safe gas mixtures (nitrox, trimix)
  • respiratory medicine to understand gas exchange in the lungs
  • chemistry for collecting gases over water in experiments
  • gas industrial mixing and storage
  • anesthesiology for administering gas mixtures

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Related to: Dalton’s law, partial pressure, gas mixture, John Dalton, total pressure, mole fraction, scuba diving, ideal gas, thermodynamics, chemistry.

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