Dalton's law of partial pressures

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Definition
  1. Noun:
    • Dalton's law of partial pressures: A fundamental law in physical chemistry and physics stating 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. Furthermore, the partial pressure of each gas is the pressure that gas would exert if it occupied the entire volume of the mixture alone at the same temperature.
Usage
  • This term is used in scientific contexts, particularly in chemistry, physics, and engineering, to describe and calculate the behavior of gas mixtures.
  • It is a proper noun, often capitalized as "Dalton's Law of Partial Pressures" or simply "Dalton's Law."
Examples
  • Noun:
    • To find the total pressure in the container, we applied Dalton's law of partial pressures.
    • Dalton's law of partial pressures is essential for understanding gas exchange in respiratory physiology.
    • The experiment confirmed Dalton's law of partial pressures for the mixture of nitrogen and oxygen.
Advanced Usage
  • "Dalton's Law" as a shorthand: The full name is often shortened in technical discourse.
    • We can use Dalton's Law to calculate the contribution of water vapor to the total atmospheric pressure.
Variants and Related Words
  • Partial Pressure (n): The pressure that a single gas in a mixture would exert if it occupied the entire volume alone.
    • The partial pressure of carbon dioxide in the blood is a critical medical measurement.
  • Dalton's Law (n): A common abbreviated form of "Dalton's law of partial pressures."
Synonyms
  • Law of Partial Pressures: A synonymous phrase that omits Dalton's name.
  • Dalton's Law: The most common abbreviated synonym.
Related Phrases
  • Ideal Gas Law: A related fundamental gas law often used in conjunction with Dalton's law for calculations.
  • Mole Fraction: A key concept used to calculate partial pressures (Partial Pressure = Mole Fraction × Total Pressure).
Noun
  1. (chemistry and physics) law stating that the pressure exerted by a mixture of gases equals the sum of the partial pressures of the gases in the mixture; the pressure of a gas in a mixture equals the pressure it would exert if it occupied the same volume alone at the same temperature

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