Partial pressure

Partial pressure is the pressure that would be exerted by one of the gases in a mixture if it occupied the same volume on its own. It is a very important concept in Chemistry and Physics, and is particularly relevant in the fields of Respiratory physiology and Anesthesia.

Definition

In a mixture of ideal gases, each gas has a partial pressure which is the pressure which the gas would have if it alone occupied the volume. The total pressure of an ideal gas mixture is the sum of the partial pressures of each individual gas in the mixture.

Dalton's Law

Dalton's law (also called Dalton's law of partial pressures) states that the total pressure exerted by the mixture of non-reactive gases is equal to the sum of the partial pressures of individual gases. This empirical law was observed by John Dalton in 1801 and is related to the ideal gas laws.

Applications

Partial pressure has a wide range of applications, particularly in the fields of Respiratory physiology and Anesthesia. In the human body, the partial pressure of oxygen and carbon dioxide in the blood is an important parameter that is measured in those who are critically ill or who have respiratory diseases. In anesthesia, the partial pressure of anesthetic agents is important in determining their uptake and distribution in the body.

See also

• Ideal gas law
• Henry's law
• Gas laws
• Respiratory physiology
• Anesthesia

References

Partial pressure Resources
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