Partial pressure
Partial pressure
Partial pressure (pronunciation: pahr-shuhl presh-er) is a term used in gas laws and physiology to describe the pressure that a gas would have if it alone occupied the volume of a mixture of gases.
Etymology
The term "partial pressure" is derived from the concept that in a mixture of gases, each gas exerts a "part" of the total pressure. This concept was first proposed by John Dalton in the early 19th century and is known as Dalton's law.
Definition
In a mixture of gases, each gas component contributes to the total pressure of the system. This contribution is the partial pressure of that gas, and it is equal to the pressure that the gas would exert if it alone occupied the entire volume. The total pressure of the gas mixture is the sum of the partial pressures of all the gases in the mixture.
Calculation
The partial pressure of a gas can be calculated using the formula:
Pi = Xi * Pt
where Pi is the partial pressure of the gas, Xi is the mole fraction of the gas in the mixture, and Pt is the total pressure of the mixture.
Applications
Partial pressure is a fundamental concept in thermodynamics and gas laws, and it has important applications in medicine and environmental science. In medicine, for example, the partial pressures of oxygen and carbon dioxide in the blood are important indicators of respiratory function.
Related terms
External links
- Medical encyclopedia article on Partial pressure
- Wikipedia's article - Partial pressure
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