Ideal gas law
Ideal Gas Law is a fundamental principle in the field of Chemistry and Physics. It describes how gases behave under varying conditions of pressure, volume, and temperature. The law is usually stated as PV = nRT, where P is the pressure of the gas, V is the volume of the gas, n is the number of moles of the gas, R is the ideal gas constant, and T is the temperature of the gas (measured in Kelvin).
History[edit | edit source]
The Ideal Gas Law was first stated by Emil Clapeyron in 1834 as a combination of Boyle's Law, Charles's Law and Avogadro's Law. The law has since been expanded and refined, and is now a cornerstone of the Kinetic Theory of Gases.
Derivation[edit | edit source]
The Ideal Gas Law can be derived from the Kinetic Theory of Gases, assuming that gases are composed of a large number of tiny particles (atoms or molecules) that are in constant, random motion.
Applications[edit | edit source]
The Ideal Gas Law has many practical applications in fields such as Engineering, Meteorology, and Medicine. For example, it is used to calculate the density and distribution of air in the atmosphere, which is crucial for weather forecasting and climate modeling.
Limitations[edit | edit source]
While the Ideal Gas Law is a good approximation for many gases under many conditions, it becomes less accurate at very high pressures and low temperatures, where real gases deviate from ideal behavior due to intermolecular interactions and the finite size of gas particles.
See Also[edit | edit source]
References[edit | edit source]
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Contributors: Prab R. Tumpati, MD
