ideal gas law

The ideal gas law is the equation of state of a hypothetical ideal gas, first stated by Benoît Paul Émile Clapeyron in 1834. The state of an amount of gas is determined by its pressure, volume, and temperature according to the equation: where is the absolute pressure [Pa], is the volume [m3] of the vessel containing  moles of gas, is the amount of substance of gas [mol], is the gas constant [8.314 472 m3·Pa·K−1·mol−1], is the temperature in kelvins [K].
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The gas laws are a set of laws that describe the relationship between thermodynamic temperature (T), pressure (P) and volume (V) of gases. They are a loose collection of rules developed between the late Renaissance and early 19th century.
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A gas whose pressure P, volume V, and temperature T are related by PV = nRT, where n is the number of moles of gas and R is the ideal gas law constant . Ideal gases have molecules with negligible size, and the average molar kinetic energy of an ideal gas depends only on its temperature. Most gases behave ideally at sufficiently low pressures.

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