Avogadro’s law definition and explanation
Avogadro’s law definition and explanation is listed below :
Avogadro’s law states that equal volumes of different gases, under the same conditions of temperature and pressure, contain the same number of molecules.
Avogadro’s law is included in a more general law: the law of “ideal gases” which reads as follows:
The amount of gas matter (or “number of moles”) is
-proportional to the volume of gas.
-proportional to the gas pressure.
– inversely proportional to the temperature.
But it is independent of the nature of the gas.
We thus obtain:
n = PV / RT
SI units: n (mol), P (Pa), V (m3), T (K)
R is the constant of ideal gases independent of the nature of the gas
R = 8.31J.K -1 · mol -1
A gas is considered “perfect” if it strictly follows the previous law. A gas is never “perfect” but it is all the closer to this model the further it is from the liquefaction conditions.
One mole occupies approximately a volume of 22.4 liters at normal temperature and pressure conditions (CNTP), which corresponds to a pressure of 1 atmosphere or 1013 h Pa (hectopascal) and a temperature of 0 ° C.
Under the usual conditions of temperature and pressure (in the laboratory for example)), one mole of gas occupies approximately 24.0 liters, the pressure is at 1 bar and the temperature at approximately 20 ° C.
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