## Avogadro’s law definition and explanation

Avogadro’s law definition and explanation are 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 which is explained below briefly:

#### The law of “ideal gases” reads as follows:

The amount of gas matter (or “number of moles”) is

- proportional to the volume of gas.
- The amount of gas matter ( or the number of moles) is
- proportional to the gas pressure.
- The amount of gas matter (or a number of moles) is
- inversely proportional to the temperature.
- But it is independent of the nature of the gas.

#### We thus obtain:

n = PV / RT

### SI units of Avogadro’s law:

The SI units of it are as follows:

n (mol), P (Pa), V (m3), T (K)

#### Where R is?

R is the constant of ideal gases independent of the nature of the gas

R = 8.31J.K ^{-1} · mol ^{-1}

### Gas is considered perfect:

Gas is considered “perfect” if it strictly follows the previous law. Gas is never “perfect” but it is all the closer to this model the further it is from the liquefaction conditions for Avogadro’s law.

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 usual conditions:

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 is at approximately 20 ° C.

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