## Ideal Gas law

### Definition :

An ideal gas is a theoretical gas composed of many randomly moving point particles that interact only through elastic collisions and do not exert any intermolecular forces on each other.

In simpler terms, an ideal gas:

• Follows the ideal gas law:

PV = nRT PV = nRT

P: pression (atm, Pa, 1 atm = 1,013 105 Pa, mmHg)

V: volume (L, m³, 1L = 10³ m³)

n: number of moles (mol)

R: ideal gas constant (R=0.0082 L am/mol K = 8.31 J/mol K = 2 cal/mol K)

T: température (°C, K, T (K) = T (°C) +273)

Boyle's Law (Pressure-Volume Relationship)

P 1 V 1 = P 2 V 2 P_1 V_1=P_2 V_2

At constant temperature, the pressure of a gas is inversely proportional to its volume.

Charles' Law (Volume-Temperature Relationship)

V 1 / T 1 = V 2 / T 2 V_1/T_1 =V_2/T_2

At constant pressure, the volume of a gas is directly proportional to its absolute temperature.

Gay-Lussac's Law (Pressure-Temperature Relationship)

P 1 / T 1 = P 2 / T 2 P_1/T_1 =P_2/T_2

At constant volume, the pressure of a gas is directly proportional to its absolute temperature.

Avogadro's Law (Volume-Amount Relationship)

V 1 / n 1 = V 2 / n 2 V_1/n_1 =V_2/n_2

At constant temperature and pressure, the volume of a gas is directly proportional to the number of moles.