The gas in chemistry, is a state of matter fluid that fills the busy container and let you easily compress.
The gas under the same conditions of temperature and pressure have very similar characteristics between them.
The macroscopic properties of gases are interpreted through the molecular study and the so-called kinetic theory of gases.
We define the ideal gas condition as the condition to which all gases tend to resemble by decreasing the temperature and pressure. The properties of an ideal gas are:
Therefore, the ideal gas fills the entire volume of its container, while the real gas does not occupy it all because the volume of the particles themselves occupies a part. The ideal gas is, therefore, infinitely compressible (V = 0).
• In the ideal gas, the particles do not interact with each other.
• The particles of the ideal gas move with uniform rectilinear motion, colliding with each other and striking the container walls: this is explained by remembering that there is no interaction between the particles. The bumps are elastic, so no energy is lost.
• The average kinetic energy of the particles is directly proportional to the gas temperature.
