# Characteristics of an Ideal Gas

Characteristics of an ideal gas:

The gases which follow fundamental postulates of kinetic theory of gases and at all temperatures and pressures simultaneously obey both Boyle’s law and Charles’s law are called ideal gases.

• Gases consist of particles in constant, random motion. They continue in a straight line until they collide with something—usually each other or the walls of their container.
• An ideal gas obeys the equation PV = nRT at all temperatures and pressures.
• Internal energy of an ideal gas at constant temperature is not dependent on its That means, (du/dV)T = 0, here, u = internal energy of the gas, V = volume of the gas, T = temperature.
• There is no attraction or repulsion between the molecules of an ideal gas.
• Total value of the gas molecules of an ideal gas is negligibly small compared with the value occupied by the gas molecules.
• The kinetic energy of a gas is a measure of its Kelvin temperature. Individual gas molecules have different speeds, but the temperature and kinetic energy of the gas refer to the average of these speeds.

The properties of an ideal gas are:

• An ideal gas consists of a large number of identical molecules.
• The volume occupied by the molecules themselves is negligible compared to the volume occupied by the gas.
• The molecules obey Newton’s laws of motion, and they move in random motion.
• The molecules experience forces only during collisions; any collisions are completely elastic, and take a negligible amount of time.
• All gases at a given temperature have the same average kinetic energy.
• Lighter gas molecules move faster than heavier molecules.