Low pressure and high temperature
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How are real gases different from ideal gases?
Real gases behave much like an ideal gas at low pressure and high temperature. An ideal gas is defined as a gas that obeys gas laws at all condition of pressure and temperature. Ideal gases have velocity and mass. They do not have volume. When compared to the total volume of the gas the volume occupied by the gas is negligible.
Why does a gas behave as an ideal gas at high pressure?
well in case of low pressure and high temperature – there will be large intermolecular distances so negligible intermolecular forces. So it well behave as an ideal gas. And if there is high pressure there will be repulsive forces and small distances which does not match with the postulates. In the real gas equation pressure is P + an2/V2.
What is a real gas?
A real gas is defined as a gas that does not obey gas laws at all standard pressure and temperature conditions. When the gas becomes massive and voluminous it deviates from its ideal behaviour. Real gases have velocity, volume and mass. When they are cooled to their boiling point, they liquefy.
What is an ideal gas?
An ideal gas is a theoretical gas that obeys the ideal gas law as the gas particles are not subject to interparticle interactions. The gas particles in an ideal gas are considered ideal particles as their interactions are perfectly elastic.