Question

Why pressure of real gas is less than ideal gas?

Answer 1

Pressure:

1. Pressure is defined as the physical force applied to an object.
2. The force applied per unit area is perpendicular to the objects' surfaces.
3. The basic pressure formula is F/A. (Force per unit area)

Reason for pressure affect boiling point:

1. Ideal gases obey the gaseous laws at all temperatures and pressures and have no volume, whereas real gases do not obey the gaseous laws at all pressures and temperatures and have some volume.
2. Real gases behave differently at low temperatures and high pressures, although it was often supposed that they followed the ideal gas laws as well. We have various assumptions in the kinetic theory of gases, one of which is that particles do not have attraction force between them, although this is not true for real gases. Van der Waals attraction exists among the particles of actual gas.
3. The particles of real gas attract one other, creating a backward force that prevents them from colliding with the container's wall with the same efficiency as they could if there was no attraction between them. As a result, the actual pressure imposed by real gas is lower than the ideal gas pressure applied to the container's walls.
4. As a result, we can deduce that the pressure of the real gas is lower than the pressure of the ideal gas due to intermolecular forces.