Why real gases do not follow gas laws perfectly under all conditions?

Real gases do not follow the ideal gas equation perfectly under all conditions . They show deviation from the ideal behavior when. It is apparent that at very high pressure, the measured volume for real gases is more than the calculated volume (from Boyle’s law) for ideal gases.

Why do real gases not always behave ideally under what conditions does a real gas behave most ideally Why?

A real gas is a gas that does not behave according to the assumptions of the kinetic-molecular theory. Real gases deviate from ideal gases at high pressures and at low temperatures. Gases are most ideal at high temperature and low pressure.

In what conditions does a real gas obey ideal gas equation?

A real gas obeys ideal gas equation when temperature is vey high and pressure is very low. [ Note : Under these conditions, the density of a gas is very low. Hence, the molecules, on an average, are far away from each other.

Why does real gas show deviation from ideal?

Real gases show deviations from ideal gas law because molecules interact with each other. At high pressures molecules of gases are very close to each other. At very low temperatures intermolecular forces become significant.

Why do real gases deviate from the ideal gas law at high pressure?

At high pressure, molecules tend to be more crowded together; if they are closer together, the intermolecular forces are stronger, and cause more deviations from ideal gas behavior, which assumes those forces don’t exist.

Why do real gases deviate from ideal Behaviour?

Gases deviate from the ideal gas behaviour because their molecules have forces of attraction between them. At high pressure the molecules of gases are very close to each other so the molecular interactions start operating and these molecules do not strike the walls of the container with full impact.

What are the conditions for an ideal gas?

For a gas to be “ideal” there are four governing assumptions: The gas particles have negligible volume. The gas particles are equally sized and do not have intermolecular forces (attraction or repulsion) with other gas particles. The gas particles move randomly in agreement with Newton’s Laws of Motion.

Why do gases deviate from ideal behaviour give two reasons?

Real gases deviate from ideal behavior because 1) they have intermolecular forces between molecules, 2) collisions aren’t always elastic (also due to intermolecular forces), and 3) gas molecules have volume.