Under what condition is the ideal-gas suitable for real gases?

Question

Under what condition is the ideal-gas suitable for real gases?

Answer 1

Atmospheric gases like oxygen and nitrogen under conditions not too far removed from ambient behave very much like ideal gases.

Real Gases deviate from Ideal Gas Behaviour because

   1. at low temperatures the gas molecules have less kinetic energy (move around less) so they do attract each other

   2. at high pressures the gas molecules are forced closer together so that the volume of the gas molecules becomes significant compared to the volume the gas occupies  

Answer 2

theoretically, never.

In the ideal gas model the size of the gas molecules are not taken into account, nor is the gravitational force they exert on each other.

These things become increasingly irrelevant when the actual gas is composed of small molecules or (more so) is at a low pressure. When you lower the temperature or pressure of an actual gas it behaves more like an ideal gas.

So the answer to your question would be 'conditions of low pressure and/or temperature'

Answer 3

Gotta be high temp and low pressure.  Particles have to act like they don't see each other and that they have so much energy they can neglect any attractions for each other.

Answer 4

A real gas can behave as an ideal gas at high temperature and at low pressure At this condition the intermolecular attrations are negligible

Question must be under what condition the real gas can be an ideal gas?