Under which conditions of temperature and pressure does a real gas behave most like an ideal gas

Under normal conditions of pressure and temperature, real gases tend to behave qualitatively in the same way as an ideal gas.

The ideal gas is considered to be part of the group of theoretical gases because it is made up of point particles that move randomly and do not interact with each other.

Therefore, we can conclude that the ideal gas is the behavior of those gases whose molecules do not interact with each other and move randomly.

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Generally, a gas behaves more like an ideal gas at higher temperature and lower pressure, as the potential energy due to intermolecular forces becomes less significant compared with the particles' kinetic energy, and the size of the molecules becomes less significant compared to the empty space between them.

Explanation:

sodium (na), for example, has one electron in its valence shell. this is an unstable state because that valence shell needs eight electrons to be full. in order to fill its valence shell, find a way to add seven electrons to its valence shell

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explanation:

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