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gases behave most ideally when they are as inert and non-interacting as possible. this is why @high temperatures and low pressure they behave most ideally; the potential energy of intermolecular forces is lessened. high temp = greater kinetic energy/moving around faster, and low pressure = less collisions and opportunities to experience vdw forces. by this logic, He is the most ideal gas.
To add on, generally the rule is that a gas behaves more like an ideal gas at higher temperature and lower pressure. This is because under these conditions, the gas molecules will have little to no intermolecular forces with each other. So it is possible to achieve ideal gas behavior under extreme conditions: incredibly high temperatures and low pressures.
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