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(B) An ideal gas is defined as a system in which there are no intermolecular or interatomic forces. Any real system approaches ideal gas behaviour in

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At low temperature and high pressure

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(B) An ideal gas is defined as a system in which there are no intermolecular or interatomic forces. Any real system approaches ideal gas behaviour in the limit where the pressure is extremely low and the temperature is high enough to overcome attractive intermolecular forces. $PV = nRT$ Here,$n$ is the number of moles of gas. The ideal gas equation describes the state of an ideal gas. At low temperature and high pressure,gases deviate more from ideal behaviour because as pressure increases,the force of attraction between molecules increases and the molecules come closer together,making the volume of the gas particles significant compared to the total volume.

When is deviation more in the behaviour of a gas from the ideal gas equation $PV = nRT$?

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