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A gas becomes non-ideal under high pressure conditions. At high pressure conditions, the molecules of gas come very close to each other, such that...
A gas becomes non-ideal under high pressure conditions.
At high pressure conditions, the molecules of gas come very close to each other, such that there is a lack of space between them. Due to such proximity, the individual volume of the particles does not remain negligible as compared to the volume of the gas, but becomes appreciable. And, hence when the volume is contracted further, as the pressure increases, but this decrease of volume does not remain proportional to the increase in pressure, as stated by the Boyle's law
Another factor which comes in significance at higher pressure conditions is the force of attraction among the individual particles of gas. This factor is negligible at lower pressures and hence a gas behaves ideally. At such higher pressures, the force of attraction of the particles bring the particles closer, and hence lead to a further decrease in volume. The reduction in the Kinetic Energy of particles, due to a lack of space at higher pressure, also aids in bringing the particles of a gas closer.
When the temperature is reduced to near the condensation point of the gas does this have an impact?
