Consider these statements :
- At Boyle point, real gases show ideal behaviour.
- Above the Boyle point, real gases show positive deviation from ideality (forces of attraction between the particles are very feeble).
- Below Boyle point, real gases first show decrease in Z value with increasing pressure, reaches a minimum value, increases again on further increase in pressure.
- What is the actual significance of Z ? (I mean, intuitively )
- What is meant by positive deviation from ideality? If this is a measure of how Z value increases, I don't get it.
Ideal gases do not have forces of attraction between the constituent particles.
If we consider Z as:
how can a real gas show a positive deviation from ideality? ie. How can a real gas with a small amount of intermolecular force of attraction expand more than an ideal gas with zero intermolecular force of attraction?
- What is meant by negative deviation from ideality? What happens to a ideal gas when we apply pressure to it? Will we be able to compress it indefinitely But won't there be repulsive interactions even in such gases due to decrease in stability when huge amount of pressure is applied?
Any answer would be greatly appreciated.