Above Boyle temperature real gases show positive deviation from ideal gases.

Explanation:
When describing the behavior of gases, the ideal gas law is often used as a simplified model. However, real gases deviate from ideal gas behavior under certain conditions. One such condition is when the temperature of the gas is above the Boyle temperature.

Boyle temperature:
The Boyle temperature, also known as the Boyle point, is the temperature at which the real gas deviates from ideal gas behavior. Above this temperature, the gas molecules experience intermolecular attractions and occupy a larger volume compared to an ideal gas.

Positive deviation:
When a real gas exhibits positive deviation from ideal gas behavior, it means that the observed pressure of the gas is higher than what would be predicted by the ideal gas law. This occurs because the intermolecular forces between the gas particles become significant at higher temperatures, causing the gas to occupy more space and exert a higher pressure.

Causes of positive deviation:
Several factors contribute to the positive deviation of real gases from ideal gases above the Boyle temperature:
1. Intermolecular attractions: Real gases experience attractive forces between molecules. At higher temperatures, these forces become significant and cause the gas particles to come closer together, resulting in an increase in pressure compared to an ideal gas.
2. Molecular size: Real gas molecules have a finite size, whereas ideal gas molecules are assumed to have negligible size. As the temperature increases, the volume occupied by the real gas molecules becomes more significant, leading to a higher pressure.
3. Non-ideal behavior: Real gases may also exhibit non-ideal behavior due to factors such as dipole-dipole interactions, hydrogen bonding, or van der Waals forces. These interactions contribute to the positive deviation observed above the Boyle temperature.

Conclusion:
In summary, above the Boyle temperature, real gases show positive deviation from ideal gases. This is due to factors such as intermolecular attractions, molecular size, and non-ideal behavior. The positive deviation results in a higher observed pressure compared to what would be expected from the ideal gas law.