State two postulates of kinetic theory of gases which real gases do not obey?

Question: State two postulates of kinetic theory of gases which real gases do not obey?

While the kinetic theory of gases provides a useful model to understand the behavior of gases, there are two postulates that real gases do not always obey:

1. Postulate of Elastic Collisions: According to the kinetic theory of gases, gas molecules are considered to be perfectly elastic spheres that undergo collisions without any loss of kinetic energy. In reality, real gas molecules may experience intermolecular forces or collisions that result in energy loss. These deviations from ideal elastic collisions are more pronounced at higher pressures or lower temperatures.

2. Postulate of Negligible Volume: The kinetic theory assumes that gas molecules occupy negligible volume compared to the total volume of the gas. However, real gas molecules have finite volumes and can occupy a significant portion of the total volume, especially at high pressures. This leads to deviations from ideal gas behavior, particularly at high pressures and low temperatures when the volume occupied by the gas molecules becomes significant.

These deviations from the postulates of the kinetic theory of gases become more apparent under conditions where intermolecular forces, molecular size, and molecular interactions play a significant role. At high pressures or low temperatures, real gases tend to deviate from ideal gas behavior and exhibit non-ideal or "real" gas behavior.

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