We’re being asked to explain the deviations from the ideal gas law often observed at high pressure and low temperature in light of kinetic molecular theory.
First, let’s state the basic postulates or assumptions of the Kinetic molecular theory:
1. The size of a particle is negligibly small
2. The average kinetic energy of a particle is proportional to the temperature in Kelvins.
3. The collision of one particle with another (or with the walls of its container) is completely elastic.
Deviations from the ideal gas law are often observed at high pressure and low temperature.
Explain why in light of kinetic molecular theory.
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