A fixed mass of an ideal gas is contained in a cylinder at a constant temperature. Now, the pressure of the gas is decreased. What happened to the molecules of gas?
Correct answer: B. Number of collision between molecules and walls of container decreased
- A. Their mean square speed decreases
- B. Number of collision between molecules and walls of container decreased
- C. The force of attraction between them increase
- D. Their size decreases
Explanation
Pressure is proportional to temperature if the number of particles and the volume of the container is constant. Because the area of the container has increased, there will be fewer of these collisions per unit area and the pressure will decrease. Note; The question does not clarify if the volume is constant or not. We mustn't assume it is constant.
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About Kinetic Molecular Theory
Kinetic molecular theory explains gases as rapidly moving particles separated by large distances, with negligible volume and negligible intermolecular attraction in the ideal model. It relates temperature to average kinetic energy and explains gas pressure, Boyle's and Charles's laws, diffusion, effusion and the conditions under which real gases deviate from ideal behavior.
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