Use the concepts of the kinetic-molecular model to explain: (a) why the pressure of a gas in a rigid container increases as heat is added to the gas and (b) why the pressure of a gas increases as we compress it, even if we do not change its temperature.

According to the Kinetic Molecular Theory of gases, the molecules of the gas experience perfectly elastic collisions and are constantly in motion. The average kinetic energy of the particles of an ideal gas is dependent only on the absolute temperature of the gas.

Adding heat to gas results in anincreasein theaveragekinetic energy of each gas atom. thisincreasestheaveragespeed and hence momentum. Therefore, gas exerts a greater force on the walls of thecontainer.

Therefore, Adding the heat to gas results in an increase in average kinetic energy which increases the average speed

Due to compression, the volume of the gas decreases, resulting in an increase in collision density and hence, collision pressure. Thus, the pressure is increased on compressing a gas.

Therefore, Due to the smaller volume collision pressure on the walls increases.