At constant volume,the temperature of a gas i | vedclass

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(B) According to the kinetic theory of gases,the average kinetic energy of gas molecules is directly proportional to the absolute temperature $(KE_{av

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Number of collisions per unit time will increase

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(B) According to the kinetic theory of gases,the average kinetic energy of gas molecules is directly proportional to the absolute temperature $(KE_{avg} \propto T)$.As the temperature increases,the average velocity $(v_{rms} \propto \sqrt{T})$ of the gas molecules increases.Since the molecules move faster,they strike the walls of the container more frequently per unit time.Therefore,the number of collisions per unit time increases.

At constant volume,the temperature of a gas is increased. Then:

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