Gas molecules move constantly, any object in constant motion possesses kinetic energy. Overall at constant temperature and volume, the molecules of a gas have average kinetic energy.
Individual molecules yet have variation in kinetic energies because of distribution in speeds. When collisions among gas molecules occur, it gives rise to the distribution of speeds.
Because the collisions among gas particles are elastic and hence there is no loss of energy, and average kinetic energy of gas molecules does not change and remains the same.
At constant temperature and volume, the number of effective and ordinary collision of gases increases. This leads to an appreciable rise in the average kinetic energy of the gases. As more gases collides at a particular temperature, their collision raises their heat content. The gases begins to move more randomly and faster as they gain more kinetic energy.
The average kinetic energy drastically increases.
The average kinetic energy drastically increases when the gas particles collide against each other at a constant temperature and volume because the collision will increase the heat content of gas at a particular temperature and gas particles begin to move faster as gain more kinetic energy.
Hence, the correct answer is "B".
the average kinetic energy remains constant
Collisions between gas particles are elastic. An elastic collision means there is no net gain or loss of kinetic energy due to the collision. This means a sample of gas will have a constant average kinetic energy at a constant temperature and volume.