What happens to the number of gas molecules colliding with the walls of a container when the volume of a gas increases?

When the volume of a gas increases while keeping the temperature and the amount of gas constant, the number of gas molecules per given volume decreases. This is due to the greater space in which the molecules can move. As a result, the frequency of collisions between the gas molecules and the walls of the container decreases.

In a larger volume, the gas molecules have to travel a greater distance to collide with the walls, thus reducing the overall number of collisions per unit of time. This behavior aligns with the principles of gas laws, particularly Boyle's law, which describes the inversely proportional relationship between pressure and volume when temperature remains constant. Therefore, the correct rationale for the situation described is that the number of collisions decreases as the volume of the gas increases.