How does the kinetic activity of gas molecules affect the pressure of a gas?

The correct choice highlights that faster-moving molecules will collide more frequently and with greater force, which directly contributes to an increase in gas pressure. In the context of gas laws, pressure is defined as the force exerted by gas molecules when they collide with the walls of their container.

As the temperature of a gas increases, the kinetic energy of its molecules also rises, resulting in more vigorous movements. This increase in speed leads to more frequent collisions against the container walls, which escalates the force exerted on those walls. Therefore, the pressure of the gas increases in accordance with the kinetic molecular theory, which posits that molecular motion is a key factor in determining gas behavior.

In summary, the kinetic activity of gas molecules fundamentally influences gas pressure through their speed and the resulting frequency and force of their collisions with surfaces.