True or false? Gas pressure is caused by molecules in a gas colliding with the walls of their container.

Answer: True

Gas pressure is indeed caused by the collisions of gas molecules with the walls of their container. When gas molecules move, they occupy space and continuously collide with the surfaces that contain them. Each collision exerts a small force on the surface, and when many molecules collide with the walls, they collectively exert pressure.

This phenomenon can be explained further by the kinetic molecular theory, which states that gases are composed of many molecules that are in constant, random motion. The pressure exerted by a gas is proportional to the frequency and intensity of these collisions. Therefore, when the temperature increases, the kinetic energy of the molecules also increases, leading to more frequent collisions, and consequently, higher pressure if the volume remains constant.

In summary, the statement is true: gas pressure arises from the collisions of gas molecules against the walls of their container.