ACCORDING TO THE KINETIC THEORY OF GASES, WHICH OF THE FOLLOWING PROPERTY OF A GAS CAN BE AFFECTED BY THE COLLISION OF THE GAS MOLECULE WITH THE WALLS OF THE CONTAINER

• A. temperature
• B. energy
• C. viscosity
• D. pressure ✓

The kinetic theory of gases describes gases as being composed of particles (atoms or molecules) that are in constant, random motion. When these gas particles collide with the walls of their container, they exert a force on the walls, which results in pressure.

In other words, in the kinetic theory of gases, gases are considered to consist of a large number of small particles (atoms or molecules) that are in constant, random motion. When these gas particles collide with the walls of their container, they exert a force on the walls. This force per unit area is what we define as pressure in a gas.

As gas molecules move randomly and collide with each other and the walls of their container, they transfer momentum during these collisions. The more frequent and intense these collisions are, the higher the pressure exerted by the gas on the walls of its container. Therefore, pressure is directly influenced by the collisions between gas molecules and the walls of the container.

Temperature is related to the average kinetic energy of gas molecules but is not directly affected by collisions with the walls. Energy is a general term that encompasses various forms and interactions within a system but is not specifically altered by wall collisions in this context. Viscosity refers to a fluid’s resistance to flow and is more related to internal friction between fluid layers rather than wall collisions in gases.

In summary, when gas molecules collide with the walls of their container, it primarily affects pressure according to the kinetic theory of gases.