How does diffusion demonstrate the kinetic theory of gases?

Diffusion demonstrates the kinetic theory of gases by showing the random, constant motion of gas particles.

The kinetic theory of gases states that gas particles are in constant, random motion and that they collide with each other and the walls of their container. This theory is clearly demonstrated through the process of diffusion. Diffusion is the movement of particles from an area of high concentration to an area of low concentration until they are evenly distributed. This process is driven by the kinetic energy of the particles, which is directly related to their temperature.

When a gas is released into a room, for example, it doesn't stay in one place. Instead, it spreads out to fill the entire room. This is because the gas particles are in constant motion, bouncing off each other and the walls of the room. Over time, the gas particles spread out evenly throughout the room, demonstrating the process of diffusion.

The speed at which diffusion occurs depends on the temperature of the gas. The higher the temperature, the faster the gas particles move and the quicker diffusion occurs. This is because temperature is a measure of the average kinetic energy of the particles. The more kinetic energy the particles have, the faster they move and the more frequently they collide with each other and the walls of their container.

In conclusion, diffusion is a clear demonstration of the kinetic theory of gases. It shows that gas particles are in constant, random motion and that they spread out to fill their container due to their kinetic energy. The speed of diffusion is also directly related to the temperature of the gas, further supporting the kinetic theory.