How is equilibrium achieved through diffusion?

Equilibrium through diffusion is achieved when the concentration of particles is evenly distributed throughout a system.

Diffusion is a process that involves the movement of particles from an area of high concentration to an area of low concentration. This movement continues until the concentration of particles is the same throughout the system, at which point equilibrium is achieved. The process of diffusion is driven by the kinetic energy of the particles, which causes them to move randomly.

In a closed system, such as a container of gas, the particles will continue to move and collide with each other and the walls of the container. Over time, these collisions will cause the particles to spread out evenly throughout the container. This is because there is a higher probability of particles moving from an area of high concentration to an area of low concentration than the other way around. Once the particles are evenly distributed, there is no net movement of particles, although individual particles continue to move randomly. This state is known as equilibrium.

In a liquid or a solution, the process is similar. Particles of a solute will move from an area of high concentration to an area of low concentration until they are evenly distributed throughout the solvent. Again, this is due to the higher probability of particles moving from an area of high concentration to an area of low concentration. Once equilibrium is achieved, there is no net movement of particles, although individual particles continue to move randomly.

It's important to note that achieving equilibrium does not mean that the movement of particles stops. Rather, it means that there is no net movement of particles because the rates of diffusion in opposite directions are equal. This is a dynamic process, with particles constantly moving and colliding, but with no overall change in the distribution of particles.