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Diffusion is the process by which particles (atoms, ions, or molecules) of a substance spread from areas of high concentration to areas of lower concentration in a fluid (liquid or gas) or across a permeable membrane because of their random motion, eventually leading to a uniform distribution. Some examples of diffusion are the spreading of perfume throughout a room and the mixing of two gases, such as oxygen and nitrogen.

Effusion is the process by which a gas escapes from a container into a vacuum or lower pressure environment through a small hole, orifice or porous material. The rate of effusion is determined by factors such as the mass of the gas particles and temperature. An example of effusion is the slow leaks of gas through a pinhole in a tire or balloon, where the lighter molecules will escape faster because of their higher average speed.

The key differences between diffusion and effusion are: 1. Diffusion involves the movement of particles (atoms, ions, or molecules) from regions of higher concentration to regions of lower concentration in a fluid, while effusion involves the passage of gas molecules from a container into a vacuum or lower pressure environment through a small hole. 2. In diffusion, the eventual result is a uniform distribution of particles throughout the fluid, whereas in effusion, the result is a decrease in the amount of gas within the container as the gas escapes. 3. Diffusion is generally a slower process as it involves the random movement of particles in all directions, whereas effusion occurs at a faster rate as the gas molecules escape through a small opening, primarily in one direction. In conclusion, while both diffusion and effusion involve the movement of gas particles, these processes are distinguished by their underlying mechanics and the environments in which they occur.