Rate of Diffusion
Diffusion of a gas is the term used to describe the net movement of the substance from the area of higher concentration to the area of lower concentration. Each gas particle starts crashing into one another. The maximum particle density zone of a gas causes the particles to begin bouncing off of each other and the border container at a faster pace than the particles in the lower particle density regions.
The rate of gas diffusion, according to effusion, is inversely proportional to the square root of the density of a gas molecule. A gas’s density is determined by dividing its mass by its volume to determine the density of a given gas molecule. It is possible to compare two gases if the gas molecule’s volume is kept constant.
Graham’s Law of Diffusion
Graham’s law of diffusion is the relationship between a gas’s rate of diffusion or effusion and its molecular weight. The law of diffusion’s basic tenet is that any gas’s rate of diffusion, at any given temperature and pressure, is inversely proportional to the square root of its density. The mechanism by which a gas can escape from the container is known as effusion, and the ability of a gas to spread and occupy all of the volumes that are available to it is known as diffusion.