Rate of Effusion
When air particles escape or leak through a hole that has a width much smaller than the mean free path of the molecules, this action is known as an effusion of a gas. Due to the small amount of molecule-to-molecule collisions that occur in these regions, all particles and molecules that reach the hole will pass through throughout this procedure.
The process by which material particles from the enclosed space begin to escape over time might be referred to as the rate of effusion of a gas. An illustration can help make this process more understandable. For instance, imagine that when we cut a hole in a balloon, the gas inside would begin to escape into the atmosphere, causing the balloon to deflate from the inside out. The effusion of gas into the atmosphere is what this is known as.
As a result, we may state that a gas’ rate of effusion is inversely related to its density and molar mass.
Rate of Effusion = 1/√(density) = 1/√(Molar mass of the gas molecule)
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.
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