The diffusion is the movement of one gas into another while effusion is the movement of gas through the aperture. Now we solve some examples related to diffusion and effusion of gases. The slow rate of diffusion in liquid can be observed by the following simple experiment: 1. i. raise in temperature is accompanied by an increase in the velocity at which the gas molecules move. The rate at which a gas will diffuse increases with increase in temperature an increase in temperature increases the kinetic energy of the gas molecules i.e. Figure \(\PageIndex{2}\): Diffusion occurs when gas molecules disperse throughout a container. The equation at the top of this page is Graham's Law of Diffusion, named after the Scottish chemist Thomas Graham (1805 - 1869). Statement.

It states that the diffusion rate of a gas is inversely proportional to the square root of its molar mass (molecular weight). Not all gases are alike, and due to their differing molecular masses, they move at different rates. Diffusion and Molecular Mass Explore the role of a molecule’s mass with respect to its diffusion rate. The same can be said for the rate of effusion. 2. Diffusion is driven by a gradient in concentration. The factors that affect the rate of diffusion of gases are described below. Graham’s Law Scottish chemist Thomas Graham experimentally determined that the ratio of the rates of effusion for two gases is equal to the square root of the inverse ratio of the gases’ molar masses.

We have studied in the previous unit that process of diffusion also occurs in liquids but the rate of diffusion in liquids is very slow. The greater the surface area, the faster the rate of diffusion Diffusion, surface area and volume For a bacterium, substances diffuse into and out of the bacterial cell across its surface. Rate of Diffusion: Rate of Diffusion = A m o u n t o f G a s P a s s i n g T h r o u g h a n A r e a U n i t o f T i m e \frac{Amount \;of \; Gas \; Passing \; Through \; an \; Area}{Unit \; of \; Time} U n i t o f T i m e A m o u n t o f G a s P a s s i n g T h r o u g h a n A r e a Here is an example to understand the diffusion of gases… Diffusion is the net movement of anything (for example, atom, ions, molecules) from a region of higher concentration to a region of lower concentration. DIFFUSION IN LIQUIDS IS MUCH SLOWER THAN THAT IN GASES. Take water in a long, clean transparent glass jar. Although diffusion and effusion rates both depend on the molar mass of the gas involved, their rates are not equal; however, the ratios of their rates are the same. The rate of diffusion of a gas ( measured in terms of number of moles of gas diffusing per unit time across unit area) is directly proportional to the pressure of the gas. Temperature.
Example: If gases X and SO 2 are send out at same time from points A and B, they meet at point 20 cm away from B. The rate of diffusion is given as:

The details of the rates of movement as they relate to molar mass are discussed in this section. Effusion rates of gases changes according to Graham's diffusion law. Expression. The law states the rate of diffusion or effusion of gases is inversely proportional to the square root of their respective molar masses at a given temperature and pressure. 9.16: Kinetic Theory of Gases - Graham's Law of Diffusion - Chemistry LibreTexts


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