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The rate of effusion of a gaseous substance is inversely proportional to the square root of its molar mass. This relationship is referred to as Graham’s law, after the Scottish chemist Thomas Graham (1805–1869).
- Diffusion
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- Diffusion
Graham's law states that the rate of diffusion or of effusion of a gas is inversely proportional to the square root of its molecular weight. Thus, if the molecular weight of one gas is four times that of another, it would diffuse through a porous plug or escape through a small pinhole in a vessel at half the rate of the other (heavier gases ...
Named after Scottish chemist Thomas Graham, who formulated it in 1848, this law is significant in understanding how gases behave at the molecular level. It is based on the Kinetic Molecular Theory, which describes how gas particles move and interact with each other.
25 cze 2023 · Graham's law of diffusion states that the ratio of the diffusion rate of two gases is the same as the ratio of the square root of the molar mass of the gases.
Graham's law states that the rate of diffusion or effusion of a gas is inversely proportional to the square root of the molar masses of its particles. Essentially, lighter gases will effuse/diffuse faster than heavier ones.
Graham's law calculates the rate of diffusion or effusion and molar mass of gases. The equation of Graham's law is: rate 1 / rate 2 = √ (mass 2 / mass 1) rate 1 and rate 2 - Rates of effusion or diffusion of Gas 1 and 2, respectively; mass 1 and mass 2 - Molar masses of Gas 1 and 2, respectively.
Graham’s law states that the rate of diffusion or effusion of a gas is inversely proportional to the square root of its molar mass. The Formula can be written as. M1 is the molar mass of gas 1. M2 is the molar mass of gas 2. Rate1 is the rate of effusion of the first gas.
