Law of effusion

This observation is now known as Graham s law of effusion. The rate of effusion is proportional to the average speed of the molecules in the gas because the average speed of the molecules determines the rate at which they approach the hole. Therefore, we can conclude that... 

The enrichment procedure uses the small mass difference between the hexafluorides of uranium-235 and uranium-238 to separate them. The first procedure to be developed converts the uranium into uranium hexafluoride, UFfl, which can be vaporized readily. The different effusion rates of the two isotopic fluorides are then used to separate them. From Graham s law of effusion (rare of effusion l/(molar mass)1/2 Section 4.9), the rates of effusion of 235UFfe (molar mass, 349.0 g-mol ) and 238UF6 (molar mass, 352.1 g-mol ) should be in the ratio... 

Graham s law of effusion The rate of effusion of a gas is inversely proportional to the square root of its molar mass. 

Graham s law of effusion / ley de la efusion de Graham establece que la tasa de efusion de un gas es inversamente proporcional a la rarz cuadrada de su masa en moles, (pig. 387)... 

Thomas Graham, a nineteenth-century Scottish chemist, did a series of experiments on the rate of effusion of gases. He found that at constant temperature, the rate of effusion of a gas is inversely proportional to the square root of its molar mass. This observation is now known as Graham s law of effusion. It follows that for two gases A and B ... 

This relation is Graham s law of effusion the ratio of the rates of effusion of two gases, at the same P and T, are inversely proportional to the square roots of their molar masses. 

Effusion and diffusion are substantially the same process. Diffusion is movement of a substance from an area of higher concentration to an area of lower concentration. Effusion is the movement of a gas through a small opening. Graham s Law of Effusion states the rate of effusion is inversely proportional to the square root of the molecular mass. 

One ramification of Eq. (18) is Graham s law of effusion, which deals with the rate at which gaseous molecules pass through a small hole in the wall of their enclosure (effusion). According to Graham, the rate per unit concentration is proportional to velocity and, thus, directly proportional to the square root of the absolute temperature and inversely proportional to the square root of the molecular mass. 

Thomas Graham developed Graham s Law of effusion and diffusion in the 1830s. He is called the father of colloid chemistry. 

D) Wrong Graham s law of effusion states that the rates of effusion are inversely related to the square root of the molar mass. This means that smaller particles will effuse more quickly than larger particles. All three balloons will get smaller at different rates, which means they will be different sizes on the next day (hydrogen will be smallest, followed by helium, and then sulfur hexafluoride). 

Graham s law of effusion states that the rate at which a gas effuses is inversely proportional to the molecular weight of the gas. 

Graham s Law of Effusion states that at the same temperature and pressure, gases diffuse at a rate inversely proportional to the square roots of their molecular masses. What this translates to is that lighter (less dense) gases travel faster than heavier (more dense) gases. 

You are given the molar masses for ammonia and hydrogen chloride. To find the ratio of the diffusion rates for ammonia and hydrogen chloride, use the equation for Graham s law of effusion. 

Graham s law of effusion (p. 387) hydrogen bond (p. 395) kinetic-molecular theory (p. 385)... 

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