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The slowest rate of effusion will be exhibited by the gas with the highest molar mass. For example, Xenon will diffuse at a slower rate than Helium, and chlorine will diffuse at a slower rate than fluorine.
The rate of effusion is inversely related to the square root of the molar mass. Or stated another way, the larger or heavier the gas, the slower the effusion rate. Nitrogen gas (N2) has a molar mass of 28 g/mole and oxygen gas (O2) has a molar mass of 32 g/mole. Nitrogen will diffuse faster. rate N2/rate O2 = sqrt 32/sqrt 28 = 5.66/5.29 = 1.07. So, N2 effuses 1.07x faster than O2, or 7% faster. For more information on this, look up Graham's Law of Effusion.
Urea
gases with the higher molar mass
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The rate of effusion for nitrogen is higher.
Graham's law of effusion.
Graham's law of effusion states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass. In other words, lighter gases effuse or diffuse at a faster rate than heavier gases under the same conditions.
The slowest rate of effusion will be exhibited by the gas with the highest molar mass. For example, Xenon will diffuse at a slower rate than Helium, and chlorine will diffuse at a slower rate than fluorine.
A process related to diffusion is effusion, the process by which a gas escapes from a container into a vacuum through a small hole. The rate of effusion is also related to root mean square velocity-heavier molecules effuse more slowly than lighter ones. The rate of effusion-the amount of gas that effused in a given time- is inversely proportional to the square root of the molar mass of the gas.
An increase in a firm's expected growth rate would normally cause its required rate of return to
50000
The mortality of pleural effusion depends on various factors such as underlying cause, patient's overall health, and timely treatment. In general, if pleural effusion is treated promptly and effectively, the mortality rate is low. However, severe or untreated cases can lead to complications such as respiratory failure and sepsis, which can increase mortality risk.
The rate of effusion of two gases in a mixture is inversely proportional to the square roots of their molar masses.
Higher is the molecular mass lower is the rate of effusion, when mass increases by 4 times rate decreases to one half (Graham's law of diffusion).
Sulfur dioxide diffuses at one-quarter the rate of helium
one year