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.
The effusion rate of a gas is inversely proportional to the square root of its molar mass. This means that lighter gases effuse faster than heavier gases. This relationship is described by Graham's law of effusion.
You mean diffusion, and particles with smaller mass diffuse faster.
The rate of effusion decreases as mass increases
When the molar mass is lower the effusion is higher.
The rate of effusion of gases is inversely proportional to the square root of their molar masses. By comparing the molar masses of the two gases, you can determine which gas effuses faster. The gas with the lower molar mass will effuse more quickly.
The larger the particle size, the slower it will diffuse. This is given by Graham's Law of effusion which states that the rate of effusion is inversely related to the square root of the molar mass of the gas.
Hydrogen would effuse the fastest because it has the lowest molar mass among the gases mentioned. Effusion rate is inversely proportional to the square root of molar mass, so lighter gases effuse faster.
The rate of effusion for nitrogen is higher.
According to Graham's Law of Effusion, the rate of diffusion of a gas is inversely related to the square root of the molar mass. Thus, smaller (lighter) gases diffuse faster than larger, heavier gases. Molar mass of H2 = 2 and molar mass of C2H6 = 30. Sqrt 2 = 1.41 and sqrt 30 = 5.48, so the ratio is 5.48/1.41 = 3.88 or H2 will diffuse almost 4x faster (3.88x) than ethane. The ratio of H2/C2H6 would be the inverse, or 1.41/5.48 = 0.257, meaning that the rate of diffusion of ethane is about 26% that of hydrogen.
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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 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.
The larger the particle size, the slower it will diffuse. This is given by Graham's Law of effusion which states that the rate of effusion is inversely related to the square root of the molar mass of the gas.
The larger the particle size, the slower it will diffuse. This is given by Graham's Law of effusion which states that the rate of effusion is inversely related to the square root of the molar mass of the gas.
The rate of effusion of gases is inversely proportional to the square root of their molar masses. By comparing the molar masses of the two gases, you can determine which gas effuses faster. The gas with the lower molar mass will effuse more quickly.
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The variables involved in Graham's law are the molar mass of the gas particles and the rate of diffusion or effusion of the gas. The rate of diffusion or effusion is inversely proportional to the square root of the molar mass of the gas particles.
The larger the particle size, the slower it will diffuse. This is given by Graham's Law of effusion which states that the rate of effusion is inversely related to the square root of the molar mass of the gas.
molar mass of the gas. This means that lighter gas molecules effuse at a faster rate than heavier gas molecules at the same temperature.
Gas leaking through a small hole in its container is called effusion. The rate of effusion depends upon molar mass. The smaller the molar mass, the more quickly a gas will effuse out. Given these gases: He, Ar, CO2, helium will effuse out the fastest because its molar mass is only 4 (compared to 40 for argon and 44 for carbon dioxide.)