molar mass
Argon is used to make argon
Curiously enough, the name of argon Is argon.
what are the uses of argon?
Argon does not have a hometown.
50000
The rate of effusion for nitrogen is higher.
Graham's law of effusion.
states that the rate of effusion for a gas is inversely proportional to the square root of its molar mass.
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 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
Graham's law states that the rate of effusion of a gas is inversely proportional to the square root of its molecular weight.Graham's law states that the rate of effusion of a gas is inversely proportional to the square root of its molecular weight.
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.)
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 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.