Graham's Law of Effusion Worksheet
Explore Graham's Law of Effusion with this Grade 10 Chemistry worksheet, covering the relationship between molecular mass and effusion rates.
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Graham's Law of Effusion
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Read each question carefully and answer to the best of your ability. Show all work for calculations.
Graham's Law of Effusion describes the relationship between the rate of effusion of a gas and its molar mass. Effusion is the process by which gas escapes through a tiny hole into a vacuum. The law states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass.
1. Which of the following gases would effuse the fastest at the same temperature and pressure?
He (Helium)
O₂ (Oxygen)
CO₂ (Carbon Dioxide)
Ar (Argon)
2. Graham's Law states that the rate of effusion is inversely proportional to the:
Molar mass of the gas
Square of the molar mass
Square root of the molar mass
Density of the gas
3. The process by which gas escapes through a tiny hole into a vacuum is called .
4. According to Graham's Law, lighter gases effuse than heavier gases.
5. Explain the importance of keeping temperature and pressure constant when comparing the effusion rates of two gases.
6. Diffusion and effusion are the exact same process.
True
False
7. A sample of an unknown gas effuses through a tiny hole in 45 seconds. An equal volume of fluorine gas (F₂) effuses through the same hole in 28 seconds. Calculate the molar mass of the unknown gas.