Graham's Law Practice Quiz

What does Graham's Law primarily describe?

• The relationship between gas diffusion rates and molar mass
• The relationship between temperature and pressure of gases
• The behavior of gases under different volumes
• The chemical reactions of gases

If gas A has a molar mass of 4 g/mol and gas B has a molar mass of 16 g/mol, how does the rate of diffusion of gas A compare to gas B?

• Gas A diffuses faster
• Gas B diffuses faster
• Both gases diffuse at the same rate
• Gas A diffuses slower

According to Graham's Law, if the rate of diffusion of gas A is 2 m/s and the molar mass of gas A is 9 g/mol, what is the expected rate of diffusion of gas B with a molar mass of 36 g/mol?

• 1 m/s
• 2 m/s
• 4 m/s
• 0.5 m/s

Which of the following equations represents Graham's Law?

• Rate A / Rate B = √(Molar Mass B / Molar Mass A)
• Rate A / Rate B = Molar Mass A / Molar Mass B
• Rate A × Rate B = Molar Mass A + Molar Mass B
• Rate A - Rate B = Molar Mass A - Molar Mass B

What is the effect of increasing temperature on the rate of diffusion of a gas according to Graham's Law?

• It decreases the rate of diffusion
• It has no effect
• It increases the rate of diffusion
• It doubles the rate of diffusion

If two gases have the same temperature and pressure, which factor primarily affects their rate of diffusion?

• Molar mass
• Volume
• Density
• Color

Which gas would diffuse faster at the same temperature and pressure: helium (Molar mass = 4 g/mol) or oxygen (Molar mass = 32 g/mol)?

• Helium
• Oxygen
• Both diffuse at the same rate
• Neither diffuses

If the rate of diffusion of gas X is 3 times that of gas Y, what can be inferred about their molar masses?

• Gas X has a higher molar mass
• Gas Y has a higher molar mass
• Both gases have equal molar mass
• Gas Y has a lower molar mass

In a practical application of Graham's Law, which scenario would demonstrate the principle effectively?

• A balloon filled with helium rising
• A gas leak in a closed container
• Perfume spreading in a room
• A sealed jar of gas

How does the molar mass of a gas relate to its kinetic energy at a constant temperature?

• Higher molar mass means higher kinetic energy
• Lower molar mass means higher kinetic energy
• Molar mass has no effect on kinetic energy
• All gases have the same kinetic energy