Graham's Law

Use Graham’s Law to calculate fast O₂ gas will effuse compared to Cl₂.

• O₂ effuses 1.5x faster than Cl₂

• O₂ effuses 0.11x as fast as Cl₂

• O₂ effuses 1.1x faster than Cl₂

• O₂ effuses 0.15x as fast as Cl₂

Grahams law refers specifically to

• the rate of diffusion

• the rate of effusion

• the temperature of gases

• the partial and total pressures of gases in a sample.

If the molar mass of gas 1 is 4.0 grams per mole and the molar mass of mass 2 is 10.0 grams per mole, what is the ratio of their speeds of diffusion?

• 1.6:1

• 2.5:1

• 25:1

• 0.0253:1

Lighter gases have a ________________ rate of effusion.

• faster 

• slower

• rate of effusion does not depend on mass.

An unknown gas diffuses 0.25 times as fast as helium gas (He). What is the molecular mass of the unknown gas?

• 64 g/mol

• 16 g/mol

• 32 g/mol

• 4 g/mol

Which of the following would have a faster rate of effusion?

• Helium

• Hydrogen

• Nitrogen

•     Oxygen

How much faster will He(g) travel than O₂(g)?

• 4 times faster

• 2.8 times faster

• 0.35 times faster

• 0.125 times faster

Tags

NGSS.HS-PS3-2

How much faster will gaseous hydrogen effuse than gaseous chlorine under the same physical conditions?

• 5.92

• 5.95

• 0.03

• 1.00

Calculate the relative rate of effusion of gaseous oxygen and nitrogen.

• 4.00

• 1.07

• 3.74

• 0.94

In order to calculate the rate of effusion of a gas, you must compare it to that of another gas and

• take the square root of the molar mass of the lighter gas divided by the square root of the molar mass of the heavier gas.

• take the square root of the molar mass of the heavier gas.

• take the square root of the molar mass of the lighter gas.

• take the square root of the molar mass of the heavier gas divided by the square root of the molar mass of the lighter gas.