Understanding Mixtures of Gases and Partial Pressures

What is the largest component of dry air by volume?

• Oxygen

• Nitrogen

• Argon

• Carbon Dioxide

Which gas law is used to derive the expression for partial pressure?

• Ideal Gas Law

• Charles's Law

• Boyle's Law

• Avogadro's Law

What does Dalton's Law of Partial Pressure state about the total pressure in a gas mixture?

• It is the product of the partial pressures.

• It is the difference between the highest and lowest partial pressures.

• It is equal to the sum of the partial pressures.

• It is the average of the partial pressures.

What is the mole fraction of a gas in a mixture?

• The ratio of the gas's volume to the total volume.

• The ratio of the gas's moles to the total moles.

• The ratio of the gas's pressure to the total pressure.

• The ratio of the gas's mass to the total mass.

How can you calculate the partial pressure of a gas using its mole fraction?

• Multiply the mole fraction by the total volume.

• Multiply the mole fraction by the total pressure.

• Divide the mole fraction by the total pressure.

• Add the mole fraction to the total pressure.

In the example problem, what is the total pressure of the gas mixture?

• 0.87 atm

• 5.0 atm

• 1.71 atm

• 2.42 atm

What is the partial pressure of xenon in the example problem?

• 1.71 atm

• 5.0 atm

• 2.42 atm

• 0.87 atm

Which constant is used in the ideal gas law to calculate moles from pressure, volume, and temperature?

• 1.00 atm

• 8.314 J/mol K

• 0.08206 L atm/mol K

• 22.4 L/mol

What is the temperature used in the example problem?

• 310.15 K

• 273.15 K

• 250.15 K

• 298.15 K

How many moles of xenon are calculated in the example problem?

• 0.19 moles

• 2.42 moles

• 1.71 moles

• 0.87 moles