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Gases Multiple Choice Review Questions for AP Chemistry

based on 3 ratings
By — McGraw-Hill Professional
Updated on Feb 9, 2011

Review the following concepts if necessary:

Problems

You have 25 minutes to do the following questions. You may not use a calculator. You may use the periodic table at the back of the book. For each question, circle the letter of your choice.

  1. A sample of argon gas is sealed in a container. The volume of the container is doubled. If the pressure remains constant, what happens to the absolute temperature?
    1. It does not change.
    2. It is halved.
    3. It is doubled.
    4. It is squared.
    5. It cannot be predicted.
  2. A sealed, rigid container is filled with three ideal gases: A, B, and C. The partial pressure of each gas is known. The temperature and volume of the system are known. What additional information is needed to determine the masses of the gases in the container?
    1. the average distance traveled between molecular collisions
    2. the intermolecular forces
    3. the volume of the gas molecules
    4. the total pressure
    5. the molar masses of the gases
  3. Two balloons are at the same temperature and pressure. One contains 14 g of nitrogen and the other contains 20.0 g of argon. Pick the false statement from the following list.
    1. The density of the nitrogen sample is less than the density of the argon sample.
    2. The average speed of the nitrogen molecules is the same as the average speed of the argon molecules.
    3. The average kinetic energy of the nitrogen molecules is the same as the average kinetic energy of the argon molecules.
    4. The volume of the nitrogen container is the same as the volume of the argon container.
    5. The number of molecules in the nitrogen container is the same as the number of atoms in the argon container.
  4. An experiment to determine the molecular mass of a gas begins by heating a solid to produce a gaseous product. The gas passes through a tube and displaces water in an inverted, water-filled bottle. Which of the following necessary items may be determined after the experiment is completed?
    1. vapor pressure of water
    2. temperature of the displaced water
    3. barometric pressure in the room
    4. mass of the solid used
    5. volume of the displaced water
  5. The true volume of a particular real gas is larger than that calculated from the ideal gas equation. This occurs because the ideal gas equation does NOT correct for:
    1. the attraction between the molecules
    2. the shape of the molecules
    3. the volume of the molecules
    4. the mass of the molecules
    5. the speed the molecules are moving
  6. Aluminum metal reacts with HCl to produce aluminum chloride and hydrogen gas. How many grams of aluminum metal must be added to an excess of HCl to produce 33.6 L of hydrogen gas, if the gas is at STP?
    1. 18.0 g
    2. 35.0 g
    3. 27.0 g
    4. 4.50 g
    5. 9.00 g
  7. A reaction produces a gaseous mixture of carbon dioxide, carbon monoxide, and water vapor. After one reaction, the mixture was analyzed and found to contain 0.60 mol of carbon dioxide, 0.30 mol of carbon monoxide, and 0.10 mol of water vapor. If the total pressure of the mixture was 0.80 atm, what was the partial pressure of the carbon monoxide?
    1. 0.080 atm
    2. 0.34 atm
    3. 0.13 atm
    4. 0.24 atm
    5. 0.48 atm
  8. A sample of methane gas was collected over water at 35°C. The sample was found to have a total pressure of 756 mm Hg. Determine the partial pressure of the methane gas in the sample (vapor pressure of water at 35°C is 41 mm Hg).
    1. 760 mm Hg
    2. 41 mm Hg
    3. 715 mm Hg
    4. 797 mm Hg
    5. 756 mm Hg
  9. A sample of oxygen gas with a volume of 8.00 L at 127°C and 775 mm Hg is heated until it expands to a volume of 20.00 L. Determine the final temperature of the oxygen gas, if the pressure remains constant.
    1. 727°C
    2. 318°C
    3. 1000°C
    4. 160°C
    5. 45°C
  10. The average kinetic energy of nitrogen molecules changes by what factor when the temperature is increased from 30°C to 60°C?
  11. A 1.15-mol sample of carbon monoxide gas has a temperature of 27°C and a pressure of 0.300 atm. If the temperature is lowered to 17°C, at constant volume, what would be the new pressure?
    1. 0.290 atm
    2. 0.519 atm
    3. 0.206 atm
    4. 0.338 atm
    5. 0.310 atm
  12. An ideal gas sample weighing 1.28 grams at 127°C and 1.00 atm has a volume of 0.250 L. Determine the molar mass of the gas.
    1. 322 g/mol
    2. 168 g/mol
    3. 0.00621 g/mol
    4. 80.5 g/mol
    5. 49.4 g/mol
  13. Increasing the temperature of an ideal gas from 50°C to 75°C at constant volume will cause which of the following to increase for the gas?
    1. the average distance between the molecules
    2. the average speed of the molecules
    3. the average molecular mass of the gas
    1. III only
    2. I only
    3. II only
    4. II and III
    5. I and II
  14. If a sample of CH4 effuses at a rate of 9.0 mol per hour at 35°C, which of the gases below will effuse at approximately twice the rate under the same conditions?
    1. CO
    2. He
    3. O2
    4. F2
    5. SiH4
  15. A steel tank containing argon gas has additional argon gas pumped into it at constant temperature. Which of the following is true for the gas in the tank?
    1. There is no change in the number of gas atoms.
    2. There is an increase in the volume of the gas.
    3. There is a decrease in the pressure exerted by the gas.
    4. The gas atoms travel with the same average speed.
    5. The gas atoms are separated by a greater average distance.
  16. 2 N2O5(s) → 4NO2(g) O2(g)
  17. A 2 L evacuated flask has a 0.2 mol sample of N2O5(s) sealed inside it. The flask is heated to decompose the solid and cooled to 300 K. The N2O5(s) is completely decomposed according to the balanced equation above. What is the nearest value to the final total pressure of the gases in the flask? (The value of the gas constant, R, is 0.082 L atm mol–1 K–1.)

    1. 0.6 atm
    2. 6 atm
    3. 0.05 atm
    4. 1.2 atm
    5. 3 atm
  18. A glass container is filled, at room temperature, with equal numbers of moles of H2(g), O2(g), and NO2(g). The gases slowly leak out through a pinhole. After some of the gas has effused, which of the following is true of the relative values for the partial pressures of the gases remaining in the container?
    1. H2 < NO2 < O2
    2. NO2 < H2 < O2
    3. H2 = NO2 = O2
    4. O2 < NO2 < H2
    5. H2 < O2 < NO2
  19. Choose the gas that probably shows the greatest deviation from ideal gas behavior.
    1. He
    2. O2
    3. SF4
    4. SiH4
    5. Ar
  20. Determine the formula for a gaseous silane (SinH2n+2) if it has a density of 5.47 g per L at 0°C and 1.00 atm.
    1. SiH4
    2. Si2H6
    3. Si3H8
    4. Si4H10
    5. Si5H12
  21. Which of the following best explains why a hotair balloon rises?
    1. The heating of the air causes the pressure inside the balloon to increase.
    2. The cool outside air pushes the balloon higher.
    3. The temperature difference between the inside and outside air causes convection currents.
    4. Hot air has a lower density than cold air.
    5. Cooler air diffuses more slowly than the warmer air.
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