Name AP Chemistry: Reading Assignment—Gases 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? a. b. c. 2. c. d. e. It is squared. It cannot be predicted. the average distance traveled between molecular collisions the intermolecular forces the volume of the gas molecules the total pressure the molar masses of the gases The density of the nitrogen sample is less than the density of the argon sample. The average speed of the nitrogen molecules is the same as the average speed of the argon molecules. The average kinetic energy of the nitrogen molecules is the same as the average kinetic energy of the argon molecules. The volume of the nitrogen container is the same as the volume f the argon container. The number of molecules in the nitrogen container is the same as he number of atoms in the argon container. 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? a. b. c. 5. d. e. 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. a. b. 4. It does not change. It is halved. It is doubled. 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? a. b. c. d. e. 3. Class Period 18.0 g 35.0 g 27.0 g d. e. 4.50 g 9.00 g Choose the gas that probably shows the greatest deviation from ideal gas behavior. a. b. c. He O2 SF4 d. e. SiH4 Ar 6. 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 ml 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? a. b. c. 7. c. d. e. 797 mm Hg 756 mm Hg 727°C 318°C 1000°C d. e. 160°C 45°C (333-303) 2 d. e. √ 28 ⁄ 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? a. b. c. 11. 760 mm Hg 41 mm Hg 715 mm Hg The average kinetic energy of nitrogen molecules changes by what factor when the temperature is increased from 30°C to 60°C? a. b. 10. 0.24 atm 0.48 atm 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. a. b. c. 9. d. e. 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). a. b. c. 8. 0.080 atm 0.34 atm 0.13 atm 0.290 atm 0.519 atm 0.206 atm d. e. 0.338 atm 0.310 atm 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. a. b. c. 322 g/mol 168 g/mol 0.00621 g/mol d. e. 80.5 g/mol 49.4 g/mol 12. Increasing the temperature of an ideal gas from 50°C to 75°C at constant volume will cause which of the following to increase? I. the average distance between the molecules II. the average speed of the molecules III. the average molecular mass of the gas a. b. c. 13. II and III I and II CO He O2 d. e. F2 SiH4 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? a. b. c. d. e. 15. d. e. 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? a. b. c. 14. III only I only II only There is no change in the number of gas atoms. There is an increase in the volume of the gas. There is a decrease in the pressure exerted by the gas. The gas atoms travel with the same average speed. The gas atoms are separated by a greater average distance. A 2 L evacuated flask has a 0.2 mol sample of N2O(s) sealed inside it. The flask is heated to decompose the solid and cooled to 300 K. The N2O5(s) is completely decomposed according o the balanced equation below. What is the nearest value to the final total pressure of the gasses in the flask? (The value of the gas constant, R, is 0.082 L atm mol-1 K-1) 2 N2O5(s)  4 NO2(g) + O2(g) a. b. c. 16. 0.6 atm 6 atm 0.05 atm d. e. 1.2 atm 3 atm A glass container is filled, at room temperature, with equal numbers of moles of H 2(g), O2(g), ad 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? a. b. c. H2<NO2<O2 NO22< H <O2 H2=NO2=O2 d. e. O2<NO2< H2 H2<O2<NO2 17. 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. a. b. c. 18. SiH4 Si2H6 Si3H8 d. e. Si4H10 Si5H12 Which of the following best explains why a hot air balloon rises? a. b. c. d. e. The heating of the air causes the pressure inside the balloon to increase. The cool outside air pushes the balloon higher. The temperature difference between the inside and outside air causes convection currents. Hot air has a lower density than cold air. Cooler air diffuses more slowly than the warmer air.