Ch9 Gases Test Bank Docx

Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 09: Gases

1. On a very cold day, you notice that your tires look a bit deflated than warmer days. This observation can be explained by _____. (Outcome # 8) (DOK 2)
2. Boyles law
3. Ideal gas law
4. Charles law
5. What is the relationship between pressure and volume of a gas at constant temperature? (Outcome # 8) (DOK 2)
6. as volume decreases, pressure increases
7. as volume decreases, pressure decreases
8. as volume increases, pressure increases
9. How many mm Hg are in 0.890 atm of pressure? (Outcome # 8) (DOK 1)
10. 854 mm Hg
11. 676 mm Hg
12. 1.17 x 10^-3 mm Hg
13. How many atmospheres are in 710 mm Hg? (Outcome # 8) (DOK 1)
14. 0.934 atm
15. 1.07 atm
16. 5.40 x 10⁵ atm
17. The average tire pressure for an automobile is 38.5 psi which is how many atmospheres of pressure? (Outcome # 8) (DOK 1)
18. 1.77 x 10^-3 atm
19. 566 atm
20. 2.62 atm
21. What is the volume for 1.00 mole of gas at STP? (Outcome # 3) (DOK 2)
22. 24.5 L
23. 22.4 L
24. 2.05 L
25. What is the standard pressure for 1.00 mole of gas at STP? (Outcome # 3) (DOK 2)
26. 760 mm Hg
27. 1.03 atm
28. 103 kPa
29. 286 L of hydrogen gas at STP reacts with excess chorine gas. What is the maximum amount of gas product that can be formed at STP? (Outcome # 3) (DOK 3)
30. 572 L
31. 143 L
32. 286 L
33. 159 L of hydrogen gas at STP reacts with excess chorine gas. What is the maximum amount of gas product that can be formed at STP? (Outcome # 3) (DOK 3) (Paired item 1)
34. 159 L
35. 79.5 L
36. 318 L
37. A _____ is an instrument used to measure atmospheric pressure specifically in the area of meteorology. (Outcome # 10) (DOK 1)
38. barometer
39. manometer
40. altimeter
41. A _____ is a general instrument that utilizes a liquid column, typically mercury, to measure pressure. (Outcome # 10) (DOK 1)
42. barometer
43. manometer
44. altimeter
45. How many psi are in 760. mm Hg? (Outcome # 7) (DOK 1)
46. 1.47 x 10¹ psi
47. 3.93 x 10⁴ psi
48. 2.54 x 10^-5 psi
49. A sample of nitrogen gas occupies 9.20 L at 21 °C and 0.959 atm. If the pressure is increased to 1.15 atm at constant temperature, what is the newly occupied volume? (Outcome # 6) (DOK 1)
50. 11.0 L
51. 7.67 L
52. 9.20 L
53. The pressure of a gas in a container is 1.85 atm and occupies a volume of 12.5 L. If the original volume is reduced by half at constant temperature, what would happen to the pressure? (Outcome # 6) (DOK 2)
54. the pressure would double
55. the pressure would reduce by half
56. the pressure would remain the same
57. The pressure of a gas in a container is 1.23 atm and occupies a volume of 1.5 L. If the original volume is doubled at constant temperature, what would happen to the pressure? (Outcome # 6) (DOK 2)
58. the pressure would remain the same
59. the pressure would double
60. the pressure would reduce by half
61. Suppose your car is equipped with tire pressure monitoring system (TPMS) and the tire pressure is 34.0 psi on a 98 °F day in California. You decided to take a road trip to Alaska where the temperature drops to 20 °F. As you arrived in Alaska, you noticed that the tire pressure monitoring system alert light is illuminated. Why did this happen? (Outcome # 6) (DOK 3)
62. as temperature decreases, gas molecules lose kinetic energy and the volume of gas is reduced thus reducing the overall pressure in the tire which results in the TPMS to become activated
63. as temperature decreases, gas molecules gain kinetic energy and the volume of gas is reduced thus reducing the overall pressure in the tire which results in the TPMS to become activated
64. as temperature decreases, gas molecules lose kinetic energy and the volume of gas increases thus reducing the overall pressure in the tire which results in the TPMS to become activated
65. On a hot summer day, you notice that a bag of chips left in your vehicle has inflated. Why did this happen? (Outcome # 6) (DOK 3)
66. as temperature increases, gas molecules gain kinetic energy and the volume of gas decreases inside the bag of chips
67. as temperature increases, gas molecules lose kinetic energy and the volume of gas increases inside the bag of chips
68. as temperature increases, gas molecules gain kinetic energy and the volume of gas increases inside the bag of chips
69. What mass of nitrogen is needed to fill an 855 L tank at STP? (Outcome # 6) (DOK 3)
70. 0.978 kg
71. 1.07 kg
72. 0.533 kg
73. What mass of oxygen is needed to fill a 585 L tank at STP? (Outcome # 6) (DOK 3) (Paired item 1)
74. 0.835 kg
75. 0.765 kg
76. 0.417 kg
77. What is the pressure in a 5.80 L container that has 0.545 moles of oxygen gas at 22.0 °C? (Outcome # 6) (DOK 1)
78. 0.170 atm
79. 2.28 atm
80. 231 atm
81. What is the pressure in a 3.41 L container that has 0.741 moles of oxygen gas at 26.0 °C? (Outcome # 6) (DOK 1) (Paired item 1)
82. 5.34 atm
83. 0.464 atm
84. 62.0 atm
85. How many moles of CO₂ gas are present in a 9.1 L container at 25 °C and 1.35 atm? (Outcome # 6) (DOK 1)
86. 4.96 x 10^-3 moles
87. 5.99 moles
88. 0.502 moles
89. Oxygen gas (P_O2 = 1.10 atm), nitrogen gas (P_N2 = 0.840 atm), and carbon dioxide gas (P_CO2 = 0.125 atm) occupy the same container. What is the total pressure in the container? (Outcome # 6) (DOK 1)
90. 2.07 atm
91. 1.94 atm
92. 0.135 atm
93. A container filled with neon and argon gas is 25.00% by volume neon. What is the partial pressure of argon if the total pressure inside the container is 5.500 atm? (Outcome # 6) (DOK 2)
94. 412.5 atm
95. 1.375 atm
96. 4.125 atm
97. A container filled with helium and argon gas is 8.00% by volume argon. What is the partial pressure of argon if the total pressure inside the container is 4.100 atm? (Outcome # 6) (DOK 2) (Paired item 1)
98. 0.328 atm
99. 3.77 atm
100. 32.8 atm
101. What is the temperature for STP conditions? (Outcome # 4) (DOK 1)
102. 273.15 K
103. 298.15 K
104. 0 K
105. What is the pressure for STP conditions? (Outcome # 4) (DOK 1)
106. 740 mm Hg
107. 780 mm Hg
108. 760 mm Hg
109. 28.5 L of an unknown gas has a mass of 55.92 g at STP. What is the identity of the unknown gas? (Outcome # 4) (DOK 3)
110. CO₂
111. O₂
112. N₂