Multiple Choice
Identify the choice that best completes the statement or answers the question.
____ 1. Pressure is the force per unit c. length. d. depth. a. volume. b. surface area.
____ 2. Why does a can collapse when a vacuum pump removes air from the can? a. The inside and outside forces balance out and crush the can. b. The unbalanced outside force from atmospheric pressure crushes the can. c. The atmosphere exerts pressure on the inside of the can and crushes it. d. The vacuum pump creates a force that crushes the can.
____ 3. If the height of mercury in a barometer at 0

C is less than 760 mm Hg, then a. the atmospheric pressure is less than standard atmospheric pressure. b. the atmospheric pressure is greater than standard atmospheric pressure. c. the atmospheric pressure is equal to standard atmospheric pressure. d. the atmospheric pressure cannot be determined.
____ 4. Convert the pressure 0.840 atm to mm Hg. a. 365 mm Hg b. 437 mm Hg c. 638 mm Hg d. 780 mm Hg
____ 5. Convert the pressure 1.30 atm to kPa. a. 2 kPa b. 115 kPa
____ 6. Standard temperature is exactly a. 100

C. b. 273

C. c. 132 kPa d. 245 kPa c. 0

C. d. 0 K.
____ 7. Three samples of gas each exert 740. mm Hg in separate 2 L containers. What pressure do they exert if they are all placed in a single 2 L container? a. 247 mm Hg b. 740 mm Hg c. 1.48 10 d. 2.22 10
3
3
mm Hg
mm Hg
____ 8. If the temperature remains constant, V and P represent the original volume and pressure, and V' and P' represent the new volume and pressure, what is the mathematical expression for Boyle's law? a. P'V = V'P c. VP= V'P' b. VV' = PP' d.
____ 9. A sample of oxygen occupies 560. mL when the pressure is 800.00 mm Hg. At constant temperature, what volume does the gas occupy when the pressure decreases to 700.0 mm Hg? a. 80.0 mL b. 490. mL c. 600. mL d. 640. mL
____ 10. If the temperature of a fixed quantity of gas decreases and the pressure remains unchanged, a. its volume increases. b. its volume is unchanged. c. its volume decreases. d. its density decreases.

____ 11. The volume of a gas is 5.0 L when the temperature is 5.0

C. If the temperature is increased to 10.0

C without changing the pressure, what is the new volume? a. 2.5 L c. 5.1 L b. 4.8 L d. 10.0 L
____ 12. On a cold winter morning when the temperature is –13

C, the air pressure in an automobile tire is 1.5 atm. If the volume does not change, what is the pressure after the tire has warmed to 15

C? c. 3.0 atm d. 19.5 atm a. –1.5 atm b. 1.7 atm
____ 13. If V , P , and T represent the original volume, pressure, and temperature in the correct units, and V' , P' , and T' represent the new conditions, what is the combined gas law? a. c. b. d.
____ 14. The volume of a gas collected when the temperature is 11.0

C and the pressure is 710 mm Hg measures 14.8 mL. What is the calculated volume of the gas at 20.0

C and 740 mm Hg? a. 7.8 mL b. 13.7 mL c. 14.6 mL d. 15 mL
____ 15. If 0.5 L of O
2
( g ) reacts with H
2
to produce 1 L of H
2
O( g ), what is the volume of H
2
O( g ) obtained from 1 L of
O
2
( g )? a. 0.5 L c. 2 L d. 2.5 L b. 1.5 L
____ 16. Volumes of gaseous reactants and products in a chemical reaction can be expressed as ratios of small whole numbers a. if all reactants and products are gases. b. if standard temperature and pressure are maintained. c. if constant temperature and pressure are maintained. d. if each mass equals 1 mol.
____ 17. What is the number of moles of H
2
produced when 23 g of sodium react with water according to the equation
2Na( s ) + 2H
2
O( l ) 2NaOH( aq ) + H
2
( g )? a. 0.50 mol b. 1.0 mol c. 2.0 mol d. 4.0 mol
____ 18. If the temperature of a container of gas remains constant, how could the pressure of the gas increase? a. The mass of the gas molecules increase. b. The diffusion of the gas molecules increases. c. The size of the container increases. d. The number of gas molecules in the container increases.
____ 19. At constant temperature and pressure, gas volume is directly proportional to the a. molar mass of the gas. c. density of the gas at STP. d. rate of diffusion. b. number of moles of gas.
____ 20. The standard molar volume of a gas is all of the following except a. the volume occupied by 1 mol of a gas at STP. b. equal for all gases under the same conditions.

c. 22.4 L at STP. d. dependent upon the size of the molecules.
____ 21. A 1.00 L sample of a gas has a mass of 1.92 g at STP. What is the molar mass of the gas? a. 1.92 g/mol b. 19.2 g/mol c. 22.4 g/mol d. 43.0 g/mol
____ 22. Chlorine is produced by the reaction 2HCl( g )

H
2
( g ) + Cl
2
( g ). How many grams of HCl (36.5 g/mol) must be used to produce 10.0 L of chlorine at STP? a. 15.8 g b. 30.2 g c. 32.6 g d. 36.5 g
____ 23. Calculate the approximate volume of a 0.600 mol sample of gas at 15.0°C and a pressure of 1.10 atm. a. 12.9 L b. 22.4 L c. 24.6 L d. 139 L
____ 24. What is the pressure exerted by 1.2 mol of a gas with a temperature of 20.

C and a volume of 9.5 L? c. 3.0 atm d. 30. atm a. 0.030 atm b. 1.0 atm
____ 25. What is the process by which molecules of a gas randomly encounter and pass through a small opening in a container? a. diffusion b. vaporization c. distillation d. effusion
____ 26. When the temperature of a gas is increased within a closed container, pressure increases due to which of the following? a. The frequency of collisions between molecules and the container walls decreases. b. The frequency of collisions between molecules and the container walls increases. c. The spaces between the molecules of gas decrease. d. The gas turns into a liquid.
____ 27. Gas A and gas B (both unreactive) are allowed to mix. The total pressure is found to be 3.50 atm. If gas B was measured initially at 1.25 atm, what is the partial pressure of gas A? a.
4.75 atm b.
-2.25 atm c.
2.25 atm d.
1.25 atm
____ 28. Calculate the volume of 12.0 g of helium at 100°C and 1.2 atm. a. 0.013 L b. 76.5 L c. 7,750 L d. 56.0 L
____ 29. 5.0 L of a gas goes from 1.0 atm to 1.3 atm. Calculate the final volume of this gas. a. 6.5 L b. 0.26 L c. 4.1 L d. 3.8 L
____ 30. The graph below shows a plot of volume versus pressure for a particular gas sample at constant temperature. Use it to answer questions 6 and 7.

What is the volume of this gas at 4.0 atm pressure? a. 0.68 L b. 1.0 L c. 0.5 L d. 4.0 L
____ 31. At what pressure would this gas occupy a volume of 5.0 L? a. 0.4 atm b. 0.33 atm c. 2.0 atm d. 0.5 atm
Choose the best answer from the options that follow each question.
____ 32. Air is about 78% nitrogen, 21% oxygen, and 1% other gases. After all the oxygen is removed from a sample of air in a glass tube and the temperature remains constant, the pressure exerted by the remaining air a. does not change. b. is reduced by 78%. c. is reduced by 50%. d. is reduced by 21%.
____ 33. Which of the following expressions relates the kelvin and Celsius temperature scales? a. K = 273.15 + °C b. K= 273.15 + °C c. °C + 273.15 K d. K = 273.15°C
____ 34. You collect 552 mL of argon gas at 23.0°C. What volume will the gas occupy at 46.0°C if the pressure remains constant? a. 276 mL b. 512 mL c. 595 mL

d. 1104 mL
Short Answer
1. Why do your ears "pop" in an airplane?
2. What are standard temperature and pressure? Why is a standard necessary?
3. A gas has a volume of 5 L at 120 K. What is its volume (in liters) at 100 K? (Round to nearest thousandth.)
Completion
Complete each statement.
PART II Write the correct term (or terms) in the space provided.
1. The pressure of a gas is directly proportional to the number of moles of the gas if both volume and
____________________ are constant.
2. The force per unit area on a surface is called ____________________.
3. The pressure exerted by each gas in a mixture is called the ____________________ of that gas.
4. The lowest possible temperature, corresponding to zero on the kelvin scale, is referred to as
____________________.
Matching
PART III For each expression in the first column, write the letter of the expression in the second column that is most closely related. a. Dalton’s law b. Charles’s law c. Gay-Lussac’s law d. Boyle’s law e. combined gas law f. Pascal’s law g. gas pressure law h. ideal gas law i. Gay-Lussac’s law of combining volumes j. Avogadro’s law k. Graham’s law
____ 1. The pressure of a fixed mass of gas varies directly with the kelvin temperature at constant volume
____ 2. The volume of a fixed mass of gas varies inversely with the pressure at constant temperature.
____ 3. At constant temperature and pressure, the volumes of gaseous reactants and products can be expressed as ratios of small whole numbers.

____ 4. Equal volumes of gases at the same temperature and pressure contain equal numbers of molecules.
____ 5. The total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gases.
____ 6. The relationship between pressure, volume, and temperature is expressed by this law.
____ 7. Pressure times volume equals molar amount times 0.0821 L atm/(mol K) times temperature in kelvins.
____ 8. The rates of effusion of gases at the same temperature and pressure are inversely proportional to their molar masses.
____ 9. The volume of a fixed mass of gas varies directly with the kelvin temperature at constant pressure.

MULTIPLE CHOICE
1. ANS: B PTS: 1 DIF: I
REF: cf2425e4-f97e-11de-9c72-001185f0d2ea
2. ANS: B PTS: 1 DIF: II
REF: cf2911ae-f97e-11de-9c72-001185f0d2ea
3. ANS: A PTS: 1 DIF: II
REF: cf2dd668-f97e-11de-9c72-001185f0d2ea
4. ANS: C
Solution:
OBJ: 1
OBJ: 1
OBJ: 2
PTS: 1
OBJ: 2
5. ANS: C
Solution:
DIF: II REF: cf329b22-f97e-11de-9c72-001185f0d2ea
PTS: 1
OBJ: 2
DIF: II REF: cf3738cc-f97e-11de-9c72-001185f0d2ea
6. ANS: C PTS: 1 DIF: I
REF: cf375fdc-f97e-11de-9c72-001185f0d2ea OBJ: 2
7. ANS: D
9. ANS: D
Solution:
PTS: 1 DIF: III
REF: cf40e950-f97e-11de-9c72-001185f0d2ea
8. ANS: C PTS: 1 DIF: I
REF: cf4a4bb4-f97e-11de-9c72-001185f0d2ea
OBJ: 3
OBJ: 2
PTS: 1
OBJ: 2
DIF: III REF: cf4cae11-f97e-11de-9c72-001185f0d2ea
10. ANS: C PTS: 1 DIF: I
REF: cf4f106e-f97e-11de-9c72-001185f0d2ea
11. ANS: C
Solution:
OBJ: 3
PTS: 1 DIF: III REF: cf5172cb-f97e-11de-9c72-001185f0d2ea

OBJ: 3
12. ANS: B
Solution:
PTS: 1
OBJ: 4
DIF: III REF: cf5b234f-f97e-11de-9c72-001185f0d2ea
13. ANS: D PTS: 1 DIF: I
REF: cf5fc0f9-f97e-11de-9c72-001185f0d2ea
14. ANS: C
Solution:
OBJ: 5
PTS: 1
OBJ: 5
15. ANS: C
Solution:
DIF: III REF: cf622356-f97e-11de-9c72-001185f0d2ea
PTS: 1
OBJ: 1
DIF: II REF: cf670f20-f97e-11de-9c72-001185f0d2ea
16. ANS: C PTS: 1 DIF: I
REF: cf6bacca-f97e-11de-9c72-001185f0d2ea OBJ: 1
17. ANS: A
Solution:
PTS: 1
OBJ: 1
DIF: III REF: cf707184-f97e-11de-9c72-001185f0d2ea
18. ANS: D PTS: 1 DIF: I
REF: cf75363e-f97e-11de-9c72-001185f0d2ea OBJ: 2
19. ANS: B
21. ANS: D
Solution:
PTS: 1 DIF: I
REF: cf79faf8-f97e-11de-9c72-001185f0d2ea
20. ANS: D PTS: 1 DIF: I
REF: cf81491f-f97e-11de-9c72-001185f0d2ea
OBJ: 2
OBJ: 3
PTS: 1
OBJ: 3
DIF: III REF: cf884926-f97e-11de-9c72-001185f0d2ea

22. ANS: C
Solution:
PTS: 1
OBJ: 3
23. ANS: A
Solution:
PTS: 1
OBJ: 5
24. ANS: C
Solution:
DIF: III
DIF: III
REF: cf8ad293-f97e-11de-9c72-001185f0d2ea
REF: cf9b5c0e-f97e-11de-9c72-001185f0d2ea
PTS: 1
OBJ: 5
DIF: III REF: cf9dbe6b-f97e-11de-9c72-001185f0d2ea
25. ANS: D PTS: 1 DIF: I
REF: cfa4e582-f97e-11de-9c72-001185f0d2ea OBJ: 1
26. ANS: B PTS: 1 STA: TEKS C.9C
TOP: Chemistry Chapter 11 - Standardized Test Practice
27. ANS: C PTS: 1 STA: TEKS C.9A
TOP: Chemistry Chapter 11 - Standardized Test Practice
28. ANS: B PTS: 1 STA: TEKS C.9A
TOP: Chemistry Chapter 11 - Standardized Test Practice
29. ANS: D PTS: 1 STA: TEKS C.9A
TOP: Chemistry Chapter 11 - Standardized Test Practice
30. ANS: C PTS: 1 STA: TEKS C.9A
TOP: Chemistry Chapter 11 - Standardized Test Practice
31. ANS: A PTS: 1 STA: TEKS C.9A
TOP: Chemistry Chapter 11 - Standardized Test Practice
32. ANS: D
33. ANS: A
34. ANS: C
PTS: 1
PTS: 1
PTS: 1
TOP: Chapter 11 Test A
TOP: Chapter 11 Test A
STA: TEKS C.9A TOP: Chapter 11 Test A
SHORT ANSWER
1. ANS:
Changes in density as altitude increases cause your ears to "pop." The atmosphere is denser closer to the surface of Earth. As an airplane rises in altitude, there is less air pressure. The "pop" occurs when the air inside your ears changes to the same pressure as the outside air.
PTS: 1
OBJ: 1
DIF: II REF: cfb5960d-f97e-11de-9c72-001185f0d2ea

2. ANS:
Standard temperature is 0

C, and standard pressure is 1 atm. Scientists have agreed upon standard conditions for temperature and pressure to compare volumes of gases.
PTS: 1
OBJ: 2
DIF: II REF: cfb5bd1d-f97e-11de-9c72-001185f0d2ea
3. ANS:
4.167 L
PTS: 1 STA: TEKS C.9A TOP: Chemistry Chapter 11 - Standardized Test Practice
COMPLETION
1. ANS: temperature
PTS: 1
2. ANS: pressure
PTS: 1
STA: TEKS C.9A TOP: Chapter 11 Test B
TOP: Chapter 11 Test B
3. ANS: partial pressure
PTS: 1 STA: TEKS C.9A TOP: Chapter 11 Test B
4. ANS: absolute zero
PTS: 1
MATCHING
1. ANS: C
2. ANS: D
3. ANS: I
4. ANS: J
5. ANS: A
6. ANS: E
7. ANS: H
8. ANS: K
9. ANS: B
TOP: Chapter 11 Test B
PTS: 1
PTS: 1
PTS: 1
PTS: 1
PTS: 1
PTS: 1
PTS: 1
PTS: 1
PTS: 1
STA: TEKS C.9A TOP: Chapter 11 Test B
TOP: Chapter 11 Test B
TOP: Chapter 11 Test B
TOP: Chapter 11 Test B
TOP: Chapter 11 Test B
TOP: Chapter 11 Test B
TOP: Chapter 11 Test B
TOP: Chapter 11 Test B
TOP: Chapter 11 Test B