Name: ______________________
Class: _________________
Date: _________
Chpter 13 review
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
1. According to the kinetic theory, collisions between molecules in a gas
a. are perfectly elastic.
b. are inelastic.
c. never occur.
d. cause a loss of total kinetic energy.
____
2. Which of the following statements is true, according to the kinetic theory?
a. There is an attraction between particles of a gas.
b. Only particles of matter in the gaseous state are in constant motion.
c. The particles of a gas collide with each other and with other objects.
d. Collisions between particles result in a net loss of energy.
____
3. Particles in a gas
a. travel in straight-line paths until they collide with other objects.
b. usually travel uninterrupted indefinitely.
c. fill the bottom of their containers regardless of the shape or volume of the container.
d. follow an aimless path known as a free-range walk.
____
4. What instrument is normally used to measure atmospheric pressure?
a. thermometer
b. barometer
c. vacuum
d. manometer
____
5. What is the SI unit of pressure?
a. candela
b. mole
c. pascal
d. newton
____
6. What is one standard atmosphere of pressure in kilopascals?
a. 0 kPa
b. 760 kPa
c. 101.3 kPa
d. 1 kPa
____
7. Standard conditions when working with gases are defined as
a. 0 K and 101.3 kPa.
b. 0 K and 1 kPa.
c. 0°C and 101.3 kPa.
d. 0°C and 1 kPa.
1
ID: A
Name: ______________________
ID: A
____
8. What causes gas pressure in a container such as a helium balloon?
a. the walls of the container
b. the vacuum maintained in the container
c. the simultaneous collisions of fast-moving particles with the container
d. atmospheric pressure acting on the outside walls of the container
____
9. The
a.
b.
c.
d.
pressure of a gas in a container is 152 mm Hg. This is equivalent to
0.2 atm.
2 atm.
0.3 atm.
0.4 atm.
____ 10. What happens to the average kinetic energy of the particles in a sample of matter as the temperature of
the sample is increased?
a. The average kinetic energy decreases.
b. The average kinetic energy increases.
c. The average kinetic energy does not change.
d. The change in average kinetic energy cannot be determined.
____ 11. What happens to the range of energies of the particles in matter when the temperature is increased?
a. The range of energies becomes narrower.
b. The range of energies becomes broader.
c. The range of energies does not change.
d. The range of energies cannot be determined.
____ 12. The
a.
b.
c.
d.
average potential energy of water molecules is greatest in
steam at 100°C.
liquid water at 90°C.
liquid water at 373 K.
ice at 0°C.
____ 13. What is the key difference between a liquid and a gas?
a. intermolecular attractions
b. the ability to flow
c. average kinetic energy
d. the motion of their particles
____ 14. Which states of matter can flow?
a. gases only
b. liquids only
c. gases and liquids only
d. gases, liquids, and solids
____ 15. What happens to the temperature of a liquid as it evaporates?
a. It increases.
b. It decreases.
c. It does not change.
d. The change cannot be determined.
2
Name: ______________________
ID: A
____ 16. Which are the first particles to evaporate from a liquid?
a. particles with the lowest kinetic energy
b. particles with the highest kinetic energy
c. particles below the surface of the liquid
d. All particles evaporate at the same rate.
____ 17. Why does a liquid's rate of evaporation increase when the liquid is heated?
a. More molecules have enough energy to overcome the attractive forces holding them
in the liquid.
b. The average kinetic energy of the liquid decreases.
c. The surface area of the liquid is reduced.
d. The potential energy of the liquid increases.
____ 18. In a dynamic equilibrium between the liquid state and the gas state, what is true about the rate of
evaporation?
a. It is greater than the rate of condensation.
b. It is less than the rate of condensation.
c. It is equal to the rate of condensation.
d. The rate of evaporation cannot be determined.
____ 19. An
a.
b.
c.
d.
increase in the temperature of a contained liquid
has no effect on the kinetic energy of the liquid.
causes the vapor pressure above the liquid to decrease.
causes fewer particles to escape from the surface of the liquid.
causes the vapor pressure above the liquid to increase.
____ 20. What is the pressure when a liquid is boiling at its normal boiling point?
a. 0 kPa
b. 101.3 kPa
c. 202 kPa
d. 505 kPa
____ 21. When the external pressure is 505 kPa, what is the vapor pressure of water at its boiling point?
a. 0 kPa
b. 101.3 kPa
c. 505 kPa
d. 1010 kPa
____ 22. Which of the following best describes the motion of the particles in a piece of steel?
a. None are moving.
b. A few are moving.
c. All are moving.
d. Most are moving.
____ 23. The
a.
b.
c.
d.
physical properties of liquids is determined by
the disruptive motions of particles in a liquid only.
the attractions among the particles only.
the interplay between the disruptive motions of particles in a liquid and the
attractions among the particles.
either the disruptive motions of particles in a liquid or the attractions among the
particles.
3
Name: ______________________
ID: A
____ 24. Which of the following is an example of a phase?
a. pressure
b. water vapor
c. temperature
d. triple point
____ 25. How are conditions of pressure and temperature, at which two phases coexist in equilibrium, shown on a
phase diagram?
a. by a line separating the phases
b. by the endpoints of the line segment separating the phases
c. by the planar regions between lines in the diagram
d. by a triple point on the diagram
4
ID: A
Chpter 13 review
Answer Section
MULTIPLE CHOICE
1. ANS: A
PTS: 1
DIF: L1
REF: p. 420
OBJ: 13.1.1 Describe the three assumptions of the kinetic theory as it applies to gases.
BLM: knowledge
2. ANS: C
PTS: 1
DIF: L2
REF: p. 420
OBJ: 13.1.1 Describe the three assumptions of the kinetic theory as it applies to gases.
BLM: comprehension
3. ANS: A
PTS: 1
DIF: L2
REF: p. 420
OBJ: 13.1.1 Describe the three assumptions of the kinetic theory as it applies to gases.
BLM: comprehension
4. ANS: B
PTS: 1
DIF: L1
REF: p. 421
OBJ: 13.1.2 Interpret gas pressure in terms of kinetic theory.
BLM: knowledge
5. ANS: C
PTS: 1
DIF: L1
REF: p. 422
OBJ: 13.1.2 Interpret gas pressure in terms of kinetic theory.
BLM: knowledge
6. ANS: C
PTS: 1
DIF: L1
REF: p. 422
OBJ: 13.1.2 Interpret gas pressure in terms of kinetic theory.
BLM: knowledge
7. ANS: C
PTS: 1
DIF: L1
REF: p. 422
OBJ: 13.1.2 Interpret gas pressure in terms of kinetic theory.
BLM: knowledge
8. ANS: C
PTS: 1
DIF: L2
REF: p. 421
OBJ: 13.1.2 Interpret gas pressure in terms of kinetic theory.
BLM: comprehension
9. ANS: A
PTS: 1
DIF: L2
REF: p. 422
OBJ: 13.1.2 Interpret gas pressure in terms of kinetic theory.
BLM: analysis
10. ANS: B
PTS: 1
DIF: L1
REF: p. 423
OBJ: 13.1.3 Define the relationship between the temperature in kelvins and the average kinetic energy
of particles.
BLM: knowledge
11. ANS: B
PTS: 1
DIF: L1
REF: p. 423
OBJ: 13.1.3 Define the relationship between the temperature in kelvins and the average kinetic energy
of particles.
BLM: knowledge
12. ANS: A
PTS: 1
DIF: L2
REF: p. 430
OBJ: 13.2.4 Identify the conditions under which boiling occurs.
BLM: comprehension
13. ANS: A
PTS: 1
DIF: L2
REF: p. 425
OBJ: 13.2.1 Identify the factors that determine physical properties of a liquid.
BLM: comprehension
14. ANS: C
PTS: 1
DIF: L2
REF: p. 425
OBJ: 13.2.1 Identify the factors that determine physical properties of a liquid.
BLM: comprehension
1
ID: A
15. ANS: B
PTS: 1
DIF: L1
REF: p. 426
OBJ: 13.2.2 Define evaporation in terms of kinetic energy. BLM: knowledge
16. ANS: B
PTS: 1
DIF: L1
REF: p. 426
OBJ: 13.2.2 Define evaporation in terms of kinetic energy. BLM: knowledge
17. ANS: A
PTS: 1
DIF: L2
REF: p. 426
OBJ: 13.2.2 Define evaporation in terms of kinetic energy. BLM: comprehension
18. ANS: C
PTS: 1
DIF: L1
REF: p. 427
OBJ: 13.2.3 Define the conditions under which a dynamic equilibrium can exist between a liquid and its
vapor. BLM:
knowledge
19. ANS: D
PTS: 1
DIF: L2
REF: p. 427
OBJ: 13.2.3 Define the conditions under which a dynamic equilibrium can exist between a liquid and its
vapor. BLM:
knowledge
20. ANS: B
PTS: 1
DIF: L2
REF: p. 429
OBJ: 13.2.4 Identify the conditions under which boiling occurs.
BLM: comprehension
21. ANS: C
PTS: 1
DIF: L2
REF: p. 428
OBJ: 13.2.4 Identify the conditions under which boiling occurs.
BLM: application
22. ANS: C
PTS: 1
DIF: L2
REF: p. 431
OBJ: 13.3.1 Describe how the structure and properties of solids are related.
BLM: comprehension
23. ANS: C
PTS: 1
DIF: L1
REF: p. 425
OBJ: 13.2.1 Identify the factors that determine physical properties of a liquid.
BLM: knowledge
24. ANS: B
PTS: 1
DIF: L2
REF: p. 438
OBJ: 13.4.2 Determine how the conditions at which phases are in equilibrium are represented on a
phase diagram.
BLM: comprehension
25. ANS: A
PTS: 1
DIF: L2
REF: p. 438
OBJ: 13.4.2 Determine how the conditions at which phases are in equilibrium are represented on a
phase diagram.
BLM: comprehension
2