practice test chapter 3
Completion
Complete each sentence or statement.
1. A(an) ____________________ has a definite volume and a definite shape.
2. The state of matter that exists only at extremely low temperatures is called a Bose-Einstein
____________________.
3. Materials can be classified as solids, liquids, or gases based on whether their shapes and
____________________ are definite or variable.
4. The shape of a material remains constant when it is moved from one container to another. This material is
a(an) ____________________.
5. The ____________________ theory of matter states that all particles of matter are in constant motion.
6. The motion of one particle of a gas is unaffected by the motion of other particles of the gas unless the
particles ____________________.
7. ____________________ between the particles of a gas and the walls of the container cause pressure in a
closed container of gas.
8. The pascal is the SI unit for ____________________.
9. Reducing the volume of a gas ____________________ its pressure if the ____________________ of the gas
and the number of particles are constant.
10. A graph representing Charles’s law shows that the ____________________ of a gas increases at the same rate
as the ____________________ of the gas.
11. The combined gas law describes the relationship among the ____________________,
____________________, and ____________________ of a gas when the number of particles is constant.
12. If you are using Charles’s law to find the volume of a gas at a certain temperature, the temperature must be
expressed in ____________________.
13. If you know the volume and pressure of a gas and the pressure changes, you can find the new volume by
multiplying P1 by V1 and ____________________ this number by P2.
14. The phase change that is the reverse of deposition is ____________________.
15. At sea level, water ____________________ at 100 C.
16. When water boils, some of its molecules have enough _________________________ to overcome the
attraction of neighboring molecules.
17. Water boils when its vapor pressure becomes equal to ____________________ pressure.
18. During vaporization, a substance changes from a(an) ____________________ to a(an)
____________________.
19. Evaporation is the process that changes a substance from a liquid to a gas at temperatures below the
substance’s ____________________ point.
20. During a(an) ____________________ change, the system releases energy to its surroundings.
Short Answer
21. Solid, liquid, and gas are three states of matter.What are two other states of matter, and under what conditions
do they exist?
22. Compare the shape and volume of solids, liquids, and gases.
23. Why is the volume of a liquid constant?
Figure 3-1
24. What substance in Figure 3-1 is a solid? Explain how you know.
25. Why does the air pressure in a car’s tires increase after a long drive?
26. If you push on the sides of a filled balloon, how does the gas pressure inside the balloon change? What
variable did you decrease to cause this change in pressure?
27. Charles’s law can be written as
. Explain what V1 and V2 represent.
28. If a gas has a volume of 1 L at a pressure of 200 kPa, what volume would it have when the pressure is
increased to 400 kPa? Assume the temperature and number of particles are constant.
29. If gas in a sealed container has a pressure of 50 kPa at 300 K, what will the pressure be if the temperature
rises to 360 K?
30. What two phase changes occur between solid water and liquid water, and at what temperature does each
phase change take place?
31. Explain why boiling water in a large pot on a stove has a temperature of 100 C even if it has been boiling for
an hour.
32. Describe what happens to the average kinetic energy of water molecules as water freezes.
33. Describe what happens to the arrangement of water molecules as ice melts.
34. Name and describe the phase change that occurs when dry ice is placed in an open container at room
temperature.
35. How could you determine if a phase change is endothermic?
Other
USING SCIENCE SKILLS
Figure 3-2
36. Interpreting Graphics Identify the phase changes in Figure 3-2 that are labeled a, b, and c.
37. Interpreting Graphics Explain why the phase changes in Figure 3-2 are shown in pairs.
38. Comparing and Contrasting Use the terms in Figure 3-2 to compare the phase changes that occur when
water vapor changes to dew or frost.
39. Interpreting Graphics Describe the two phase changes represented in Figure 3-2 that can happen to a liquid.
40. Applying Concepts What three phase changes in Figure 3-2 are endothermic?
Figure 3-3
41. Interpreting Graphics In Figure 3-3, what is the unit used for pressure? What is the pressure when the
volume is 0.5 L? What is the pressure when the volume is 1.0 L?
42. Interpreting Graphics In Figure 3-3, what is the manipulated variable, and what is the responding variable?
43. Predicting What would happen to the gas pressure in Figure 3-3 if the volume of the cylinder remained
constant and temperature was the manipulated variable?
44. Inferring Based on Figure 3-3, compare the collisions between particles of gas and the walls of a container
when the volume of gas is 1.0 L and when the volume is 2.0 L. Assume the number of particles does not
change. Explain any differences in collisions.
45. Interpreting Graphics In Figure 3-3, if P1 is 200 kPa and P2 is 50 kPa, what are V1 and V2?
practice test chapter 3
Answer Section
COMPLETION
1. ANS: solid
DIF: L1
2. ANS: condensate
OBJ: 3.1.1
DIF: L2
3. ANS: volumes
OBJ: 3.1.1
DIF: L1
4. ANS: solid
OBJ: 3.1.2
DIF: L1
5. ANS: kinetic
OBJ: 3.1.2
DIF: L1
6. ANS: collide
OBJ: 3.1.3
DIF: L2
7. ANS: Collisions
OBJ: 3.1.3
DIF: L1
8. ANS: pressure
OBJ: 3.2.1
DIF: L2
OBJ: 3.2.1
9. ANS: increases, temperature
DIF: L1
OBJ: 3.2.2
10. ANS: volume, temperature
DIF: L1
OBJ: 3.2.4
11. ANS: temperature, volume, pressure
DIF: L2
12. ANS: kelvins
OBJ: 3.2.4
DIF: L1
13. ANS: dividing
OBJ: 3.2.5
DIF: L2
14. ANS: sublimation
OBJ: 3.2.5
DIF: L2
15. ANS: boils
OBJ: 3.3.1
DIF: L2
16. ANS:
kinetic energy
speed
OBJ: 3.3.2
DIF: L2
17. ANS: atmospheric
OBJ: 3.3.3
DIF: L1
18. ANS: liquid, gas
OBJ: 3.3.4
DIF: L2
19. ANS: boiling
OBJ: 3.3.4
DIF: L2
20. ANS: exothermic
OBJ: 3.3.4
DIF: L1
OBJ: 3.3.5
SHORT ANSWER
21. ANS:
Plasma exists at extremely high temperatures, and a Bose-Einstein condensate exists at extremely low
temperatures.
DIF: L2
OBJ: 3.1.1
22. ANS:
Solids have a definite shape and definite volume, liquids have a definite volume but not a definite shape, and
gases do not have a definite volume or a definite shape.
DIF: L1
OBJ: 3.1.2
23. ANS:
The volume of a liquid is constant because forces of attraction keep the particles close together.
DIF: L1
OBJ: 3.1.3
24. ANS:
Substance A; its particles are packed close together and arranged in a regular pattern.
DIF: L2
OBJ: 3.1.3
25. ANS:
The constant motion of the tires on the road causes the tires and the air in the tires to warm up. The increase in
temperature increases the average kinetic energy of the air in the tires. The frequency and force of collisions
between particles increases, which increases the air pressure.
DIF: L1
OBJ: 3.2.2
26. ANS:
The gas pressure increased because the volume of the gas was decreased.
DIF: L1
OBJ: 3.2.3
27. ANS:
V1 is the volume of a gas before a change occurs, and V2 is the volume of a gas after a change occurs.
DIF: L1
OBJ: 3.2.4
28. ANS:
The new volume would be 0.5 L.
DIF: L1
OBJ: 3.2.5
29. ANS:
The new pressure would be 60 kPa.
DIF: L2
OBJ: 3.2.5
30. ANS:
Melting and freezing are the two phase changes that occur between solid water and liquid water, and they
both take place at 0 C.
DIF: L1
OBJ: 3.3.1
31. ANS:
A phase change is taking place as water boils and changes from a liquid to water vapor. The temperature of a
substance does not change during a phase change.
DIF: L1
OBJ: 3.3.2
32. ANS:
As water freezes, it releases energy to its surroundings, and the average kinetic energy of the water molecules
decreases.
DIF: L1
OBJ: 3.3.3
33. ANS:
At the melting point of water, some molecules gain enough energy to move from their fixed positions.
DIF: L2
OBJ: 3.3.3
34. ANS:
At room temperature, dry ice changes from solid carbon dioxide to carbon dioxide gas, which is an example
of sublimation.
DIF: L1
OBJ: 3.3.4
35. ANS:
Take the temperature measurements of the surroundings during the phase change. If the temperature
decreases, the phase change is endothermic; a system absorbs energy from its surroundings during an
endothermic phase change.
DIF: L2
OBJ: 3.3.5
OTHER
36. ANS:
a. vaporization, b. melting, c. freezing
DIF: L1
OBJ: 3.3.1
37. ANS:
Each pair represents the opposing endothermic and exothermic changes that occur between the same two
states of matter.
DIF: L1
OBJ: 3.3.1
38. ANS:
Water vapor is a gas. The phase change from water to liquid dew is called condensation. The phase change
from water vapor to solid frost is called deposition.
DIF: L1
OBJ: 3.3.4
39. ANS:
Vaporization is the phase change in which a liquid changes to a gas. Freezing is the phase change in which a
liquid changes to a solid.
DIF: L1
OBJ: 3.3.4
40. ANS:
melting, vaporization, and sublimation
DIF: L1
OBJ: 3.3.5
41. ANS:
the kilopascal; 200 kPa; 100 kPa
DIF: L2
OBJ: 3.2.2
42. ANS:
Volume is the manipulated variable. Pressure is the responding variable.
DIF: L2
OBJ: 3.2.2
43. ANS:
The pressure would increase as the temperature increased.
DIF: L2
OBJ: 3.2.3
44. ANS:
The number of collisions will increase when the volume is reduced from 2.0 L to 1.0 L because the same
number of particles occupies a smaller space and will collide more often with the walls of the container.
DIF: L2
OBJ: 3.2.3
45. ANS:
V1 is 0.5 L, and V2 is 2.0 L.
DIF: L2
OBJ: 3.2.4