Chapter 13 Student Worksheets 4w395g
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THE NATURE OF GASES
13.1
Section Review Objectives • Describe the assumptions of the kinetic theory as it applies to gases • Interpret gas pressure in of kinetic theory • Define the relationship between Kelvin temperature and average kinetic energy
Vocabulary • kinetic energy • kinetic theory • gas pressure
• vacuum • atmospheric pressure • barometer
• pascal (Pa) • standard atmosphere (atm)
Part A Completion Use this completion exercise to check your understanding of the concepts and that are introduced in this section. Each blank can be completed with a term, short phrase, or number. The kinetic theory describes the
1
of particles in matter
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and the forces of attraction between them. The theory assumes 2
that the volume occupied by a gas is mostly particles of gas are relatively and are in constant
5
3
motion. The
6
particles are perfectly elastic so that the total
2.
, that the
4
, move
3.
of each other, between
7
remains
1.
4. 5. 6.
constant. Gas pressure results from the simultaneous collisions
7.
of billions of particles with an object. Barometers are used to
8.
measure
8
pressure. Standard conditions are defined
as a temperature of
9
and a pressure of
10
.
9. 10.
Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. ________ 11. Atmospheric pressure is 760 mm Hg. ________ 12. The SI unit of pressure is the pascal.
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________ 13. Atmospheric pressure increases as you climb a mountain because the density of Earth’s atmosphere decreases with altitude. ________ 14. When particles of a substance are heated, some of the energy is absorbed by the particle and stored in the form of potential energy. ________ 15. The Kelvin temperature of a substance is directly proportional to the total kinetic energy of the particles in the substance. ________ 16. At any given temperature, the particles of all substances have the same average kinetic energy.
Part C Matching Match each description in Column B to the correct term in Column A.
Column A
Column B
________ 17. vacuum
a. an instrument used to measure atmospheric pressure
________ 18. kinetic energy
b. a space where no particles of matter exist
________ 19. gas pressure
c. the energy an object has because of its motion
________ 20. atmospheric pressure
d. results from the force exerted by a gas per unit surface area of an object
________ 21. barometer
e. results from the collisions of atoms and molecules in air with objects
Answer the following in the space provided. 22. A gas is at a pressure of 4.30 atm. What is this pressure in kilopascals? In mm Hg?
23. Describe the motion of particles of a gas according to kinetic theory.
24. What simple evidence demonstrates that gas particles are in constant motion?
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Part D Questions and Problems
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THE NATURE OF LIQUIDS
13.2
Section Review Objectives • • • •
Identify factors that determine physical properties of a liquid Define evaporation in of kinetic energy Describe the equilibrium between a liquid and its vapor Identify the conditions under which boiling occurs
Vocabulary • vaporization • evaporation • vapor pressure
• boiling point • normal boiling point
Part A Completion Use this completion exercise to check your understanding of the concepts and that are introduced in this section. Each blank can be completed with a term, short phrase, or number. 1
Liquids are much
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are known as
2
1.
states of matter. The conversion of a liquid
to a gas or vapor is called 4
than gases. Liquids and solids
3
2.
. When a liquid that is not
3.
changes to a gas, the process is called evaporation. A
4.
liquid evaporates faster when heated; however, evaporation itself 5
is a
5.
process. When a partially filled container of liquid is 6
sealed, some of the particles at the
6.
of the liquid vaporize.
7.
These particles collide with the walls of the container, producing a force called
7
. The vapor pressure of a liquid can be
determined by a device called a 9
8.
8
9.
. A liquid boils when its
10.
equals the external pressure. The normal boiling point of a
liquid is the temperature at which the vapor pressure is equal to
10
.
Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. ________ 11. Particles in a liquid don’t have enough kinetic energy to overcome the attractive forces between them and vaporize. Chapter 13 States of Matter
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________ 12. When a liquid is in a closed container, there are more particles evaporating than condensing. ________ 13. The change of a substance directly from a solid to a gas or vapor is called condensation. ________ 14. The rates of evaporation and condensation are equal at equilibrium. ________ 15. Heating a liquid will increase the temperature of the liquid. ________ 16. During evaporation in an open container, the temperature of a liquid decreases.
Part C Matching Match each description in Column B to the correct term in Column A.
Column A
Column B
________ 17. vapor pressure
a. a measure of the pressure exerted by a gas above a liquid
________ 18. condensation
b. the forces between molecules
________ 19. normal boiling point
c. the boiling point of a liquid at a pressure of 101.3 kPa
________ 20. liquid
d. a fluid with a fixed volume
________ 21. intermolecular attractions
e. the change of a gas or vapor directly to a liquid
Answer the following in the space provided. 22. Describe what happens on a particle level when a liquid is at its boiling point.
23. Liquid A has a vapor pressure of 7.37 kPa at 40°C. Liquid B has a vapor pressure of 18.04 kPa at 40°C. Which liquid would evaporate faster at 40°C? Explain your answer.
24. Explain why evaporation leads to cooling of the liquid.
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Part D Questions and Problems
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THE NATURE OF SOLIDS
13.3
Section Review Objectives • Evaluate how the way particles are organized explains the properties of solids • Identify the factors that determine the shape of a crystal • Explain how allotropes of an element are different
Vocabulary • melting point • crystal • unit cell
• allotropes • amorphous solid • glass
Part A Completion Use this completion exercise to check your understanding of the concepts and that are introduced in this section. Each blank can be completed with a term, short phrase, or number. 1
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Solids tend to be dense and difficult to
. They do not
1.
flow or take the shape of their containers, like liquids do, because
2.
2
the particles in solids vibrate around
points. When a solid
3.
is heated until its particles vibrate so rapidly that they are no longer held in fixed positions, the solid
3
. The
4
is the
temperature at which a solid changes to a liquid. The melting and 5
of a substance are at the same temperature. In general,
ionic solids tend to have relatively
6
4. 5. 6. 7.
melting points, while
8.
molecular solids tend to have relatively low melting points. Most
9.
7
solids are as a crystal is the
9
and are called
. The particles are arranged in a pattern known 8
10.
. The smallest subunit of a crystal lattice
. Some solids lack an ordered internal structure 10
solids.
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Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. ________ 11. Glasses do not melt at a definite temperature, but soften gradually. ________ 12. Solid substances can exist in more than one form. ________ 13. Allotropes are two or more different elements that exist in the same state with the same crystal system. ________ 14. When the atoms in a solid have a random arrangement, the solid is a glass. ________ 15. The type of bonding that exists between the atoms in a crystal tends to determine the melting point of the solid.
Part C Matching Match each description in Column B to the correct term in Column A.
Column A
Column B a. describes a solid in which the particles are randomly arranged
________ 17. unit cell
b. transparent fusion products of inorganic substances that have cooled to a rigid state without crystallizing
________ 18. rhombohedral
c. the smallest group of particles within a crystal that retains the geometric shape of the crystal
________ 19. amorphous
d. the temperature at which a solid changes to a liquid
________ 20. glasses
e. has a regular three-dimensional arrangement of particles
________ 21. solid
f. one of the seven crystal systems.
________ 22. melting point
g. dense state of matter that has a fixed shape and is not easily compressed
Part D Questions and Problems Answer the following in the space provided. 24. Explain what happens at the particle level when a solid melts.
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________ 16. crystal
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CHANGES OF STATE
13.4
Section Review Objectives • Identify the conditions necessary for sublimation • Describe how equilibrium conditions are represented in a phase diagram
Vocabulary • sublimation • triple point • phase diagram
Part A Completion Use this completion exercise to check your understanding of the concepts and that are introduced in this section. Each blank can be completed with a term, short phrase, or number. The change that occurs when a solid goes directly to the gas
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or vapor state without first becoming a liquid is
1
1.
.
2.
This change can occur because solids, like liquids, have a
3.
2
. Substances that sublime include iodine and solid
4.
3
(dry ice).
5.
A graph that shows the relationship between the states of a substance is called a
4
6.
diagram. On this diagram, a line
7.
between two phases shows the conditions at which the phases
8.
are in
5
. The
6
is the only set of conditions at
which solid, liquid, and gas phases coexist. The triple point for water is a temperature of
7
and a pressure of
8
.
Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. ________ 9. A phase diagram gives information on changes in mass of solids, liquids, and gases. ________ 10. Water could be made to boil at 105°C by increasing the pressure. Chapter 13 States of Matter
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________ 11. The sublimation point of a substance refers to the temperature and pressure at which the substance exists in all three phases of matter. ________ 12. Below the triple point for water, decreasing the pressure will not change water vapor to ice. ________ 13. Water has more than one triple point. ________ 14. At 101.3 kPa, the normal boiling point and melting point of water are the same.
Part C Matching Match each description in Column B to the correct term in Column A.
Column A
Column B a. the change of a solid to a vapor without ing through the liquid state
________ 16. freeze drying
b. the change of a solid to the liquid state
________ 17. phase diagram
c. a method of removing water from food, using sublimation
________ 18. 0.016°C, 0.61 kPa
d. graph that shows the relationship among the states of a substance
________ 19. sublimation
e. defines the triple point for water
________ 20. 100°C at 101.3 kPa
f. normal boiling point for water
Part D Questions and Problems Answer the following in the space provided. 21. Explain how some solids can vaporize and then condense back to a solid without ing through the liquid state. What is the process called?
22. When the physical state of a substance changes during a phase change, what happens to the temperature of the system?
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________ 15. melting
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STATES OF MATTER
Practice Problems In your notebook, answer the following questions or solve the following problems.
SECTION 13.1 THE NATURE OF GASES 1. Explain why there is no gas pressure inside a vacuum. 2. How would the reading on a barometer change if you were to take one on a trip from Los Angeles to Lake Tahoe, which is at a much higher altitude? 3. The height of a column of mercury in a barometer is 754.3 mm. What is the atmospheric pressure in atm? In kPa? 4. How does the average kinetic energy of the helium atoms in a balloon change as the helium gas is heated from 100.0C to 73C?
SECTION 13.2 THE NATURE OF LIQUIDS 1. In general, how do the intermolecular attractions between particles in a gas compare with those between particles in a liquid?
3. Explain how the following description is an analogy for evaporative cooling: If the fastest runner is removed from a race, the average speed of the remaining runners will be lower. 4. The normal boiling point of ethanol is 78.5°C. The normal boiling point of water is 100°C. At 75°C, which liquid, ethanol or water, has the greater vapor pressure? Explain.
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2. An open beaker is about half filled with water. How can a dynamic equilibrium be established between the water and the vapor forming above its surface?
1. How does the crystalline structure of graphite compare with that of diamond? 2. Why is diamond classified as an allotrope of carbon? 3. Peanut brittle is a candy that is poured out while hot onto a surface. It is allowed to cool and harden into a sheet, which easily breaks into irregularly shaped pieces. The sugar in peanut brittle solidifies without reforming its crystal lattice. What type of solid is peanut brittle? 4. Which type of solid is likely to have the lowest melting point—an ionic solid or a molecular solid? Explain. 5. Give an example of a crystalline solid. What is a crystal?
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SECTION 13.4 CHANGES OF STATE To answer the following questions, refer to the phase diagram shown in Figure 13.15 of your textbook. 1. How does the melting point of water change as the pressure increases? 2. What does the line separating the solid phase from the vapor phase represent? 3. What does the line separating the liquid phase from the vapor phase represent? 4. What is the vapor pressure of liquid water at 100C?
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INTERPRETING GRAPHICS Use with Section 13.4
100
80
Pressure (kPa)
60
40
20
0 30
10
0
20
40
60
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Temperature (°C) Figure 1 Phase diagram for bromine (Br2). Note that the scale on the x-axis is distorted to emphasize some of the graph’s features. At standard temperature and pressure, bromine is a red liquid. Bromine sublimes when the temperature is 25C and the pressure is 101.3 kPa. 1. Label each region of the graph as solid, liquid, or vapor. 2. Label the triple point, normal melting point, and normal boiling point on the graph and estimate their temperature values. Include an estimate of the pressure for the triple point. Normal melting point Normal boiling point Triple point 3. Use the letter A to label the line that gives the conditions for equilibrium between solid and liquid phases of bromine, the letter B to label the curve that gives the conditions for equilibrium between liquid and vapor phases of bromine, and the letter C to label the curve that gives the conditions for equilibrium between solid and vapor phases of bromine.
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4. Describe how the melting point of bromine changes with the external pressure. Based on the slope of the melting-point curve in the phase diagram, would you characterize the solid phase of bromine as more dense or less dense than the liquid phase of bromine?
5. What is the boiling point of bromine when the external pressure is 75 kPa?
6. Explain the significance of the triple point.
7. Place direction arrows labeled S, V, and M on the phase diagram to indicate where sublimation, vaporization, and melting occur, respectively. Circle the correct word in the parentheses in each of the following sentences. 8. Bromine vapor at 15°C (condenses, sublimes) when the pressure is raised to 50 kPa.
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9. Bromine liquid at 70 kPa (vaporizes, freezes) when the temperature is decreased to 15°C.
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STATES OF MATTER
Vocabulary Review Each clue describes a vocabulary term. Read the clues and write the letters of each term on the lines. 1. Clue: the energy an object has because of its motion. ____ ____ ____ ____ ____ ____ ____
____ ____ ____ ____ ____ ____
2. Clue: results from the force exerted by a gas per unit surface area of an object. ____ ____ ____ ____ ____ ____ ____ ____ ____ ____ ____ 3. Clue: the process in which molecules of a liquid escape from the surface of a liquid that is not boiling. ____ ____ ____ ____ ____ ____ ____ ____ ____ ____ ____ 4. Clue: the temperature at which the vapor pressure of a liquid is just equal to the external pressure. ____ ____ ____ ____ ____ ____ ____ 5. Clue: sample in which particles are arranged in an orderly, repeating, three-dimensional pattern. ____ ____ ____ ____ ____ ____ ____ 6. Clue: two or more different molecular forms of the same element in the same physical state. ____ ____ ____ ____ ____ ____ ____ ____ ____ ____ 7. Clue: the temperature at which a solid changes into a liquid. ____ ____ ____ ____ ____ ____ ____
____ ____ ____ ____ ____
8. Clue: the SI unit of pressure. ____ ____ ____ ____ ____ ____
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Write the letters found inside the circles on the lines below. Then unscramble them to find the name of a device for measuring the atmospheric pressure. Scrambled Letters: ____ ____ ____ ____ ____ ____ ____ ____ ____ Solution: ____ ____ ____ ____ ____ ____ ____ ____ ____
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STATES OF MATTER
Chapter Quiz Fill in the word(s) that will make each statement true. 13.1
with an increase in elevation.
2.
13.1
3 3. An increase in the of a substance corresponds to an increase in the average kinetic energy of its particles.
3.
13.1
4.
13.1
5.
13.1
6.
13.2
7. During evaporation, only those molecules that possess a 7 certain can escape from the surface of a liquid.
7.
13.2
8. At the boiling point, the vapor pressure of a liquid is equal to 8 the .
8.
13.2
9. The smallest group of particles in a crystal that retains the 9 shape of a crystal is a(n) .
9.
13.3
10.
13.3
2. Atmospheric pressure
2
4. The energy an object has because of its motion is energy.
4
5. In the kinetic theory, it is assumed that the collisions between 5 gas particles are perfectly . 6. Liquids and solids are known as
6
states of matter.
10. A solid that lacks an ordered internal structure is a(n) 10 solid.
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. ________ 11. The change of a substance to vapor is called vaporization.
13.3, 13.4
________ 12. At the triple point, solid, liquid, and gas can exist in equilibrium with one another.
13.4
________ 13. A phase diagram shows the temperature and pressure conditions at which a substance exists as a solid, liquid, and gas or vapor.
13.4
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1.
1 1. The theory states that the tiny particles in matter are in constant motion.
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STATES OF MATTER
Chapter Test A A. Matching Match each description in Column B with the correct term in Column A. Write the letter of the correct description on the line.
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Column A
Column B
________ 1. amorphous
a. an empty space with no particles of matter
________ 2. unit cell
b. the temperature at which a solid changes into a liquid
________ 3. crystal
c. a device used to measure atmospheric pressure
________ 4. normal boiling point
d. the pressure resulting from the collision of particles in air with objects
________ 5. barometer
e. the temperature at which the vapor pressure of a liquid is equal to the external pressure
________ 6. atmospheric pressure
f. the smallest group of particles within a crystal that retains the shape of the crystal
________ 7. melting point
g. a solid in which the particles are arranged in an orderly, repeating, three-dimensional pattern
________ 8. sublimation
h. a measure of the force exerted by a gas above a liquid
________ 9. boiling point
i. describes a solid that lacks an ordered internal structure
________ 10. kinetic theory
j. the temperature at which a liquid boils at a pressure of 101.3 kPa
________ 11. allotrope
k. one of two or more different molecular forms of the same element in the same physical state
________ 12. vapor pressure
l. the conversion of a liquid to a gas or vapor at a temperature below the boiling point
________ 13. evaporation
________ 14. vacuum
m. states that the tiny particles in all forms of matter are in constant motion n. the change of a solid to a vapor without ing through the liquid state
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B. Multiple Choice Choose the best answer and write its letter on the line. ________ 15. The average kinetic energy of water molecules is greatest in a. steam at 200C. c. liquid water at 373 K. b. liquid water at 90C. d. ice at 0C. ________ 16. According to the kinetic theory of gases, a. the particles in a gas move rapidly. b. the particles in a gas are relatively far apart. c. the particles in a gas move independently of each other. d. all of the above are true. ________ 17. The temperature at which the motion of particles theoretically ceases is a. 0C. c. 273 K. b. 273C. d. 0 K. ________ 18. The average kinetic energy of particles of a substance a. is not affected by the temperature of the substance. b. increases as the temperature of the substance decreases. c. is directly proportional to the temperature of a substance. d. is equal to 0. ________ 19. Which of these statements is not true, according to kinetic theory? a. There is no 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. All collisions between particles of gas are perfectly elastic.
________ 21. The pressure of a gas in a container is 76 mm Hg. This is equivalent to a. 0.1 atm. c. 0.2 atm. b. 1 atm. d. 0.76 atm. ________ 22. A phase diagram gives information on a. volumes of gases. b. conditions at which a substance exists as a solid, liquid, and gas. c. volumes of liquids and solids. d. changes in mass of solids, liquids, and gases. ________ 23. An increase in the temperature of a contained liquid a. causes the vapor pressure above the liquid to increase. b. decreases the vapor pressure above a liquid. c. causes fewer particles to escape the surface of the liquid. d. has no effect on the kinetic energy of the liquid.
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________ 20. Standard conditions when working with gases are defined as a. 0 K and 101.3 kilopascals. c. 0C and 101.3 kilopascals. b. 0 K and 1 mm Hg. d. 0C and 1 mm Hg.
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________ 24. Water could be made to boil at 105C by a. applying a great deal of energy. b. increasing the air pressure above the water. c. heating the water more gradually. d. decreasing the air pressure above the water. ________ 25. The direct change of a substance from a solid to a vapor is called: a. evaporation c. condensation. b. sublimation. d. vaporization. ________ 26. Most solids a. are amorphous. b. lack an orderly internal structure. c. are dense and not easily compressed. d. have low melting points. ________ 27. The escape of molecules from the surface of an uncontained liquid is a. boiling. c. evaporation. b. sublimation. d. condensation.
C. True-False Classify each of these statements as always true, AT, sometimes true, ST, or never true, NT. ________ 28. The rates of evaporation and condensation are equal at equilibrium.
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________ 29. The kinetic energy of all the particles in a given sample of matter is the same. ________ 30. The average kinetic energy of all the molecules in liquid water at 80C is the same as the average kinetic energy of the molecules in oxygen gas at 80C. ________ 31. Heating a liquid will increase the temperature of the liquid. ________ 32. The melting point and freezing point of a substance are the same.
D. Problems Solve the following problems in the space provided. Show your work. 33. A gas is at a pressure of 3.70 atm. What is this pressure in kilopascals?
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34. What is the pressure of the gas in problem 33, expressed in millimeters of mercury?
E. Essay Write a short essay for the following. 35. Explain why the temperature of a gas does not depend on the number of particles in the sample of gas.
F. Additional Problems Solve the following problems in the space provided. Show your work. 36. A gas has a pressure of 610.0 mm Hg. What is the pressure in atmospheres?
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37. What is the pressure of the gas in problem 36, expressed in kilopascals?
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G. Additional Questions Answer the following questions in the space provided. 38. A 100-g sample of water is heated from 50C to 100C. At 100C, although the water is still being heated, the temperature of the water does not rise. Explain why.
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39. Some types of bacteria are killed by being heated to a temperature of 150C for 30 minutes. Explain why water heated under pressure can be used to kill these bacteria, although boiling water at atmospheric pressure does not kill them.
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STATES OF MATTER
Chapter Test B A. Matching Match each term in Column B to the correct description in Column A. Write the letter of the correct term on the line.
Column A
Column B a. normal boiling point
________ 2. a measure of the force exerted by a gas above a liquid
b. pascal
________ 3. The tiny particles in all forms of matter are in constant motion.
c. kinetic energy
________ 4. the temperature at which a solid changes into a liquid
d. standard atmosphere
________ 5. the pressure required to 760 mm of Hg at 25C
e. melting point
________ 6. the change of a substance from a solid to a gas or vapor without ing through the liquid state
f. triple point
________ 7. the SI unit of pressure
g. evaporation
________ 8. the conversion of a liquid to a gas or vapor at a temperature below the liquid’s boiling point
h. kinetic theory
________ 9. describes the only conditions of temperature and pressure at which all three phases of a substance can exist in equilibrium
i. allotropes
________ 10. the pressure that results from the collisions of particles in air with objects
j. barometer
________ 11. the temperature at which a liquid boils at a pressure of 101.3 kPa
k. sublimation
________ 12. the smallest group of particles within a crystal that retains the geometric shape of the crystal
l. atmospheric pressure
________ 13. the energy an object has because of its motion ________ 14. two or more different molecular forms of the same element in the same physical state
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m. unit cell n. vapor pressure
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________ 1. an instrument used to measure atmospheric pressure
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Date ___________________
Class __________________
B. Multiple Choice Choose the best answer and write its letter on the line. ________ 15. According to the kinetic theory, gases consist of particles that a. occupy considerable volume. b. are relatively close together. c. exert attractive and repulsive forces on other particles. d. have motion that is constant, random, and rapid. ________ 16. As you climb a mountain, atmospheric pressure: a. increases. c. remains the same. b. decreases. d. varies randomly. ________ 17. Which of the following is true about atmospheric pressure? a. It is measured with a hydrometer. b. It varies widely, depending on the weather. c. It increases with altitude. d. It affects the boiling point of a liquid.
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________ 18. At sea level in fair weather, atmospheric pressure is equal to a. 101.3 kPa. c. 760 mm Hg. b. 1 standard atmosphere. d. all of the above ________ 19. STP refers to: a. 100C and 1 atm. b. 0C and 1 kPa.
c. 0C and 1 atm. d. 100C and 760 mm Hg.
________ 20. A pressure of 2.5 atm is equivalent to a. 41 kPa. b. 1900 mm Hg.
c. 3.0 102 mm Hg. d. 2.5 kPa.
________ 21. Absolute zero is a. the temperature at which the motion of particles theoretically ceases. b. defined as 0C. c. the triple point for water. d. all of the above ________ 22. At 80 K, the particles of a gas have a. twice the average kinetic energy of the same particles at 40 K. b. half the average kinetic energy of the same particles at 40 K. c. one fourth the average kinetic energy of the same particles at 20 K. d. none of the above ________ 23. Compared with gases, liquids: a. have stronger intermolecular attractions. b. have more space between their particles. c. are much less dense. d. are more easily compressed.
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________ 24. Evaporation is a type of a. boiling. b. vaporization.
Class __________________
c. sublimation. d. condensation.
________ 25. A decrease in the temperature of a contained liquid causes a. an increase in the vapor pressure. b. a decrease in the vapor pressure. c. more particles to evaporate. d. an increase in the average kinetic energy of the particles. ________ 26. Water could be made to boil at 92C by a. lowering the external air pressure. b. raising the external air pressure. c. increasing the pressure on the water. d. none of the above ________ 27. In comparison with liquids and gases, solids are a. more dense. c. less organized. b. more easily compressed. d. more likely to flow. ________ 28. Diamond and graphite are examples of a. phases. c. allotropes. b. amorphous solids. d. glasses. ________ 29. The conditions at which the solid, liquid, and gaseous phases of a substance can exist in equilibrium with one another is called a. boiling point. c. sublimation point. b. freezing point. d. triple point.
C. True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. ________ 31. In an elastic collision, kinetic energy is transferred from one particle to another, but the total kinetic energy remains constant. ________ 32. Atmospheric pressure is 101.3 kPa. ________ 33. The Kelvin temperature of a substance is directly proportional to the average kinetic energy of the particles in that substance. ________ 34. At any given temperature, the particles of all substances have the same average kinetic energy. ________ 35. The temperature of a boiling liquid can rise above its boiling point. ________ 36. Water boils at 100C. ________ 37. The melting and freezing points of a substance are the same temperature.
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________ 30. Sublimation can occur because solids have a. a melting point. c. a boiling point. b. a vapor pressure. d. a triple point.
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D. Essay Write a short essay for the following. 38. Distinguish between the boiling point and the normal boiling point of a liquid. Explain the impact of a change in atmospheric pressure on the relationship between the boiling point and the normal boiling point.
E. Additional Questions Answer the following questions in the space provided.
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39. Distinguish between gases, liquids, and solids in of the kinetic theory.
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40. Explain why each of the following is true. a. The temperature of a boiling liquid never rises above its boiling point.
b. The temperature of an ice and water mixture at 1 standard atmosphere remains at 0C as long as both ice and liquid water are present, no matter what the surrounding temperature.
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THE NATURE OF GASES
13.1
Section Review Objectives • Describe the assumptions of the kinetic theory as it applies to gases • Interpret gas pressure in of kinetic theory • Define the relationship between Kelvin temperature and average kinetic energy
Vocabulary • kinetic energy • kinetic theory • gas pressure
• vacuum • atmospheric pressure • barometer
• pascal (Pa) • standard atmosphere (atm)
Part A Completion Use this completion exercise to check your understanding of the concepts and that are introduced in this section. Each blank can be completed with a term, short phrase, or number. The kinetic theory describes the
1
of particles in matter
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and the forces of attraction between them. The theory assumes 2
that the volume occupied by a gas is mostly particles of gas are relatively and are in constant
5
3
motion. The
6
particles are perfectly elastic so that the total
2.
, that the
4
, move
3.
of each other, between
7
remains
1.
4. 5. 6.
constant. Gas pressure results from the simultaneous collisions
7.
of billions of particles with an object. Barometers are used to
8.
measure
8
pressure. Standard conditions are defined
as a temperature of
9
and a pressure of
10
.
9. 10.
Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. ________ 11. Atmospheric pressure is 760 mm Hg. ________ 12. The SI unit of pressure is the pascal.
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________ 13. Atmospheric pressure increases as you climb a mountain because the density of Earth’s atmosphere decreases with altitude. ________ 14. When particles of a substance are heated, some of the energy is absorbed by the particle and stored in the form of potential energy. ________ 15. The Kelvin temperature of a substance is directly proportional to the total kinetic energy of the particles in the substance. ________ 16. At any given temperature, the particles of all substances have the same average kinetic energy.
Part C Matching Match each description in Column B to the correct term in Column A.
Column A
Column B
________ 17. vacuum
a. an instrument used to measure atmospheric pressure
________ 18. kinetic energy
b. a space where no particles of matter exist
________ 19. gas pressure
c. the energy an object has because of its motion
________ 20. atmospheric pressure
d. results from the force exerted by a gas per unit surface area of an object
________ 21. barometer
e. results from the collisions of atoms and molecules in air with objects
Answer the following in the space provided. 22. A gas is at a pressure of 4.30 atm. What is this pressure in kilopascals? In mm Hg?
23. Describe the motion of particles of a gas according to kinetic theory.
24. What simple evidence demonstrates that gas particles are in constant motion?
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Part D Questions and Problems
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THE NATURE OF LIQUIDS
13.2
Section Review Objectives • • • •
Identify factors that determine physical properties of a liquid Define evaporation in of kinetic energy Describe the equilibrium between a liquid and its vapor Identify the conditions under which boiling occurs
Vocabulary • vaporization • evaporation • vapor pressure
• boiling point • normal boiling point
Part A Completion Use this completion exercise to check your understanding of the concepts and that are introduced in this section. Each blank can be completed with a term, short phrase, or number. 1
Liquids are much
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are known as
2
1.
states of matter. The conversion of a liquid
to a gas or vapor is called 4
than gases. Liquids and solids
3
2.
. When a liquid that is not
3.
changes to a gas, the process is called evaporation. A
4.
liquid evaporates faster when heated; however, evaporation itself 5
is a
5.
process. When a partially filled container of liquid is 6
sealed, some of the particles at the
6.
of the liquid vaporize.
7.
These particles collide with the walls of the container, producing a force called
7
. The vapor pressure of a liquid can be
determined by a device called a 9
8.
8
9.
. A liquid boils when its
10.
equals the external pressure. The normal boiling point of a
liquid is the temperature at which the vapor pressure is equal to
10
.
Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. ________ 11. Particles in a liquid don’t have enough kinetic energy to overcome the attractive forces between them and vaporize. Chapter 13 States of Matter
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________ 12. When a liquid is in a closed container, there are more particles evaporating than condensing. ________ 13. The change of a substance directly from a solid to a gas or vapor is called condensation. ________ 14. The rates of evaporation and condensation are equal at equilibrium. ________ 15. Heating a liquid will increase the temperature of the liquid. ________ 16. During evaporation in an open container, the temperature of a liquid decreases.
Part C Matching Match each description in Column B to the correct term in Column A.
Column A
Column B
________ 17. vapor pressure
a. a measure of the pressure exerted by a gas above a liquid
________ 18. condensation
b. the forces between molecules
________ 19. normal boiling point
c. the boiling point of a liquid at a pressure of 101.3 kPa
________ 20. liquid
d. a fluid with a fixed volume
________ 21. intermolecular attractions
e. the change of a gas or vapor directly to a liquid
Answer the following in the space provided. 22. Describe what happens on a particle level when a liquid is at its boiling point.
23. Liquid A has a vapor pressure of 7.37 kPa at 40°C. Liquid B has a vapor pressure of 18.04 kPa at 40°C. Which liquid would evaporate faster at 40°C? Explain your answer.
24. Explain why evaporation leads to cooling of the liquid.
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Part D Questions and Problems
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THE NATURE OF SOLIDS
13.3
Section Review Objectives • Evaluate how the way particles are organized explains the properties of solids • Identify the factors that determine the shape of a crystal • Explain how allotropes of an element are different
Vocabulary • melting point • crystal • unit cell
• allotropes • amorphous solid • glass
Part A Completion Use this completion exercise to check your understanding of the concepts and that are introduced in this section. Each blank can be completed with a term, short phrase, or number. 1
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Solids tend to be dense and difficult to
. They do not
1.
flow or take the shape of their containers, like liquids do, because
2.
2
the particles in solids vibrate around
points. When a solid
3.
is heated until its particles vibrate so rapidly that they are no longer held in fixed positions, the solid
3
. The
4
is the
temperature at which a solid changes to a liquid. The melting and 5
of a substance are at the same temperature. In general,
ionic solids tend to have relatively
6
4. 5. 6. 7.
melting points, while
8.
molecular solids tend to have relatively low melting points. Most
9.
7
solids are as a crystal is the
9
and are called
. The particles are arranged in a pattern known 8
10.
. The smallest subunit of a crystal lattice
. Some solids lack an ordered internal structure 10
solids.
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Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. ________ 11. Glasses do not melt at a definite temperature, but soften gradually. ________ 12. Solid substances can exist in more than one form. ________ 13. Allotropes are two or more different elements that exist in the same state with the same crystal system. ________ 14. When the atoms in a solid have a random arrangement, the solid is a glass. ________ 15. The type of bonding that exists between the atoms in a crystal tends to determine the melting point of the solid.
Part C Matching Match each description in Column B to the correct term in Column A.
Column A
Column B a. describes a solid in which the particles are randomly arranged
________ 17. unit cell
b. transparent fusion products of inorganic substances that have cooled to a rigid state without crystallizing
________ 18. rhombohedral
c. the smallest group of particles within a crystal that retains the geometric shape of the crystal
________ 19. amorphous
d. the temperature at which a solid changes to a liquid
________ 20. glasses
e. has a regular three-dimensional arrangement of particles
________ 21. solid
f. one of the seven crystal systems.
________ 22. melting point
g. dense state of matter that has a fixed shape and is not easily compressed
Part D Questions and Problems Answer the following in the space provided. 24. Explain what happens at the particle level when a solid melts.
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________ 16. crystal
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CHANGES OF STATE
13.4
Section Review Objectives • Identify the conditions necessary for sublimation • Describe how equilibrium conditions are represented in a phase diagram
Vocabulary • sublimation • triple point • phase diagram
Part A Completion Use this completion exercise to check your understanding of the concepts and that are introduced in this section. Each blank can be completed with a term, short phrase, or number. The change that occurs when a solid goes directly to the gas
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or vapor state without first becoming a liquid is
1
1.
.
2.
This change can occur because solids, like liquids, have a
3.
2
. Substances that sublime include iodine and solid
4.
3
(dry ice).
5.
A graph that shows the relationship between the states of a substance is called a
4
6.
diagram. On this diagram, a line
7.
between two phases shows the conditions at which the phases
8.
are in
5
. The
6
is the only set of conditions at
which solid, liquid, and gas phases coexist. The triple point for water is a temperature of
7
and a pressure of
8
.
Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. ________ 9. A phase diagram gives information on changes in mass of solids, liquids, and gases. ________ 10. Water could be made to boil at 105°C by increasing the pressure. Chapter 13 States of Matter
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________ 11. The sublimation point of a substance refers to the temperature and pressure at which the substance exists in all three phases of matter. ________ 12. Below the triple point for water, decreasing the pressure will not change water vapor to ice. ________ 13. Water has more than one triple point. ________ 14. At 101.3 kPa, the normal boiling point and melting point of water are the same.
Part C Matching Match each description in Column B to the correct term in Column A.
Column A
Column B a. the change of a solid to a vapor without ing through the liquid state
________ 16. freeze drying
b. the change of a solid to the liquid state
________ 17. phase diagram
c. a method of removing water from food, using sublimation
________ 18. 0.016°C, 0.61 kPa
d. graph that shows the relationship among the states of a substance
________ 19. sublimation
e. defines the triple point for water
________ 20. 100°C at 101.3 kPa
f. normal boiling point for water
Part D Questions and Problems Answer the following in the space provided. 21. Explain how some solids can vaporize and then condense back to a solid without ing through the liquid state. What is the process called?
22. When the physical state of a substance changes during a phase change, what happens to the temperature of the system?
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________ 15. melting
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Date ___________________
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STATES OF MATTER
Practice Problems In your notebook, answer the following questions or solve the following problems.
SECTION 13.1 THE NATURE OF GASES 1. Explain why there is no gas pressure inside a vacuum. 2. How would the reading on a barometer change if you were to take one on a trip from Los Angeles to Lake Tahoe, which is at a much higher altitude? 3. The height of a column of mercury in a barometer is 754.3 mm. What is the atmospheric pressure in atm? In kPa? 4. How does the average kinetic energy of the helium atoms in a balloon change as the helium gas is heated from 100.0C to 73C?
SECTION 13.2 THE NATURE OF LIQUIDS 1. In general, how do the intermolecular attractions between particles in a gas compare with those between particles in a liquid?
3. Explain how the following description is an analogy for evaporative cooling: If the fastest runner is removed from a race, the average speed of the remaining runners will be lower. 4. The normal boiling point of ethanol is 78.5°C. The normal boiling point of water is 100°C. At 75°C, which liquid, ethanol or water, has the greater vapor pressure? Explain.
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2. An open beaker is about half filled with water. How can a dynamic equilibrium be established between the water and the vapor forming above its surface?
1. How does the crystalline structure of graphite compare with that of diamond? 2. Why is diamond classified as an allotrope of carbon? 3. Peanut brittle is a candy that is poured out while hot onto a surface. It is allowed to cool and harden into a sheet, which easily breaks into irregularly shaped pieces. The sugar in peanut brittle solidifies without reforming its crystal lattice. What type of solid is peanut brittle? 4. Which type of solid is likely to have the lowest melting point—an ionic solid or a molecular solid? Explain. 5. Give an example of a crystalline solid. What is a crystal?
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SECTION 13.4 CHANGES OF STATE To answer the following questions, refer to the phase diagram shown in Figure 13.15 of your textbook. 1. How does the melting point of water change as the pressure increases? 2. What does the line separating the solid phase from the vapor phase represent? 3. What does the line separating the liquid phase from the vapor phase represent? 4. What is the vapor pressure of liquid water at 100C?
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INTERPRETING GRAPHICS Use with Section 13.4
100
80
Pressure (kPa)
60
40
20
0 30
10
0
20
40
60
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Temperature (°C) Figure 1 Phase diagram for bromine (Br2). Note that the scale on the x-axis is distorted to emphasize some of the graph’s features. At standard temperature and pressure, bromine is a red liquid. Bromine sublimes when the temperature is 25C and the pressure is 101.3 kPa. 1. Label each region of the graph as solid, liquid, or vapor. 2. Label the triple point, normal melting point, and normal boiling point on the graph and estimate their temperature values. Include an estimate of the pressure for the triple point. Normal melting point Normal boiling point Triple point 3. Use the letter A to label the line that gives the conditions for equilibrium between solid and liquid phases of bromine, the letter B to label the curve that gives the conditions for equilibrium between liquid and vapor phases of bromine, and the letter C to label the curve that gives the conditions for equilibrium between solid and vapor phases of bromine.
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4. Describe how the melting point of bromine changes with the external pressure. Based on the slope of the melting-point curve in the phase diagram, would you characterize the solid phase of bromine as more dense or less dense than the liquid phase of bromine?
5. What is the boiling point of bromine when the external pressure is 75 kPa?
6. Explain the significance of the triple point.
7. Place direction arrows labeled S, V, and M on the phase diagram to indicate where sublimation, vaporization, and melting occur, respectively. Circle the correct word in the parentheses in each of the following sentences. 8. Bromine vapor at 15°C (condenses, sublimes) when the pressure is raised to 50 kPa.
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9. Bromine liquid at 70 kPa (vaporizes, freezes) when the temperature is decreased to 15°C.
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STATES OF MATTER
Vocabulary Review Each clue describes a vocabulary term. Read the clues and write the letters of each term on the lines. 1. Clue: the energy an object has because of its motion. ____ ____ ____ ____ ____ ____ ____
____ ____ ____ ____ ____ ____
2. Clue: results from the force exerted by a gas per unit surface area of an object. ____ ____ ____ ____ ____ ____ ____ ____ ____ ____ ____ 3. Clue: the process in which molecules of a liquid escape from the surface of a liquid that is not boiling. ____ ____ ____ ____ ____ ____ ____ ____ ____ ____ ____ 4. Clue: the temperature at which the vapor pressure of a liquid is just equal to the external pressure. ____ ____ ____ ____ ____ ____ ____ 5. Clue: sample in which particles are arranged in an orderly, repeating, three-dimensional pattern. ____ ____ ____ ____ ____ ____ ____ 6. Clue: two or more different molecular forms of the same element in the same physical state. ____ ____ ____ ____ ____ ____ ____ ____ ____ ____ 7. Clue: the temperature at which a solid changes into a liquid. ____ ____ ____ ____ ____ ____ ____
____ ____ ____ ____ ____
8. Clue: the SI unit of pressure. ____ ____ ____ ____ ____ ____
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Write the letters found inside the circles on the lines below. Then unscramble them to find the name of a device for measuring the atmospheric pressure. Scrambled Letters: ____ ____ ____ ____ ____ ____ ____ ____ ____ Solution: ____ ____ ____ ____ ____ ____ ____ ____ ____
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STATES OF MATTER
Chapter Quiz Fill in the word(s) that will make each statement true. 13.1
with an increase in elevation.
2.
13.1
3 3. An increase in the of a substance corresponds to an increase in the average kinetic energy of its particles.
3.
13.1
4.
13.1
5.
13.1
6.
13.2
7. During evaporation, only those molecules that possess a 7 certain can escape from the surface of a liquid.
7.
13.2
8. At the boiling point, the vapor pressure of a liquid is equal to 8 the .
8.
13.2
9. The smallest group of particles in a crystal that retains the 9 shape of a crystal is a(n) .
9.
13.3
10.
13.3
2. Atmospheric pressure
2
4. The energy an object has because of its motion is energy.
4
5. In the kinetic theory, it is assumed that the collisions between 5 gas particles are perfectly . 6. Liquids and solids are known as
6
states of matter.
10. A solid that lacks an ordered internal structure is a(n) 10 solid.
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. ________ 11. The change of a substance to vapor is called vaporization.
13.3, 13.4
________ 12. At the triple point, solid, liquid, and gas can exist in equilibrium with one another.
13.4
________ 13. A phase diagram shows the temperature and pressure conditions at which a substance exists as a solid, liquid, and gas or vapor.
13.4
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1.
1 1. The theory states that the tiny particles in matter are in constant motion.
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STATES OF MATTER
Chapter Test A A. Matching Match each description in Column B with the correct term in Column A. Write the letter of the correct description on the line.
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Column A
Column B
________ 1. amorphous
a. an empty space with no particles of matter
________ 2. unit cell
b. the temperature at which a solid changes into a liquid
________ 3. crystal
c. a device used to measure atmospheric pressure
________ 4. normal boiling point
d. the pressure resulting from the collision of particles in air with objects
________ 5. barometer
e. the temperature at which the vapor pressure of a liquid is equal to the external pressure
________ 6. atmospheric pressure
f. the smallest group of particles within a crystal that retains the shape of the crystal
________ 7. melting point
g. a solid in which the particles are arranged in an orderly, repeating, three-dimensional pattern
________ 8. sublimation
h. a measure of the force exerted by a gas above a liquid
________ 9. boiling point
i. describes a solid that lacks an ordered internal structure
________ 10. kinetic theory
j. the temperature at which a liquid boils at a pressure of 101.3 kPa
________ 11. allotrope
k. one of two or more different molecular forms of the same element in the same physical state
________ 12. vapor pressure
l. the conversion of a liquid to a gas or vapor at a temperature below the boiling point
________ 13. evaporation
________ 14. vacuum
m. states that the tiny particles in all forms of matter are in constant motion n. the change of a solid to a vapor without ing through the liquid state
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B. Multiple Choice Choose the best answer and write its letter on the line. ________ 15. The average kinetic energy of water molecules is greatest in a. steam at 200C. c. liquid water at 373 K. b. liquid water at 90C. d. ice at 0C. ________ 16. According to the kinetic theory of gases, a. the particles in a gas move rapidly. b. the particles in a gas are relatively far apart. c. the particles in a gas move independently of each other. d. all of the above are true. ________ 17. The temperature at which the motion of particles theoretically ceases is a. 0C. c. 273 K. b. 273C. d. 0 K. ________ 18. The average kinetic energy of particles of a substance a. is not affected by the temperature of the substance. b. increases as the temperature of the substance decreases. c. is directly proportional to the temperature of a substance. d. is equal to 0. ________ 19. Which of these statements is not true, according to kinetic theory? a. There is no 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. All collisions between particles of gas are perfectly elastic.
________ 21. The pressure of a gas in a container is 76 mm Hg. This is equivalent to a. 0.1 atm. c. 0.2 atm. b. 1 atm. d. 0.76 atm. ________ 22. A phase diagram gives information on a. volumes of gases. b. conditions at which a substance exists as a solid, liquid, and gas. c. volumes of liquids and solids. d. changes in mass of solids, liquids, and gases. ________ 23. An increase in the temperature of a contained liquid a. causes the vapor pressure above the liquid to increase. b. decreases the vapor pressure above a liquid. c. causes fewer particles to escape the surface of the liquid. d. has no effect on the kinetic energy of the liquid.
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________ 20. Standard conditions when working with gases are defined as a. 0 K and 101.3 kilopascals. c. 0C and 101.3 kilopascals. b. 0 K and 1 mm Hg. d. 0C and 1 mm Hg.
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________ 24. Water could be made to boil at 105C by a. applying a great deal of energy. b. increasing the air pressure above the water. c. heating the water more gradually. d. decreasing the air pressure above the water. ________ 25. The direct change of a substance from a solid to a vapor is called: a. evaporation c. condensation. b. sublimation. d. vaporization. ________ 26. Most solids a. are amorphous. b. lack an orderly internal structure. c. are dense and not easily compressed. d. have low melting points. ________ 27. The escape of molecules from the surface of an uncontained liquid is a. boiling. c. evaporation. b. sublimation. d. condensation.
C. True-False Classify each of these statements as always true, AT, sometimes true, ST, or never true, NT. ________ 28. The rates of evaporation and condensation are equal at equilibrium.
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________ 29. The kinetic energy of all the particles in a given sample of matter is the same. ________ 30. The average kinetic energy of all the molecules in liquid water at 80C is the same as the average kinetic energy of the molecules in oxygen gas at 80C. ________ 31. Heating a liquid will increase the temperature of the liquid. ________ 32. The melting point and freezing point of a substance are the same.
D. Problems Solve the following problems in the space provided. Show your work. 33. A gas is at a pressure of 3.70 atm. What is this pressure in kilopascals?
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Date ___________________
Class __________________
34. What is the pressure of the gas in problem 33, expressed in millimeters of mercury?
E. Essay Write a short essay for the following. 35. Explain why the temperature of a gas does not depend on the number of particles in the sample of gas.
F. Additional Problems Solve the following problems in the space provided. Show your work. 36. A gas has a pressure of 610.0 mm Hg. What is the pressure in atmospheres?
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37. What is the pressure of the gas in problem 36, expressed in kilopascals?
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Date ___________________
Class __________________
G. Additional Questions Answer the following questions in the space provided. 38. A 100-g sample of water is heated from 50C to 100C. At 100C, although the water is still being heated, the temperature of the water does not rise. Explain why.
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39. Some types of bacteria are killed by being heated to a temperature of 150C for 30 minutes. Explain why water heated under pressure can be used to kill these bacteria, although boiling water at atmospheric pressure does not kill them.
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Name ___________________________
13
Date ___________________
Class __________________
STATES OF MATTER
Chapter Test B A. Matching Match each term in Column B to the correct description in Column A. Write the letter of the correct term on the line.
Column A
Column B a. normal boiling point
________ 2. a measure of the force exerted by a gas above a liquid
b. pascal
________ 3. The tiny particles in all forms of matter are in constant motion.
c. kinetic energy
________ 4. the temperature at which a solid changes into a liquid
d. standard atmosphere
________ 5. the pressure required to 760 mm of Hg at 25C
e. melting point
________ 6. the change of a substance from a solid to a gas or vapor without ing through the liquid state
f. triple point
________ 7. the SI unit of pressure
g. evaporation
________ 8. the conversion of a liquid to a gas or vapor at a temperature below the liquid’s boiling point
h. kinetic theory
________ 9. describes the only conditions of temperature and pressure at which all three phases of a substance can exist in equilibrium
i. allotropes
________ 10. the pressure that results from the collisions of particles in air with objects
j. barometer
________ 11. the temperature at which a liquid boils at a pressure of 101.3 kPa
k. sublimation
________ 12. the smallest group of particles within a crystal that retains the geometric shape of the crystal
l. atmospheric pressure
________ 13. the energy an object has because of its motion ________ 14. two or more different molecular forms of the same element in the same physical state
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m. unit cell n. vapor pressure
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________ 1. an instrument used to measure atmospheric pressure
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Date ___________________
Class __________________
B. Multiple Choice Choose the best answer and write its letter on the line. ________ 15. According to the kinetic theory, gases consist of particles that a. occupy considerable volume. b. are relatively close together. c. exert attractive and repulsive forces on other particles. d. have motion that is constant, random, and rapid. ________ 16. As you climb a mountain, atmospheric pressure: a. increases. c. remains the same. b. decreases. d. varies randomly. ________ 17. Which of the following is true about atmospheric pressure? a. It is measured with a hydrometer. b. It varies widely, depending on the weather. c. It increases with altitude. d. It affects the boiling point of a liquid.
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________ 18. At sea level in fair weather, atmospheric pressure is equal to a. 101.3 kPa. c. 760 mm Hg. b. 1 standard atmosphere. d. all of the above ________ 19. STP refers to: a. 100C and 1 atm. b. 0C and 1 kPa.
c. 0C and 1 atm. d. 100C and 760 mm Hg.
________ 20. A pressure of 2.5 atm is equivalent to a. 41 kPa. b. 1900 mm Hg.
c. 3.0 102 mm Hg. d. 2.5 kPa.
________ 21. Absolute zero is a. the temperature at which the motion of particles theoretically ceases. b. defined as 0C. c. the triple point for water. d. all of the above ________ 22. At 80 K, the particles of a gas have a. twice the average kinetic energy of the same particles at 40 K. b. half the average kinetic energy of the same particles at 40 K. c. one fourth the average kinetic energy of the same particles at 20 K. d. none of the above ________ 23. Compared with gases, liquids: a. have stronger intermolecular attractions. b. have more space between their particles. c. are much less dense. d. are more easily compressed.
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________ 24. Evaporation is a type of a. boiling. b. vaporization.
Class __________________
c. sublimation. d. condensation.
________ 25. A decrease in the temperature of a contained liquid causes a. an increase in the vapor pressure. b. a decrease in the vapor pressure. c. more particles to evaporate. d. an increase in the average kinetic energy of the particles. ________ 26. Water could be made to boil at 92C by a. lowering the external air pressure. b. raising the external air pressure. c. increasing the pressure on the water. d. none of the above ________ 27. In comparison with liquids and gases, solids are a. more dense. c. less organized. b. more easily compressed. d. more likely to flow. ________ 28. Diamond and graphite are examples of a. phases. c. allotropes. b. amorphous solids. d. glasses. ________ 29. The conditions at which the solid, liquid, and gaseous phases of a substance can exist in equilibrium with one another is called a. boiling point. c. sublimation point. b. freezing point. d. triple point.
C. True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. ________ 31. In an elastic collision, kinetic energy is transferred from one particle to another, but the total kinetic energy remains constant. ________ 32. Atmospheric pressure is 101.3 kPa. ________ 33. The Kelvin temperature of a substance is directly proportional to the average kinetic energy of the particles in that substance. ________ 34. At any given temperature, the particles of all substances have the same average kinetic energy. ________ 35. The temperature of a boiling liquid can rise above its boiling point. ________ 36. Water boils at 100C. ________ 37. The melting and freezing points of a substance are the same temperature.
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________ 30. Sublimation can occur because solids have a. a melting point. c. a boiling point. b. a vapor pressure. d. a triple point.
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Name ___________________________
Date ___________________
Class __________________
D. Essay Write a short essay for the following. 38. Distinguish between the boiling point and the normal boiling point of a liquid. Explain the impact of a change in atmospheric pressure on the relationship between the boiling point and the normal boiling point.
E. Additional Questions Answer the following questions in the space provided.
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39. Distinguish between gases, liquids, and solids in of the kinetic theory.
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Date ___________________
Class __________________
40. Explain why each of the following is true. a. The temperature of a boiling liquid never rises above its boiling point.
b. The temperature of an ice and water mixture at 1 standard atmosphere remains at 0C as long as both ice and liquid water are present, no matter what the surrounding temperature.
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