States of Matter

1
Table of Contents

• States of Matter
• Changes of State
• Gas Behavior
• Graphing Gas Behavior

2
Learning Objectives

• Describe the characteristics of
• Solids
• Liquids
• Gases
• Note that these characteristics include
  definite shape, definite volume, kinetic energy
  of the particles that make up each state of
  matter, and the distance between the particles
  for each state of matter.

3
Solids, Liquids, Gases

• Goal Compare and contrast characteristics of
  solids, liquids, and gases while reviewing the
  signs of a chemical change energy changes.
• Examine the citric acid with the magnifying glass
  and the green substance in the film canister.
• Place no more than HALF a spoonful of citric acid
  and baking soda in the bag, the place the film
  canister in the bag too (but make sure it doesnt
  spill). Then seal the bag and shake it. Be sure
  to make several different observations including
  feeling the bag. When the change is about
  finished, then open the bag up. Note that the
  gas shouldnt be in your table until you perform
  the experiment.
• Create a table like the one on the next slide and
  complete it in your lab notebook. MAKE SURE YOU
  HAVE ONLY 1 SOLID, 1 LIQUID, AND 1 GAS IN THE
  TABLE! Then answer the questions below the
  table.

4
Solids, Liquids, Gases Data Analysis
Substance (Name or Description such its color or clear if its colorless) Definite Shape (Yes, No, or No- Takes the shape of the container) Definite Volume (Yes or No) Solid, Liquid, or Gas



Review (Changes in Matter) Was there a chemical
change? If so, then list the signs you used to
tell that a chemical reaction took place? Review
(Changes in Energy) Was there a change in
energy? Was the change an endothermic or
exothermic change? Explain how you know.
5
Learning Objectives

• Describe the characteristics of
• Solids
• Liquids
• Gases
• Note that these characteristics include
  definite shape, definite volume, kinetic energy
  of the particles that make up each state of
  matter, and the distance between the particles
  for each state of matter.

6
Solids
- States of Matter

• A fixed, closely packed arrangement of particles
  causes a solid to have a definite shape and
  volume. KE low

7
Solids
- States of Matter

• In amorphous solids, the particles are not
  arranged in a regular pattern. Particles are
  arranged randomly, so these solids are more
  brittle and break unevenly. Example- Glass

• Solids that are made up of crystals are called
  crystalline solids. Example- Table Salt

8
Liquids
- States of Matter

• Because its particles are free to move, a liquid
  has NO definite shape. However, it does have a
  definite volume. KE middle
• Liquids also have several other properties
  including surface tension (particles pulling
  inward making the surface particles closer
  together to form a sort of skin) and viscosity
  (resistance to flow).

9
Gases
- States of Matter

• As they move, gas particles spread apart, filling
  all the space available. Thus, a gas has neither
  definite shape nor definite volume. KE high

10
Which of the following could be classified as an
amorphous solid?

1. Butter
2. Glass
3. Salt
4. Choices A B are correct.
5. Choices A, B C are correct.

11
Why are some substances that are more dense than
water able to float on its surface?

1. Due to waters mass
2. Due to waters skin-like surface
3. Due to waters viscosity
4. Due to waters density

12
If a substance has a high viscosity, then what
would you observe if you saw someone pouring the
substance into a container?

1. The substance will pour quickly at first and then
   slowly.
2. The substance has a high surface tension.
3. The substance will pour quickly because it cannot
   resist the force of gravity.
4. The substance will pour slowly because it can
   resist the force of gravity.

13
Which of the following substances has the highest
viscosity?

1. Honey
2. Glass
3. Water
4. Motor Oil

14
Which of the following have a definite shape?

1. Solids
2. Liquids
3. Gases
4. All of the above

15
Which of the following have a definite volume?

1. Solids
2. Liquids
3. Gases
4. Choices A B
5. Choices A, B, C

16
Which of the following takes the shape of the
container?

1. Solids
2. Liquids
3. Gases
4. All of the above

17
Which of the following have neither definite
shape nor a definite volume?

1. Solids
2. Liquids
3. Gases
4. All of the above

18
Rank solids, liquids, and gases in terms of the
kinetic energy of their particles. 1 Least
kinetic energy, 3 Most kinetic energy

1. 1 Gases, 2 Solids, 3 Liquids
2. 1 Liquids, 2 Solids, 3 Gases
3. 1 Solids, 2 Liquids, 3 Gases
4. 1 Gases, 2 Liquids, 3 Solids

19
Rank the states of matter in terms of the
distance between their particles. 1 Closest
together, 3 Furthest apart

1. 1 Solids, 2 Liquids, 3 Gases
2. 1 Gases, 2 Liquids, 3 Solids
3. 1 Liquids, 2 Gases, 3 Solids
4. 1 Solids, 2 Gases, 3 Liquids

20
Building Vocabulary
- States of Matter

• A definition states the meaning of a word or
  phrase by telling about its most important
  feature or function. After you read the section,
  reread the paragraphs that contain definitions of
  Key Terms. Use all the information you have
  learned to write a definition of each Key Term.

Key Terms
Examples
solid
A solid has a definite shape and a definite
volume.
Surface tension is the result of an inward pull
among the molecules of a liquid that brings the
molecules on the surface closer together.
crystalline solid
Solids that are made up of crystals are called
crystalline solids.
Another property of liquids is viscositya
liquids resistance to flowing.
amorphous solid
In amorphous solids, the particles are not
arranged in a regular pattern.
Like a liquid, a gas is a fluid. Unlike a liquid,
however, a gas can change volume very easily.
liquid
A liquid has a definite volume but no shape of
its own.
fluid
A liquid is also called a fluid, meaning a
substance that flows.
21
Viscosity
- States of Matter

• Click the Video button to watch a movie about
  viscosity.

22
End of SectionStates of Matter
23
Noggin Knocker Quiz (7 points-1 pt. per problem)

• 1a- Solids
• 1b- Gases
• 2- Liquids
• 3- Vibrate back and forth
• 4- Gases
• 5- Due to surface tension
• 6- Maple Syrup

24
Effect of Temperature on Particle Movement (No
lab write-up)

• Goal- Determine how temperature affects the
  movement (and KE) of the particles that make up
  matter.
• Hypothesis (in your head)- Which type of water
  will cause the particles of water to move faster
  hot or cold? Why?
• Procedure- Place hot water on one side of the
  divider of the plexiglass container and cold
  water on the other side. Immediately drop 2-3
  drops of food coloring on each side and observe
  what happens.
• Conclusion- How did temperature affect the
  movement of the particles of water (as indicated
  by the food dye)? Explain how you know.

25
Learning Objectives

• Explain what happens to a substance during the
  changes between
• Solid and Liquid
• Liquid and Gas
• Solid and Gas

26
Changes Between Solid and Liquid
- Changes of State

• The change in state from a solid to a liquid is
  called melting.
• What is needed for silver or any other solid to
  melt?
• Energy!
• As the molecules receive more energy, what do
  they start to do (more of)?
• They move more freely.
• This causes the substance itself to expand, but
  the particles do NOT expand. They spread farther
  apart!!!

27
Changes Between Solid and Liquid
- Changes of State

• The change of state from liquid to solid is
  called freezing.

28
Changes Between Liquid and Gas

• The change of state from liquid to gas is called
  vaporization.
• Vaporization can occur by boiling (vaporization
  below the liquid surface and on the liquid
  surface) or by evaporation (vaporization ONLY on
  the liquid surface). See Figure 11 on page 51 of
  your textbook.
• The change of state from gas to liquid is called
  condensation. Example- Water condensing on a
  mirror from a hot shower.

29
Learning Objectives

• Explain what happens to a substance during the
  changes between
• Solid and Liquid
• Liquid and Gas
• Solid and Gas

30
Changes Between Solid and Gas

• The change of state from solid to gas is called
  sublimation. Examples- Dry ice Iodine.
• Solid Gas

31
What happens to a solid metal when heated (but
not so much that the solid metal would melt)?

1. The metal would not change at all.
2. The metal would expand.
3. The metal would shrink.
4. The metal would break.

32
What caused the solid metal to expand from the
previous question?

1. The cold caused the particles to come closer
   together.
2. The heat caused the particles to come closer
   together.
3. The cold caused the particles to spread slightly
   further apart.
4. The heat caused the particles to spread slightly
   further apart.

33
Why does the liquid inside a thermometer move up
when the temperature increases?

1. The liquid doesnt move up the thermometer.
2. The liquid expands and can only go up the tube
   because the particles are starting to move faster
   and spread further apart.
3. The liquid would shrink an can only go down the
   tube because the particles are slowing down and
   getting closer together.
4. The liquid wouldnt rise up the tube, it would
   just get warmer.

34
A change where a solid becomes a liquid is called

1. freezing
2. melting
3. sublimation
4. vaporization
5. constipation

35
The change from a liquid to a gas is called
______________, while a change from a gas to a
liquid is called ____________.

1. Vaporization condensation
2. Vaporization freezing
3. Condensation vaporization
4. Condensation sublimation

36
If a substance melts at 20oC and boils at 180oC,
then at what temperature would the substance be a
gas?

1. 200oC
2. 150oC
3. 20oC
4. 10oC

37
Some Glade air freshener plug-ins contain a solid
substance that gives off sweet smelling vapors.
This is an example of

1. freezing
2. melting
3. vaporization
4. sublimation

38
Phase Change Diagram for Water Experiment

• Goal Observe and explain temperature changes as
  ice water is heated to past boiling.
• Hypothesis Sketch what you believe a
  temperature-time graph would look like for
  heating ice water to boiling.
• Procedure
• Observe the graph when the ice is melting, when
  the water is boiling, and the water temperature
  between melting and boiling.
• Results
• Sketch the graph in your lab notebook with the
  x-axis and y-axis properly labeled.
• There should be 3 parts to the graph one flat
  line, one slanted line, and another flat line.
• Label the parts of the graph as boiling, melting,
  or liquid.
• Add another slanted line where the solid phase
  would show up on the graph and label it solid,
  then do the same thing for where the gas phase
  would be on the graph. Think about where these
  lines should be based upon the pattern you
  observed during the experiment!

39
Analysis

• Discussion/Conclusions (in complete sentences)
• What happened to the water particles as the
  experiment progressed (moved forward)?
• Using evidence from your experiment, why didnt
  the temperature go up when the ice was melting
  and the water was boiling even though heat was
  being added? Hint- Determine if melting and
  boiling are endo- or exothermic changes first,
  and then use the definition to arrive at your
  answer.

40
Temperature and Changes of State
- Changes of State

• Interpreting Data
• What does the temperature value for segment B
  represent? For segment D?

• Segment B melting point of ice segment D
  boiling point of water

41
Temperature and Changes of State
- Changes of State

• Inferring
• In which segment, A or E, do the water molecules
  have more thermal energy? Explain your reasoning.

• Water molecules in segment E have more thermal
  energy because they are at a higher temperature.

42
Phase Change Review By examining the data table
below, determine at which temperature a solid
melted.

1. 75oC
2. 210oC
3. 98oC
4. 134oC
5. 160 oC

Time (min.) Temp. (oC)
0 46
5 75
10 75
15 75
20 98
25 134
30 160
43
A state of matter with a definite shape and
volume is a

1. liquid
2. solid
3. gas
4. All of the above

44
Solids can be either _________ or ________.

1. Amorphous or powders.
2. Crystalline or amorphous.
3. Crystalline or small.
4. Chunks or powders.

45
In which state of matter are the particles packed
tightly together in fixed positions?

1. gas
2. liquid
3. solid
4. All of the above

46
In which state of matter do the particles have
the lowest amount of kinetic energy?

1. solid
2. liquid
3. gas
4. All of the above

47
What state of matter is made up of the particles
that are the furthest apart?

1. solids
2. liquids
3. gases
4. All of the above

48
Particles of a liquid

1. are free to move in a container but remain in
   close contact with one another.
2. have no viscosity.
3. decrease in volume with increasing temperature.
4. All of the above are true.

49
The resistance of a liquid to flowing is its

1. Pressure
2. Surface tension
3. Viscosity
4. gravity

50
Some insects can walk on top of a sample of
water. This is likely due to waters

1. Pressure.
2. Surface tension.
3. Volume.
4. Viscosity.

51
The freezing point of water is the same as its

1. Boiling point.
2. Melting point.
3. Flash point.
4. Sharp point.

52
Suppose a substance has a melting point of -20oC
and a boiling point of 200oC. At what
temperature would the substance be a liquid?

1. -30oC
2. 80oC
3. -100oC
4. 212oC

53
What process occurs when water is heated on a
stove?

1. Sublimation
2. Melting
3. Condensation
4. Vaporization

54
An uncovered pot of soup is simmering on a stove,
and there are water droplets on the wall above
the back of the stove. What sequence can you
infer has occurred?

1. Condensation then vaporization
2. Melting then boiling
3. Freezing then thawing
4. Vaporization then condensation

55
Since iodine can go directly from a solid to gas,
it undergoes ____________.

1. vaporization
2. freezing
3. sublimation
4. condensation

56
In cold climates, the amount of snow on the
ground may decrease even if the temperature stays
below freezing (zero degrees Celsius). The
process that best explains this event is

1. Melting.
2. Vaporization.
3. Sublimation.
4. Freezing.

57
End of SectionChanges of State
58
Noggin Knockers- 10 points (Hwk. Grade)

1. The particles move faster and spread apart. (2
   points)
2. Melt the snow so you do NOT lose body heat. (2
   points)
3. Heat from your body causes the sweat to
   evaporate, so you feel cooler. (2 points)
4. Sublimation (1 point)
5. Water vapor condenses to form liquid water. (2
   points)
6. Any temperature from -9.9oC to 89.9oC would be
   correct. (1 point)

59
Learning Objectives

1. List the types of measurements used when working
   with gases.

60
A Change in Pressure
- Gas Behavior

• A punctured basketball deflates as gas particles
  begin to escape.
• What are two other factors that would be useful
  when discussing the pressure of a gas?
• Temperature and Volume

61
Learning Objective

• Explain how the temperature, volume, and pressure
  of a gas are related (when the number of gas
  particles is kept constant).
• Pressure and Volume (constant temperature)
• Pressure and Temperature (constant volume)
• Volume and Temperature (constant pressure)

62
Gas Law Activities/Demos Boyles Law

• Goal Determine the relationship between the
  pressure and volume of a sample of gas in a
  closed container at constant temperature.
• Predictions/Hypothesis What will happen to the
  VOLUME of jet-puffed marshmallows when pressure
  is increased? VOLUME when the pressure is
  decreased?
• Results List volume observations of the
  marshmallows under different pressures (pulling
  up vs. pushing down on the plunger of the
  syringe).
• Conclusion State your claim/conclusion (see
  goal) and provide evidence from the experiment.

63
Pressure and Volume
- Gas Behavior

• As weights are added, the gas particles occupy a
  smaller volume. The pressure increases. This is
  Boyles Law.

64
If you reduce the volume of a gas in a cylinder
by pushing the piston down, then the pressure
inside would

1. Decrease.
2. Increase.
3. Stay the same.

65
Before the breath in, your chest cavity and lungs
expand (get bigger). This allows the air outside
to flow in because the pressure inside your lungs

1. Decreased.
2. increased
3. Stay the same.

66
Deep sea divers can sometimes risk severe pains
or death if they come to the surface too quickly.
As they ascend to the surface, the gases
dissolved in their blood will __________.

1. Expand until they are big enough to cause pain.
2. Contract until they are small enough to cause
   pain.
3. Stay the same volume or size.
4. React with the iron in your blood.

67
Gas Law Activities/Demos Pressure Temperature

• Goal Determine the relationship between the
  pressure and temperature of a sample of gas in a
  closed container at constant volume.
• Predictions/Hypothesis Write your hypothesis
  for the experiment. Be sure that it corresponds
  to the goal above.
• Results List pressure observations of the
  apparatus under different temperatures (Hot vs.
  Cold Water).
• Conclusion State your claim/conclusion (see
  goal) and provide evidence from the
  demonstration. Explain what happens to the
  particles of a gas when heated or cooled.

68
Pressure and Temperature
- Gas Behavior

• When a gas is heated, the particles move faster
  and collide more often with each other and with
  the walls of their container. The pressure of the
  gas increases.

69
Why are truck and car tires more likely to pop in
the summer?

1. Because its warmer, so the pressure inside will
   decrease and the tire deflates.
2. Because its colder, so the pressure inside will
   increase and build up.
3. Because its warmer, so the pressure inside will
   increase and build up.
4. Because its colder, so the pressure inside will
   increase and build up.

70
Why do mechanics recommend putting more air
(greater pressure) in your tires in the winter?

1. Because the warmer temperatures dont affect the
   pressure inside the tire.
2. Because the colder temperatures cause the tires
   to explode due to more pressure inside them.
3. Because the warmer temperatures cause the tire to
   deflate slightly due to the lower pressure inside
   the tire.
4. Because the colder temperatures cause the tire to
   deflate slightly due to the lower pressure inside
   the tire.

71
Gas Law Activities/Demos Charles Law

• Goal Determine the relationship between the
  volume and temperature of a sample of gas in a
  closed system at constant pressure.
• Predictions/Hypothesis Write your hypothesis
  for the experiment.
• Results List volume observations of the ivory
  soap when heated and the balloon when cooled with
  liquid nitrogen.
• Conclusion State your claim/conclusion (see
  goal) and provide evidence from the
  demonstrations. Explain what happens to the
  distance between the particles as a gas is heated.

72
Volume and Temperature
- Gas Behavior

• Changing the temperature of a gas at constant
  pressure changes the volume similarly. This is
  Charles Law.

73
As the temperature of a gas in a closed container
increases, the volume of the gas will

1. Decrease.
2. Increase.
3. Stay the same.

74
What tends to happen to the volume of a car tire
in the winter months?

1. It decreases.
2. It increases.
3. It stays the same.
4. Nothing happens.

75
Gas Law Activities/Demos Charles Law

• Goal Determine the relationship between the
  volume and temperature of a sample of gas in a
  closed system at constant pressure.
• Predictions/Hypothesis Write your hypothesis
  for the experiment.
• Results List volume observations of the ivory
  soap when heated and the balloon when cooled with
  liquid nitrogen.
• Conclusion State your claim/conclusion (see
  goal) and provide evidence from the
  demonstrations. Explain what happens to the
  distance between the particles as a gas is heated.

76
Pressure and Volume
- Graphing Gas Behavior

• Graph the data from the experiment below in your
  lab notebook table. Note that you may want to
  start with the bottom data point.

77
Pressure and Volume
- Graphing Gas Behavior

• The graph of Boyles law shows that the pressure
  of a gas varies inversely with its volume at
  constant temperature.

78
Temperature and Volume
- Graphing Gas Behavior

• The data from the experiment are recorded in the
  notebook table.
• In your lab notebook, sketch what you think the
  volume vs. temperature graph will look like.
  This is your hypothesis.
• Then plot the VOLUME data to the right for EVERY
  20oC and create a best-fit line on your graph.
• Temperature and volume are
• Directly proportional

79
Temperature and Volume
- Graphing Gas Behavior

• The graph of Charless law shows that the volume
  of a gas is directly proportional to its kelvin
  (and Celsius) temperature under constant pressure.

80
Noggin Knockers (Quiz grade- 9 pts.)

• 1 (2 pts.)- Higher temperature faster moving
  gas particles greater pressure.
• 2 (2 pts.)- Dont inflate the balloons as much
  because as the temp. of a gas increases, so does
  volume since the balloons would expand (for
  constant pressure).
• 3 (3 pts.)- Pressure inside your body/chest
  cavity increases and the volume of your lungs
  decreases as air flows out of your mouth.
• 4 (1 pt.)- Inversely (pressure increases, volume
  decreases and vice-versa)
• 5 (1 pt.)- Directly (Volume and temperature
  increase and decrease together)

81
Asking Questions
- Gas Behavior

• Before you read, preview the red headings. In a
  graphic organizer like the one below, ask a what
  or how question for each heading. As you read,
  write answers to your questions.

Questions
Answers
What measurements are useful in studying gases?
Volume, temperature, and pressure
How are the pressure and volume of gases related?
When the pressure of a gas increases at constant
temperature, its volume decreases.
How are the pressure and temperature of gases
related?
When the temperature of a gas increases at
constant volume, its pressure increases.
How are the volume and temperature of gases
related?
When the temperature of a gas increases at
constant pressure, its volume increases.
82
End of SectionGas Behavior
83
Homework p. 61- 1 2 (all parts)- 2 pts. per ?

• 1a- The outward force of the gas particles
  divided by the area of the walls of the
  container.
• 1b- Gas particles exert pressure by colliding
  with the inside of the container. Faster moving
  particles more pressure.
• 1c- More gas particles more collisions with the
  inside of the ball more pressure
• 2a- Volume decreases, pressure increases and
  vice-versa
• 2b- Higher temperature faster moving gas
  particles greater pressure
• 2c- Dont inflate the balloons as much because as
  the temp. of a gas increases, so does volume (for
  constant pressure)

84
Learning Objectives

• Identify the type of relationship shown by the
  graph for Boyles Law.
• Identify the type of relationship shown by the
  graph for Charles Law.

85
Pressure and Volume
- Graphing Gas Behavior

• Graph the data from the experiment below in your
  lab notebook table. Note that you may want to
  start with the bottom data point.

86
Pressure and Volume
- Graphing Gas Behavior

• The graph of Boyles law shows that the pressure
  of a gas varies inversely with its volume at
  constant temperature.

87
Temperature and Volume
- Graphing Gas Behavior

• The data from the experiment are recorded in the
  notebook table.
• In your lab notebook, sketch what you think the
  volume vs. temperature graph will look like.
  This is your hypothesis.
• Then plot the VOLUME data to the right for EVERY
  20oC and create a best-fit line on your graph.
• Temperature and volume are
• Directly proportional

88
Temperature and Volume
- Graphing Gas Behavior

• The graph of Charless law shows that the volume
  of a gas is directly proportional to its kelvin
  (and Celsius) temperature under constant pressure.

89
Making a Graph
- Graphing Gas Behavior

• The x-axis (horizontal) and the y-axis (vertical)
  form the backbone of a graph.

90
Graphing Boyles Law

• Goal Graph pressure and volume data for a
  closed sample of gas at constant temperature
  determine the relationship between pressure and
  volume shown by the graph.
• Hypothesis (1) Sketch what you think the
  volume vs. pressure graph will look like based
  upon your prior knowledge. (2) Predict what
  will happen to the volume of the gas when more
  books (greater pressure) are added to a sealed
  syringe. These 2 predictions should match up!
• Results/Conclusion Record your data construct
  a graph based upon the steps on pages 66 67,
  but use 2 books for each 1 book youre supposed
  to use.
• Also, you may need to estimate the volume with 0
  books since it may be above the graduations on
  the syringe.
• Exclude Procedure steps 9 10 and Analyze
  Conclude steps 2, 3, 4.

91
Pressure and Volume
- Graphing Gas Behavior

• Pushing on the top of the piston decreases the
  volume of the gas. The pressure of the gas
  increases.

92
Pressure and Volume
- Graphing Gas Behavior

• The graph of Boyles law shows that the pressure
  of a gas varies inversely with its volume at
  constant temperature.

93
What would the graph look like for a volume vs.
pressure graph of a gas at constant temperature
in a sealed container?

1. A straight line going up and to the right.
2. A curved line going downward and to the right.
3. A curved line going upward and to the right.
4. A straight line going down and to the right.

94
By examining a pressure-volume graph of a gas in
a sealed container at a constant temperature, the
relationship between pressure and volume is

1. Not related.
2. The same.
3. Inversely proportional.
4. Directly proportional.

95
Phase Change Review By examining the data table
below, determine at which temperature a liquid
turned into a gas (or boiled). Hint- Think back
to your phase change diagram for water lab and
assume the substance started out as a liquid.
Time (min.) Temp. (oC)
0 23
5 46
10 75
15 120
20 120
25 120
30 160
35 210

1. 75oC
2. 210oC
3. -10oC
4. 120oC
5. 160 oC

96
Temperature and Volume
- Graphing Gas Behavior

• As the temperature of the water bath decreases,
  the gas inside the cylinder is cooled by the
  water. The volume is then decreased.

97
Temperature and Volume
- Graphing Gas Behavior

• The data from the experiment are recorded in the
  notebook table.
• In your lab notebook, sketch what you think the
  volume vs. temperature graph will look like.
  This is your hypothesis.
• Then plot the VOLUME data to the right for EVERY
  20oC and create a best-fit line on your graph.
• Temperature and volume are
• Directly proportional

98
Temperature and Volume
- Graphing Gas Behavior

• The graph of Charless law shows that the volume
  of a gas is directly proportional to its kelvin
  (and Celsius) temperature under constant pressure.

99
How does the graph for Charles Law appear? Its
a volume vs. temperature graph.

1. A curved line going up and to the right.
2. A straight line going up and top the right.
3. A curved line going down and to the right.
4. A straight line going down and to the right.

100
The Charles Law graph clearly shows that as
temperature increases, volume

1. Increases then decreases.
2. Stays the same.
3. Decreases.
4. Increases.

101
Practice Problems

• p. 65- 1b Volume increases when temp. goes up.
• 1c 73-78 mL (See Figure 23)
• 2a Pressure goes up, volume goes down
• 2b 45-56 kPa (kilopascals- units of pressure)
• 2c Line going up and to the right directly
  proportional
• Line going down and to the right inversely
  proportional
• p. 69- 1 b (liquid) 2 c (expand to fill all
  available space) 3 d (condensation)
• p. 70- 21 Sublimation occurs (solid directly to
  a gas)
• p. 71- 1 C (Evaporation)

102
Previewing Visuals
- Graphing Gas Behavior

• Before you read, preview Figure 23. In a graphic
  organizer like the one below, write questions
  that you have about the diagram. As you read,
  answer your questions.

Graphing Charless Law
Q. What is the relationship between temperature
and volume?
A. The volume of a gas is directly proportional
to its temperature under constant pressure.
Q. What does the dotted line show?
A. The dotted line predicts how the graph would
look if the gas could be cooled further.
103
Links on Gases
- Graphing Gas Behavior

• Click the SciLinks button for links on gases.

104
End of SectionGraphing Gas Behavior
105
Graphic Organizer

Solids, Liquids, and Gases
Example (at room temperature)
State of Matter
Shape
Volume
Solid
Definite
Definite
Diamond
Not definite
Water
Liquid
Definite
Not definite
Oxygen
Gas
Not definite
106
End of SectionGraphic Organizer
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