• Home
  • Textbooks
  • Chemistry Matter and Change
  • States of Matter

Chemistry Matter and Change

Thandi Buthelezi, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom, Dinah Zike

Chapter 12

States of Matter - all with Video Answers

Educators


Chapter Questions

00:41

Problem 1

Calculate the ratio of effusion rates for nitrogen $\left(\mathrm{N}_{2}\right)$ and neon (Ne).

Anna Miller
Anna Miller
Numerade Educator
01:30

Problem 2

Calculate the ratio of diffusion rates for carbon monoxide and carbon dioxide.

Anna Miller
Anna Miller
Numerade Educator
View

Problem 3

Challenge What is the rate of effusion for a gas that has a molar mass twice that of
a gas that effuses at a rate of 3.6 $\mathrm{mol} / \mathrm{min}$ ?

Rachel Levin
Rachel Levin
Numerade Educator
01:07

Problem 4

What is the partial pressure of hydrogen gas in a mixture of hydrogen and helium if the
total pressure is 600 $\mathrm{mm} \mathrm{Hg}$ and the partial pressure of helium is 439 $\mathrm{mm} \mathrm{Hg?}$

Anna Miller
Anna Miller
Numerade Educator
00:36

Problem 5

Find the total pressure for a mixture that contains four gases with partial pressures of
$5.00 \mathrm{kPa}, 4.56 \mathrm{kPa}, 3.02 \mathrm{kPa},$ and 1.20 $\mathrm{kPa}$

Anna Miller
Anna Miller
Numerade Educator
01:18

Problem 6

Find the partial pressure of carbon dioxide in a gas mixture with a total pressure of 30.4 $\mathrm{kPa}$ if the partial pressures of the other two gases in the mixture are 16.5 $\mathrm{kPa}$ and 3.7 $\mathrm{kPa}$ .

Anna Miller
Anna Miller
Numerade Educator
00:51

Problem 7

Challenge Air is a mixture of gases. By percentage, it is roughly 78 percent nitrogen,
21 percent oxygen, and 1 percent argon. (There are trace amounts of many other gases
in air. If the atmospheric pressure is 760 $\mathrm{mm}$ Hg, what are the partial pressures of
nitrogen, oxygen, and argon in the atmosphere?

Anna Miller
Anna Miller
Numerade Educator
00:49

Problem 8

Explain Use the kinetic theory to explain the behavior of gases.

Anna Miller
Anna Miller
Numerade Educator
00:30

Problem 9

Describe how the mass of a gas particle affects its rate of effusion and
diffusion.

Anna Miller
Anna Miller
Numerade Educator
06:16

Problem 10

Explain how gas pressure is measured.

Caroline Basil
Caroline Basil
Numerade Educator
00:26

Problem 11

Explain why the container of water must be inverted when a gas is collected by
displacement of water.

Anna Miller
Anna Miller
Numerade Educator
01:06

Problem 12

Calculate Suppose two gases in a container have a total pressure of 1.20 atm.
What is the pressure of Gas $B$ if the partial pressure of Gas A is 0.75 atm?

Anna Miller
Anna Miller
Numerade Educator
00:28

Problem 13

Infer whether or not temperature has any effect on the diffusion rate of a gas.
Explain your answer.

Anna Miller
Anna Miller
Numerade Educator
00:56

Problem 14

Explain what determines a substance's state at a given
temperature.

Anna Miller
Anna Miller
Numerade Educator
00:47

Problem 15

Compare and contrast intermolecular forces and describe intramolecular
forces.

Anna Miller
Anna Miller
Numerade Educator
05:38

Problem 16

Evaluate Which of the molecules listed below can form hydrogen bonds? For
which of the molecules would dispersion forces be the only intermolecular force?
Give reasons for your answers.
$$\text { a. }\mathrm{H}_{2} \quad \text { b. } \mathrm{H}_{2} \mathrm{S} \quad \text { c. }
\mathrm{HCl} \quad \text { d. } \mathrm{HF}$$

Caroline Basil
Caroline Basil
Numerade Educator
00:46

Problem 17

Intepret Data In a methane molecule $\left(\mathrm{H}_{4}\right),$ there four single covalent
bonds. In an octane molecule $\left(\mathrm{C}_{8} \mathrm{H}_{18}\right)$ , there are 25 single covalent bonds. How does the number of bonds affect the dispersion forces in samples of methane and octane? Which compound is a gas at room temperature? Which is a liquid?

Anna Miller
Anna Miller
Numerade Educator
00:34

Problem 18

Contrast the arrangement of particles in solids and liquids.

Anna Miller
Anna Miller
Numerade Educator
00:39

Problem 19

Describe the factors that affect viscosity.

Anna Miller
Anna Miller
Numerade Educator
00:52

Problem 20

Explain why soap and water are used to clean clothing instead of water alone.

Anna Miller
Anna Miller
Numerade Educator
00:38

Problem 21

Compare a unit cell and a crystal lattice.

Anna Miller
Anna Miller
Numerade Educator
01:11

Problem 22

Describe the difference between a molecular solid and a covalent network solid.

Anna Miller
Anna Miller
Numerade Educator
00:29

Problem 23

Explain why water forms a meniscus when it is in a graduated cylinder.

Anna Miller
Anna Miller
Numerade Educator
00:46

Problem 24

Infer why the surface of mercury in a thermometer is convex, that is, the surface
is higher at the center.

Anna Miller
Anna Miller
Numerade Educator
00:56

Problem 25

Predict which solid is more likely to be amorphous - one formed by allowing
a molten material to cool slowly to room temperature one formed by quickly
cooling the same material in an ice bath.

Anna Miller
Anna Miller
Numerade Educator
04:43

Problem 26

Design an experiment to compare the relative abilities of water and isopropyl
alcohol to support skipping stones. Include a prediction about which liquid will
be better, along with a brief explanation of your prediction.

Caroline Basil
Caroline Basil
Numerade Educator
00:52

Problem 27

Explain how the addition or removal of energy can cause a phase change.

Anna Miller
Anna Miller
Numerade Educator
00:39

Problem 28

Explain the difference between the processes of melting and freezing.

Anna Miller
Anna Miller
Numerade Educator
00:43

Problem 29

Compare deposition and sublimation.

Anna Miller
Anna Miller
Numerade Educator
01:27

Problem 30

Compare and contrast sublimation and evaporation.

Anna Miller
Anna Miller
Numerade Educator
01:01

Problem 31

Describe the information that a phase diagram supplies.

Anna Miller
Anna Miller
Numerade Educator
00:48

Problem 32

Explain what the triple point and the critical point on a phase diagram represent.

Anna Miller
Anna Miller
Numerade Educator
01:21

Problem 33

Determine the phase of water at $75.00^{\circ} \mathrm{C}$ and 3.00 atm using Figure 12.29

Anna Miller
Anna Miller
Numerade Educator
00:42

Problem 34

What is an elastic collision?

Anna Miller
Anna Miller
Numerade Educator
00:46

Problem 35

How does the kinetic energy of particles vary as a function of temperature?

Anna Miller
Anna Miller
Numerade Educator
01:04

Problem 36

Use the kinetic-molecular theory to explain the compression and expansion of gases.

Anna Miller
Anna Miller
Numerade Educator
00:47

Problem 37

List the three basic assumptions of the kinetic-molecular
theory.

Anna Miller
Anna Miller
Numerade Educator
01:05

Problem 38

Describe the common properties of gases.

Anna Miller
Anna Miller
Numerade Educator
01:10

Problem 39

Compare diffusion and effusion. Explain the relationship between the rates of these processes and the molar mass of a gas.

Anna Miller
Anna Miller
Numerade Educator
01:14

Problem 40

In Figure 12.31 , what happens to the density of gas particles in the cylinder as the piston moves from Position A to Position B?

Anna Miller
Anna Miller
Numerade Educator
01:24

Problem 41

Baking Explain why the baking instructions on a box
of cake mix are different for high and low elevations.
Would you expect to have a longer or a shorter cooking
time at a high elevation?

Anna Miller
Anna Miller
Numerade Educator
01:26

Problem 42

What is the molar mass of a gas that takes three times
longer to effuse than helium?

Anna Miller
Anna Miller
Numerade Educator
01:04

Problem 43

What is the ratio of effusion rates of krypton and neon
at the same temperature and pressure?

Anna Miller
Anna Miller
Numerade Educator
01:35

Problem 44

Calculate the molar mass of a gas that diffuses three
times faster than oxygen under similar conditions.

Anna Miller
Anna Miller
Numerade Educator
02:55

Problem 45

What is the partial pressure of water vapor in an air
sample when the total pressure is 1.00 atm, the partial
pressure of nitrogen is 0.79 atm, the partial pressure of
oxygen is 0.20 atm, and the partial pressure of all other
gases in air is 0.0044 atm?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:25

Problem 46

What is the total gas pressure in a sealed flask that contains oxygen at a partial pressure of 0.41 atm and water vapor at a partial pressure of 0.58 atm?

Anna Miller
Anna Miller
Numerade Educator
00:25

Problem 47

Mountain Climbing The pressure atop the world's
highest mountain, Mount Everest, is usually about 33.6
kPa. Convert the pressure to atmospheres. How does the
pressure compare with the pressure at sea level?

Anna Miller
Anna Miller
Numerade Educator
02:04

Problem 48

High Altitude The atmospheric pressure in Denver, Colorado, is usually about 84.0 $\mathrm{kP}$ a. What is this pres- sure in atm and torr units?

Anna Miller
Anna Miller
Numerade Educator
00:41

Problem 49

At an ocean depth of $76.2 \mathrm{m},$ the pressure is about
8.4 $\mathrm{atm} .$ Convert the pressure to $\mathrm{mm} \mathrm{Hg}$ and kPa units.

Anna Miller
Anna Miller
Numerade Educator
00:46

Problem 50

Figure 12.32 represents an experimental set-up in which
the left bulb is filled with chlorine gas and the right bulb
is filled with nitrogen gas. Describe what happens when
the stopcock is opened. Assume that the temperature of
the system is held constant during the experiment.

Anna Miller
Anna Miller
Numerade Educator
00:52

Problem 51

Explain the difference between a temporary dipole and a
permanent dipole.

Anna Miller
Anna Miller
Numerade Educator
00:46

Problem 52

Why are dispersion forces weaker than dipole-dipole
forces?

Anna Miller
Anna Miller
Numerade Educator
00:58

Problem 53

Explain why hydrogen bonds are stronger than most
dipole-dipole forces.

Anna Miller
Anna Miller
Numerade Educator
00:49

Problem 54

Compare intramolecular and intermolecular forces.

Anna Miller
Anna Miller
Numerade Educator
00:52

Problem 55

Hypothesize why long, nonpolar molecules would interact more strongly with one another than spherical
nonpolar molecules of similar composition.

Anna Miller
Anna Miller
Numerade Educator
01:32

Problem 56

Polar Molecules Use relative differences in electronegativity to label the ends of the polar molecules listed as partially positive or partially negative.
$$\quad \text { a. HF }\quad \text { b. HBr } \quad \text { c.NO } \quad \text { d. } C O$$

Anna Miller
Anna Miller
Numerade Educator
00:40

Problem 57

Draw the structure of the dipole-dipole interaction
between two molecules of carbon monoxide.

Anna Miller
Anna Miller
Numerade Educator
01:36

Problem 58

Decide which of the substances listed can form
hydrogen bonds.
$$\mathbf{a} \cdot \mathrm{H}_{2} \mathrm{O} \quad \text { b. } \mathrm{H}_{2} \mathrm{O}_{2} \quad \text { c. HF } \quad \text { d. } \mathrm{NH}_{3}$$

Anna Miller
Anna Miller
Numerade Educator
00:47

Problem 59

Decide which one of the molecules listed below can
form intermolecular hydrogen bonds, and then draw
it, showing several molecules attached together by
hydrogen bonds.
$$\quad \text { a. }\mathrm{NaCl}\quad \text { b. } \mathrm{MgCl}_{2} \quad \text { c. } \mathrm{H}_{2} \mathrm{O}_{2} \quad \mathrm{d} . \mathrm{CO}_{2}$$

Anna Miller
Anna Miller
Numerade Educator
00:39

Problem 60

What is surface tension, and what conditions must exist
for it to occur?

Anna Miller
Anna Miller
Numerade Educator
00:28

Problem 61

Explain why the surface of water in a graduated cylinder
is curved.

Anna Miller
Anna Miller
Numerade Educator
00:49

Problem 62

Which liquid is more viscous at room temperature,
water or molasses? Explain.

Anna Miller
Anna Miller
Numerade Educator
03:41

Problem 63

Explain how two different forces play a role in capillary
action.
$$\begin{array}{c}{a=b \neq c} \\ {\alpha=\beta=90^{\circ}, \gamma=120^{\circ}} \\ {\text { Hexagonal }}\end{array}$$$$
\begin{array}{c}{a \neq b \neq c} \\ {\alpha=\gamma=90^{\circ} \neq \beta} \\ {\text { Monoclinic }}\end{array}
$$$$
\begin{array}{c}{a=b=c} \\ {\alpha=\beta=\gamma=90^{\circ}} \\ {\text { Cubic }}\end{array}
$$

Caroline Basil
Caroline Basil
Numerade Educator
01:55

Problem 64

Use the drawings in Figure 12.33 to compare the cubic,
monoclinic, and hexagonal crystal systems.

Anna Miller
Anna Miller
Numerade Educator
00:22

Problem 65

What is the difference between a network solid and an
ionic solid?

Anna Miller
Anna Miller
Numerade Educator
00:51

Problem 66

Explain why most metals bend when struck but most
ionic solids shatter.

Anna Miller
Anna Miller
Numerade Educator
00:23

Problem 67

List the types of crystalline solids that are usually good
conductors of heat and electricity.

Anna Miller
Anna Miller
Numerade Educator
01:06

Problem 68

How does the strength of a liquid's intermolecular forces
affect its viscosity?

Anna Miller
Anna Miller
Numerade Educator
00:47

Problem 69

Explain why water has a higher surface tension than
benzene, whose molecules are nonpolar.

Anna Miller
Anna Miller
Numerade Educator
05:52

Problem 70

Compare the number of particles in one unit cell for
each of the following types of unit cells.
$$
\begin{array}{l}{\text { a. simple cubic }} \\ {\text { b. body-centered cubic }}\end{array}
$$

Caroline Basil
Caroline Basil
Numerade Educator
00:43

Problem 71

Predict which solid is more likely to be amorphous-
one formed by cooling a molten material over 4 h at
room temperature or one formed by cooling a molten
material quickly in an ice bath.

Anna Miller
Anna Miller
Numerade Educator
00:58

Problem 72

Conductivity Predict which solid will conduct electricity better-sugar or salt.

Anna Miller
Anna Miller
Numerade Educator
00:50

Problem 73

Explain why ice floats in water but solid benzene sinks
in liquid benzene. Which behavior is more "normal"?

Anna Miller
Anna Miller
Numerade Educator
10:09

Problem 74

Given edge lengths and face angles, predict the shape of
each of the following crystals.
$$
\begin{aligned} \text { a. } & a=3 \mathrm{nm}, b=3 \mathrm{nm}, c=3 \mathrm{nm} ; \alpha=90^{\circ}, \beta^{\circ}=90 \\ & \gamma=90^{\circ} \\ \text { b. } & a =4 \mathrm{nm}, b=3 \mathrm{nm}, c=5 \mathrm{nm} ; \alpha=90^{\circ}, \beta^{\circ}=100 \\ & \gamma=90^{\circ} \\ \text { c. } & a=3 \mathrm{nm}, b=3 \mathrm{nm}, c=5 \mathrm{nm} ; \alpha=90^{\circ}, \beta^{\circ}=90 \\ & \gamma=90^{\circ} \\ \text { d. } a &=3 \mathrm{nm}, b=3 \mathrm{nm}, c=5 \mathrm{nm} ; \alpha=90^{\circ}, \beta^{\circ}=90 \\ & \gamma=120^{\circ} \end{aligned}
$$

Caroline Basil
Caroline Basil
Numerade Educator
00:32

Problem 75

How does sublimation differ from deposition?

Anna Miller
Anna Miller
Numerade Educator
01:01

Problem 76

Compare boiling and evaporation.

Anna Miller
Anna Miller
Numerade Educator
00:23

Problem 77

Define the term melting point.

Anna Miller
Anna Miller
Numerade Educator
00:54

Problem 78

Explain the relationships among vapor pressure, atmospheric pressure, and boiling point.

Anna Miller
Anna Miller
Numerade Educator
00:23

Problem 79

Explain why dew forms on cool mornings.

Anna Miller
Anna Miller
Numerade Educator
00:44

Problem 80

Snow Why does a pile of snow slowly shrink even on
days when the temperature never rises above the freezing point of water?

Anna Miller
Anna Miller
Numerade Educator
01:35

Problem 81

Copy and label the solid, liquid, and gas phases, triple
point, and critical point on Figure 12.34

Anna Miller
Anna Miller
Numerade Educator
01:02

Problem 82

Why does it take more energy to boil 10 $\mathrm{g}$ of liquid
water than to melt an equivalent mass of ice?

Anna Miller
Anna Miller
Numerade Educator
00:40

Problem 83

Use the kinetic-molecular theory to explain why both
gases and liquids are fluids.

Anna Miller
Anna Miller
Numerade Educator
01:25

Problem 84

Use intermolecular forces to explain why oxygen is a gas
at room temperature and water is a liquid.

Anna Miller
Anna Miller
Numerade Educator
00:40

Problem 85

Use the kinetic-molecular theory to explain why gases
are easier to compress than liquids or solids.

Anna Miller
Anna Miller
Numerade Educator
01:50

Problem 86

At $25^{\circ} \mathrm{C}$ and a pressure of $760 \mathrm{mm} \mathrm{Hg},$ the density of
mercury is 13.5 $\mathrm{g} / \mathrm{mL}$ ; water at the same temperature
and pressure has a density of 1.00 $\mathrm{g} / \mathrm{mL}$ . Explain this
difference in terms of intermolecular forces and the
kinetic-molecular theory.

Anna Miller
Anna Miller
Numerade Educator
00:55

Problem 87

If two identical containers each hold the same gas at the
same temperature but the pressure inside one container
is exactly twice that of the other container, what must be
true about the amount of gas inside each container?

Anna Miller
Anna Miller
Numerade Educator
01:13

Problem 88

List three types of intermolecular forces.

Anna Miller
Anna Miller
Numerade Educator
01:12

Problem 89

When solid sugar crystals are dissolved in a glass of
water, they form a clear homogeneous solution in which
the crystals are not visible. If the beaker is left out at
room temperature for a few days, the crystals reappear
in the bottom and on the sides of the glass. Is this an
example of freezing?

Anna Miller
Anna Miller
Numerade Educator
01:39

Problem 90

Interpret Graphs Examine Figure $12.35,$ which plots
vapor pressure versus temperature for water and ethyl
alcohol.
$$\begin{array}{l}{\text { a. What is the boiling point of water at } 1 \text { atm? }} \\ {\text { b. What is the boiling point of ethyl alcohol at } 1 \text { atm? }} \\ {\text { c. Estimate the temperature at which water will boil }} \\ {\text { when the atmospheric pressure is } 0.80 \text { atm. }}\end{array}$$

Anna Miller
Anna Miller
Numerade Educator
01:30

Problem 91

Hypothesize What type of crystalline solid do you
predict would best suit the following needs?
$$
\begin{array}{l}{\text { a. a material that can be melted and reformed at a low }} \\ {\text { temperature }} \\ {\text { b. a material that can be drawn into long, thin wires }} \\ {\text { c. a material that conducts electricity when molten }} \\ {\text { d. an extremely hard material that is nonconductive }}\end{array}
$$

Anna Miller
Anna Miller
Numerade Educator
01:05

Problem 92

Compare and Contrast An air compressor uses energy to squeeze air particles together. When the air is released, it expands, allowing the energy to be used for purposes such as gently cleaning surfaces without using a more abrasive liquid or solid. Hydraulic systems essentially work the same way, but involve compression of liquid water rather than air. What do you think are some advantages and disadvantages of these two types of technology?

Anna Miller
Anna Miller
Numerade Educator
01:45

Problem 93

Graph Use Table 12.6 to construct a phase diagram for
ammonia.

Anna Miller
Anna Miller
Numerade Educator
00:53

Problem 94

Apply A solid being heated stays at a constant temperature until it is completely melted. What happens to the heat energy put into the system during that time?

Anna Miller
Anna Miller
Numerade Educator
00:52

Problem 95

Communicate Which process-effusion or diffusion-
is responsible for your being able to smell perfume from
an open bottle that is located across the room from you?
Explain.

Anna Miller
Anna Miller
Numerade Educator
01:37

Problem 96

Infer A laboratory demonstration involves pouring
bromine vapors, which are a deep red color, into a flask
of air and then tightly sealing the top of the flask. The
bromine is observed to first sink to the bottom of the
beaker. After several hours have passed, the red
color is distributed equally throughout the flask.
$$
\begin{array}{l}{\text { a. Is bromine gas more or less dense than air? }} \\ {\text { b. Would liquid bromine diffuse more or less quickly }} \\ {\text { than gaseous bromine after you pour it into another }} \\ {\text { liquid? }}\end{array}
$$

Anna Miller
Anna Miller
Numerade Educator
01:06

Problem 97

Analyze Use your knowledge of intermolecular forces
to predict whether ammonia (NH $_{3} )$ or methane $\left(\mathrm{CH}_{4}\right)$
will be more soluble in water.

Anna Miller
Anna Miller
Numerade Educator
01:14

Problem 98

Evaluate List three changes that require energy and
three that release energy.

Anna Miller
Anna Miller
Numerade Educator
01:52

Problem 99

Evaluate Supercritical carbon dioxide is a liquid form
of $\mathrm{CO}_{2}$ used in the food industry to decaffeinate tea, coffee, and colas, as well as in the pharmaceutical industry
to form polymer microparticles used in drug delivery
systems. Use Figure 12.36 to determine what conditions
must be used to form supercritical carbon dioxide.

Anna Miller
Anna Miller
Numerade Educator
07:40

Problem 100

You have a solution containing 135.2 g of dissolved $\mathrm{KBr}$
in 2.3 $\mathrm{L}$ of water. What volume of this solution, in mL,
would you use to make 1.5 $\mathrm{L}$ of a 0.1 $\mathrm{mol} / \mathrm{L}$ KBr solu-
tion? What is the boiling point of this new solution?

Caroline Basil
Caroline Basil
Numerade Educator
01:45

Problem 101

Identify each of the following as an element, a compound, a homogeneous mixture, or a heterogeneous mixture. (Chapter 3$)$
$$
\begin{array}{ll}{\text { a. air }} & {\text { d. ammonia }} \\ {\text { b. blood }} & {\text { e. mustard }} \\ {\text { c. antimony }} & {\text { f. water }}\end{array}
$$

Anna Miller
Anna Miller
Numerade Educator
00:55

Problem 102

You are given two clear, colorless aqueous solutions. You
are told that one solution contains an ionic compound,
and one contains a covalent compound. How could you
determine which is an ionic solution and which is a
covalent solution? (Chapter 8)

Anna Miller
Anna Miller
Numerade Educator
00:52

Problem 103

Which branch of chemistry would most likely study
matter and phase changes? (Chapter 1)
$$
\begin{array}{ll}{\text { a. biochemistry }} & {\text { c. physical chemistry }} \\ {\text { b. organic chemistry }} & {\text { d. polymer chemistry }}\end{array}
$$

Anna Miller
Anna Miller
Numerade Educator
01:29

Problem 104

What type of reaction is the following? (Chapter 9)
$$
\mathrm{K}_{2} \mathrm{CO}_{3}(\mathrm{aq})+\mathrm{BaCl}_{2}(\mathrm{aq}) \rightarrow 2 \mathrm{KCl}(\mathrm{aq})+\mathrm{BaCO}_{3}(\mathrm{s})
$$
$$
\begin{array}{ll}{\text { a. combustion }} & {\text { c. single-replacement }} \\ {\text { b. double-replacement }} & {\text { d. synthesis }}\end{array}
$$

Anna Miller
Anna Miller
Numerade Educator
00:20

Problem 105

Which chemist produced the first widely used and
accepted periodic table? (Chapter 6$)$
$$
\begin{array}{ll}{\text { a. Dmitri Mendeleev }} & {\text { c. John Newlands }} \\ {\text { b. Henry Moseley }} & {\text { d. Lothar Meyer }}\end{array}
$$

Anna Miller
Anna Miller
Numerade Educator
01:33

Problem 106

Musk is the basic ingredient of many perfumes,
soaps, shampoos, and even foods such as chocolates,
licorice, and hard candies. Both synthetic and natural
musk molecules have high molecular weights compared to other perfume ingredients, and as a result,
have a slower rate of diffusion, assuring a slow, sustained release of fragrance. Write a report on the
chemistry of perfume ingredients, emphasizing the
importance of diffusion rate as a property of perfume.

Anna Miller
Anna Miller
Numerade Educator
02:33

Problem 107

Birthstones Find out what your birthstone is and
write a brief report about the chemistry of that gem.
Find out its chemical composition, which category its
unit cell is in, how hard and durable it is, and what its
approximate cost is at present.

Caroline Basil
Caroline Basil
Numerade Educator
01:54

Problem 108

Propane gas is a commonly used heating fuel for gas
grills and homes. However, it is not packaged as a gas.
It is liquefied and referred to as liquid propane or
"LP gas." Make a poster explaining the advantages
and disadvantages of storing and transporting propane as a liquid rather than a gas.

Anna Miller
Anna Miller
Numerade Educator
03:23

Problem 109

Other States of Matter Research and prepare an oral
report about one of the following topics: plasma,
superfluids, fermionic condensate, or Bose-Einstein
condensate. Share your report with your classmates
and prepare a visual aid that can be used to explain
your topic.

Caroline Basil
Caroline Basil
Numerade Educator
04:21

Problem 110

Jodine Solid iodine that is left at room temperature subli-
mates from a solid to a gas. But when heated quickly, a
different process takes place, as described here.
"About 1 g of iodine crystals is placed in a sealed glass
ampoule and gently heated on a hot plate. A layer of purple
gas is formed at the bottom, and the iodine liquefies. If one
tilts the tube, this liquid flows along the wall as a narrow
stream and solidifies very quickly".
$$\begin{array}{l}{\text { Why does solid iodine sublime readily? Use your }} \\ {\text { knowledge of intermolecular forces to explain. }}\end{array}$$

Caroline Basil
Caroline Basil
Numerade Educator
02:53

Problem 111

Jodine Solid iodine that is left at room temperature subli-
mates from a solid to a gas. But when heated quickly, a
different process takes place, as described here.
"About 1 g of iodine crystals is placed in a sealed glass
ampoule and gently heated on a hot plate. A layer of purple
gas is formed at the bottom, and the iodine liquefies. If one
tilts the tube, this liquid flows along the wall as a narrow
stream and solidifies very quickly".
$$\begin{array}{l}{\text { Why is liquid iodine not usually visible if crystals are }} \\ {\text { heated in the open air? }}\end{array}$$

Caroline Basil
Caroline Basil
Numerade Educator
02:54

Problem 112

Jodine Solid iodine that is left at room temperature subli-
mates from a solid to a gas. But when heated quickly, a
different process takes place, as described here.
"About 1 g of iodine crystals is placed in a sealed glass
ampoule and gently heated on a hot plate. A layer of purple
gas is formed at the bottom, and the iodine liquefies. If one
tilts the tube, this liquid flows along the wall as a narrow
stream and solidifies very quickly".
$$\begin{array}{l}{\text { Why is it necessary to use a sealed ampoule in this }} \\ {\text { investigation? }}\end{array}$$

Caroline Basil
Caroline Basil
Numerade Educator
03:13

Problem 113

Jodine Solid iodine that is left at room temperature subli-
mates from a solid to a gas. But when heated quickly, a
different process takes place, as described here.
"About 1 g of iodine crystals is placed in a sealed glass
ampoule and gently heated on a hot plate. A layer of purple
gas is formed at the bottom, and the iodine liquefies. If one
tilts the tube, this liquid flows along the wall as a narrow
stream and solidifies very quickly".
$$\text{Infer why the iodine solidifies when the tube is tilted}.$$

Caroline Basil
Caroline Basil
Numerade Educator