Chapter 3 Matter and Energy

General, Organic, and Biological Chemistry: Structures of Life, 5/e

Karen C. Timberlake

© 2016 Pearson Education, Inc.

Karen C. Timberlake

Lecture Presentation

Chapter 3

Matter and Energy


Karen C. Timberlake


Matter

• is the material that

makes up all things.

• is anything that

has mass and

occupies space.

Learning Goal Classify examples of matter as pure

substances or mixtures.

3.1 Classification of Matter


Karen C. Timberlake


Matter is classified according to its composition.

• Pure substances have a fixed or definite

composition.

• Mixtures contain two or more different

substances that are physically mixed but not

chemically combined.

Core Chemistry Skill Classifying Matter

Matter: Pure Substances or Mixtures


Karen C. Timberlake


A pure substance is

classified as

• a type of matter with a fixed or

definite composition.

• an element that is composed

of one type of atom.

• a compound that is

composed of two or more

elements always combined in

the same proportion. An aluminum can

consists of many atoms

of aluminum.

Pure Substances:Elements and Compounds


Karen C. Timberlake


Elements are pure

substances that contain

only one type of atom,

such as the following:

• copper, Cu

• lead, Pb

• aluminum, Al

• There are 92

naturally occurring

elements The element copper

consists of copper atoms.

Elements


Karen C. Timberlake


A compound contains two

or more different elements

chemically bonded

together in a definite ratio,

such as the following:

• hydrogen peroxide (H2O2)

• table salt (NaCl)

• sugar (C12H22O11)

• water (H2O)

Compounds


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“Table salt” is a compound that contains the elements

sodium and chlorine.

The decomposition of salt, NaCl, produces the elements

sodium and chlorine.

Elements in a Compounds


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A mixture is a type of

matter that consists of

• two or more substances

that are physically mixed

but not chemically

combined.

• two or more substances

in different proportions.

• substances that can be

separated by physical

methods.

A mixture of a liquid

and a solid is separated

by filtration.

Mixtures


Karen C. Timberlake


In a homogeneous

mixture,

• the composition is

uniform throughout.

• the different parts of the

mixture are not visible.

Brass is a homogeneous mixture

of copper and zinc atoms.

Homogeneous Mixtures


Karen C. Timberlake


Breathing mixtures for scuba are

homogeneous mixtures. Some

examples are the following:

• nitrox (oxygen and nitrogen gases)

• heliox (oxygen and helium gases)

• trimix (oxygen, helium, and

nitrogen gases)

A nitrox mixture is used

to fill scuba tanks.

Chemistry Link to Health: Scuba Breathing

Mixtures


Karen C. Timberlake


In a heterogeneous mixture,

• the composition varies from

one part of the mixture to

another.

• the different parts of the

mixture are visible.

Copper metal and water form

a heterogeneous mixture.

Heterogeneous Mixtures


Karen C. Timberlake


Classification of Matter


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Identify each of the following as a pure substance

or mixture:

A. pasta and tomato sauce

B. aluminum foil

C. helium

D. air

Study Check


Karen C. Timberlake


Identify each of the following as a pure substance

or mixture:

A. pasta and tomato sauce mixture

B. aluminum foil pure substance

C. helium pure substance

D. air mixture

Solution


Karen C. Timberlake


Identify each of the following as a homogeneous or

heterogeneous mixture:

A. hot fudge sundae

B. shampoo

C. sugar water

D. peach pie

Study Check


Karen C. Timberlake


Identify each of the following as a homogeneous or

heterogeneous mixture:

A. hot fudge sundae heterogeneous mixture

B. shampoo homogeneous mixture

C. sugar water homogeneous mixture

D. peach pie heterogeneous mixture

Solution


Karen C. Timberlake


Learning Goal Identify the states and the physical and

chemical properties of matter.

The evaporation

of water from

seawater gives

white, solid

crystals of salt

called sodium

chloride.

3.2 States and Properties of Matter


Karen C. Timberlake


Solids have

• a definite shape.

• a definite volume.

• particles that are close

together in a fixed

arrangement.

• particles that move

very slowly.

A solid has a definite

shape and volume.

Amethyst, a solid, is a purple

form of quartz (SiO2).

Solids


Karen C. Timberlake


Liquids have

• an indefinite shape but a

definite volume.

• the same shape as their

container.

• particles that are close

together but mobile.


slowly.

A liquid has a definite

volume but takes the

shape of its container.

Liquids


Karen C. Timberlake


Gases have

• an indefinite shape.

• an indefinite volume.

• the same shape and

volume as their

container.

• particles that are far

apart.


very fast.

A gas takes the shape and

volume of its container.

Gases


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Comparison of Solids, Liquids, and Gases


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Identify each description as that of a solid, liquid, or gas.

A. It has definite volume but takes the shape of the

container.

B. Its particles are moving rapidly.

C. Its particles fill the entire volume of a container.

D. Its particles have a fixed arrangement.

E. Its particles are close together but moving randomly.

Study Check


Karen C. Timberlake


Identify each description as that of a solid, liquid, or gas.

A. It has definite volume but takes the shape of the

container. liquid

B. Its particles are moving rapidly. gas

C. Its particles fill the entire volume of a container. gas

D. Its particles have a fixed arrangement. solid

E. Its particles are close together but moving randomly. liquid

Solution


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Identify the state of matter for each of the following:

A. vitamin tablets

B. eye drops

C. vegetable oil

D. a candle

E. air in a tire

Study Check


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Identify the state of matter for each of the following:

A. vitamin tablets solid

B. eye drops liquid

C. vegetable oil liquid

D. a candle solid

E. air in a tire gas

Solution


Karen C. Timberlake


Physical properties

• are characteristics observed or measured without

changing the identity of a substance.

• include shape, physical state, boiling and freezing

points, density, and color of the substance.

Core Chemistry Skill Identifying Physical and Chemical

Changes

Physical Properties


Karen C. Timberlake


Copper has these physical

properties:

• reddish-orange color

• shiny

• excellent conductor of

heat and electricity

• solid at 25 °C

• melting point 1083 °C

• boiling point 2567 °C

Copper, used in cookware, is

a good conductor of heat.

Physical Properties of Copper


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A physical change occurs

in a substance if there is

• a change in the state.

• a change in the physical

shape.

• no change in the identity

and composition of the

substance.

Physical Change

The evaporation of water from

seawater gives white, solid

crystals of salt called sodium

chloride.


Karen C. Timberlake


Examples of Physical Changes


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Classify each of the following as a change of state or

change of shape:

A. chopping a log into kindling wood

B. water boiling in a pot

C. ice cream melting

D. ice forming in a freezer

E. cutting dough into strips

Study Check


Karen C. Timberlake


Chemical properties describe the ability of

a substance

• to interact with other substances.

• to change into a new substance.

When a chemical change takes place, the original

substance is turned into one or more new

substances with new chemical and physical

properties.

Chemical Properties and Changes


Karen C. Timberlake


During a chemical change, a

new substance forms that has

• a new composition.

• new chemical properties.

• new physical properties.

Sugar caramelizing at a high

temperature is an example of a

chemical change.

Chemical Change

Flan has a topping of caramelized

sugar.


Karen C. Timberlake


Examples of Chemical Changes


Karen C. Timberlake


Classify each of the following properties as physical or

chemical:

A. Ice melts in the sun.

B. Copper is a shiny metal.

C. Paper can burn.

D. A silver knife can tarnish.

E. A magnet removes iron particles from a mixture.

Study Check


Karen C. Timberlake


Classify each of the following changes as physical or

chemical:

A. burning a candle

B. ice melting on the street

C. toasting a marshmallow

D. cutting a pizza

E. iron rusting in an old car

Study Check


Karen C. Timberlake


A digital ear

thermometer is used

to measure body

temperature.

Learning Goal Given a temperature, calculate a

corresponding temperature on another scale.

3.3 Temperature


Karen C. Timberlake


Temperature

• is a measure of how hot or cold

an object is compared to another

object.

• indicates the heat flow from the

object with a higher temperature

to the object with a lower

temperature.

• is measured using a thermometer.

Temperature


Karen C. Timberlake


The temperature scales are Fahrenheit (°F) and Celsius (°C).

• The temperature difference between boiling and freezing of water are divided into smaller units called degrees.

• On the Celsius scale, there are 100 degrees between the boiling and freezing points of water.

• On the Fahrenheit scale, there are 180 degrees between the boiling and freezing points of water.

Core Chemistry Skill Converting between Temperature

Scales

Temperature Scales


Karen C. Timberlake


Scientists have learned that the coldest

temperature possible is −273 °C. On the

Kelvin scale, this is called absolute zero

and is represented as 0 K.

The Kelvin scale has

• units called kelvins (K).

• no degree symbol in front of K

• no negative temperatures.

• the same size units as Celsius: 1 K = 1 °C.

Kelvin Temperature Scale


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A comparison of the

Fahrenheit, Celsius,

and Kelvin temperature

scales between the

freezing and boiling

points of water.

Temperature Scales


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A. What is the temperature at which water freezes?

1) 0 °F 2) 0 °C 3) 0 K

B. What is the temperature at which water boils?

1) 100 °F 2) 32 °F 3) 373 K

C. How many Celsius units are between the boiling and

freezing points of water?

1) 100 2) 180 3) 273

Study Check


Karen C. Timberlake


To convert temperatures between the Celsius and

Fahrenheit scales, we adjust for the size of the degrees.

There are

• 100 degrees Celsius between the freezing and boiling

points of water.

• 180 degrees Fahrenheit between the freezing and boiling

points of water.

Therefore, 180 degrees Fahrenheit = 100 degrees Celsius

Converting between °C and °F


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Adjusting for the different freezing points, 0 °C and 32 °F,

we can write temperature equations to convert between

Fahrenheit and Celsius temperatures.

Converting between °C and °F


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Guide to Calculating Temperature


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Example: A person with hypothermia has a body temperature of 34.8 °C. What is that temperature in degrees Fahrenheit?

STEP 1 State given and needed quantities.

STEP 2 Write a temperature equation.

ANALYZE Given Need

THE PROBLEM 34.8 °C T in °F

TF = 1.8TC + 32

Solving a Temperature Problem


Karen C. Timberlake


Example: A person with hypothermia has a body temperature of 34.8 °C. What is that temperature in degrees Fahrenheit?

STEP 3 Substitute in the known values and calculate the

new temperature.

Three SFs Exact

TF = 62.6 + 32 = 94.6 °F

Answer to the tenths place

TF = 1.8(34.8) + 32 1.8 is exact; 32 is exact

Solving a Temperature Problem


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Temperature Comparison


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On a cold winter day, the temperature is –15 °F. What is that

temperature in degrees Celsius?

A. −85 °C

B. −47 °C

C. −42 °C

D. −26 °C

Study Check


Karen C. Timberlake


What is the normal body temperature, 37 °C, in kelvins?

A. 236 K

B. 310. K

C. 342 K

D. 98.0 K

Study Check


Karen C. Timberlake


Energy

• makes objects move.

• makes things stop.

• is defined as the ability

to do work.

Learning Goal Identify energy as potential or kinetic;

convert between units of energy.

A defibrillator provides electrical

energy to heart muscle to re-

establish normal rhythm.

3.4 Energy


Karen C. Timberlake


Kinetic energy is the

energy of motion.

Examples are the

following:

• swimming

• water flowing over

a dam

• working out

The movement of water that flows from the

top of a dam is an example of kinetic energy.

Kinetic Energy


Karen C. Timberlake


Potential energy is energy stored for use at a later time.

Examples are the following:

• water at the top of a dam

• a compressed spring

• chemical bonds in gasoline, coal, or food

The water at the top of a dam has potential energy by

virtue of its position. As the water falls over and down the

dam, the potential energy is converted to kinetic energy.

Potential Energy


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Identify the energy in each example as potential or kinetic:

A. rollerblading

B. a peanut butter and jelly sandwich

C. mowing the lawn

D. gasoline in the gas tank

Study Check


Karen C. Timberlake


Heat is the energy associated with the movement of particles.

The faster the particles move, the greater the heat or thermal

energy of the substance.

Given an ice cube, as heat is added, the H2O molecules

• that are moving slowly increase their motion.

• eventually have enough energy to change the ice cube

from a solid to a liquid.

Core Chemistry Skill Using Energy Units

Heat and Energy


Karen C. Timberlake


Energy is measured in

• the SI unit, the joule (J), or in kilojoules (kJ), 1000 joules.

• units of calories (cal) or in kilocalories (kcal), 1000 calories.

The calorie is defined as the amount of energy needed to raise

the temperature of 1 g of water by 1 °C.

Units of Energy


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Energy Comparison


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How many calories are obtained from a pat of butter if it

provides 150 J of energy when metabolized?

A. 0.86 cal

B. 630 cal

C. 36 cal

Study Check


Karen C. Timberlake





STEP 2 Write a plan to convert the given unit to the

needed unit.

joules calories

ANALYZE Given Need

THE PROBLEM 150 J calories

Energy

Factor

Solution


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STEP 3 State the equalities and conversion factors.

Solution


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STEP 4 Set up the problem to calculate the needed

quantity.

Answer is C.

Solution

×


Karen C. Timberlake


Learning Goal Use the energy values to calculate the

kilocalories (kcal) or kilojoules (kJ) for a food.

One hour of swimming

uses 2100 kJ of energy.

3.5 Energy and Nutrition


Karen C. Timberlake


Nutritionists burn food in a calorimeter that

• is used to measure heat transfer.

• consists of a steel container filled with oxygen and a

measured amount of water.

• indicates the heat gained by water, which is the heat lost by

a sample during combustion.

In a calorimeter, the burning of a food sample increases the

temperature of the water, which is used to calculate the

energy value of the food.

Calorimeters


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Heat released

from burning a

food sample in a

calorimeter is

used to determine

the energy value

for the food.

Calorimeters Measure Energy Values


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On food labels, energy is

shown as the nutritional

Calorie, written with a capital

C. In countries other than the

United States, energy is

shown in kilojoules (kJ).

1 Cal = 1000 calories

1 Cal = 1 kcal

Energy and Nutrition


Karen C. Timberlake


The caloric or energy

value for 1 g of a food

is given in kilojoules (kJ)

or kilocalories (kcal).

The typical energy

values are different for

each food type.

Caloric Food Values


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Energy Values for Some Foods


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Guide to Calculating Energy from Food


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A cup of whole milk contains 13 g of carbohydrate, 9.0 g of

fat, and 9.0 g of protein. How many kilocalories does a cup

of whole milk contain? (Round the final answer to the

tens place.)

A. 50 kcal

B. 80 kcal

C. 170 kcal

Study Check


Karen C. Timberlake




of whole milk contain?


ANALYZE Given Need

THE PROBLEM 13 g carbohydrate

9.0 g fat

9.0 g protein kilocalories

Solution


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STEP 2 Use the energy value for each food type

and calculate kJ or kcal rounded off to the

tens place.

13 g carbohydrate × 4 kcal/g = 50 kcal

9.0 g fat × 9 kcal/g = 80 kcal

9.0 g protein × 4 kcal/g = 40 kcal

Solution


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STEP 3 Add the energy for each food type to give

the total energy from the food.

Total energy = 50 kcal + 80 kcal + 40 kcal = 170 kcal

Solution


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The number of kilocalories

or kilojoules needed in the

daily diet of an adult

depends on gender, age,

and level of physical

activity.

A person loses weight

when food intake is less

than energy output.

Chemistry Link to Health: Weight Loss


Karen C. Timberlake


Learning Goal Use specific heat to calculate heat loss

or gain.

The high specific

heat of water keeps

temperature more

moderate in summer

and winter.

3.6 Specific Heat


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Specific heat (SH)

• is different for different substances.

• is the amount of heat that raises the temperature of exactly

1 g of a substance by exactly 1 °C.

• has units of J/g °C in the SI system and units of cal/g °C in

the metric system.

Specific Heat

×


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Specific Heats of Some Substances


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1. When ocean water cools, the surrounding air

B. warms.

2. Sand in the desert is hot in the day and cool at night.

Sand must have a

B. low specific heat.

Solution


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When we know the specific heat of a substance, we can

• calculate the heat lost or gained, by measuring its mass

and temperature change.

• write a heat equation.

Core Chemistry Skill Using the Heat Equation

Calculations Using Specific Heat


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Guide to Calculations Using Specific Heat


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What is the specific heat if 24.8 g of a metal absorbs 275 J of

energy and the temperature rises from 20.2 °C to 24.5 °C?

Study Check


Karen C. Timberlake


Learning Goal Describe the changes of state between

solids, liquids, and gases; calculate the energy involved.

Matter undergoes a

change of state

when it is converted

from one state to

another state.

3.7 Changes of State


Karen C. Timberlake


A substance

• is melting while it changes from a solid to a liquid at

its melting point (mp).

• is freezing while it changes from a liquid to a solid at

its freezing point (fp).

• Water has a freezing (melting) point of 0 °C.

Melting and freezing are reversible processes.

Melting and Freezing


Karen C. Timberlake


The heat of fusion

• is the amount of heat released when 1 g of liquid freezes

(at its freezing point).

• is the amount of heat needed to melt 1 g of solid (at its

melting point).

For a given amount of substance,

heat released during freezing = heat needed during melting

Heat of Fusion


Karen C. Timberlake


Heat of Fusion for Water

• To melt water,

H2O(s) + 80. cal/g (or 334 J/g) H2O(l)

• To freeze water,

H2O(l) H2O(s) + 80. cal/g (or 334 J/g)

Heat of Fusion


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Guide to Calculations Using a Heat Conversion Factor


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How many joules are needed to melt 32.0 g of ice at 0 °C?

Study Check


Karen C. Timberlake




STEP 2 Write a plan to convert the given quantity to

the needed quantity.

grams of H2O(s) joules (to melt)

ANALYZE Given Need

THE PROBLEM 32.0 g ice

0 °C joules to melt ice

Heat of

Fusion

Solution


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STEP 3 Write the heat conversion factor and any

metric factor.

1 g of H2O (s l) = 334 J

Solution


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STEP 4 Set up the problem and calculate the needed

quantity.

Solution

×


Karen C. Timberlake


Water

• evaporates when molecules

on the surface gain sufficient

energy to form a gas.

• condenses when gas

molecules lose energy and

form a liquid.

During evaporation, molecules

of the liquid are converted to

gas at the surface of the liquid.

Evaporation, Boiling, and Condensation


Karen C. Timberlake


When water is boiling,

• all the water molecules

acquire enough energy to

form a gas (vaporize).

• bubbles of water vapor

appear throughout the liquid.

During boiling, molecules of the

liquid are converted to gas

throughout the liquid as well as

at the surface.

Boiling Water


Karen C. Timberlake


When sublimation occurs,

• the particles on the surface of the solid change directly to a vapor.

• there is no change in temperature.

When deposition occurs, gas particles change directly to a solid.

• Dry ice undergoes sublimation at –78 °C.

Sublimation and deposition are

reversible processes.

Dry ice sublimes at –78 °C.

Sublimation and Deposition


Karen C. Timberlake


Sublimation is used to prepare freeze-dried foods for long-term storage.

Water vapor will change to solid on contact with a cold surface.

Freeze-dried foods have a long shelf life because they contain no water.

Sublimation and Deposition


Karen C. Timberlake


The heat of vaporization is the amount of heat

• absorbed to change 1 g of liquid to gas at the boiling point.

• released when 1 g of gas changes to liquid at the boiling point.

Vaporization and condensation

are reversible processes.

Heat of Vaporization


Karen C. Timberlake


• The heat of vaporization for water (boiling point 100 °C)

is the heat absorbed when 1 g of water changes to

steam.

H2O(l) + 540 cal/g (or 2260 J/g) H2O(g)

• The heat of condensation for water is the heat released when 1 g of steam changes to water.

H2O(g) H2O(l) + 540 cal/g (or 2260 J/g)

Heat of Vaporization


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How many kilojoules (kJ) are released when 50.0 g of steam

from a volcano condenses at 100 °C?

Study Check


Karen C. Timberlake







grams joules kilojoules of H2O(g)

ANALYZE Given Need

THE PROBLEM 50.0 g steam

100 °C kilojoules released

Heat of

Condensation

Metric

Factor

Solution


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metric factor.


quantity.

1 g of H2O (g l) = 2260 J 103 J = 1 kJ

Solution

× ×


Karen C. Timberlake


On a heating curve, diagonal lines indicate changes in

temperature for a physical state, and horizontal lines

(plateaus) indicate changes of state.

A heating curve diagrams

the temperature increases

and changes of state as

heat is added.

Heating and Cooling Curves


Karen C. Timberlake


1. A plateau (horizontal line) on a heating curve represents

A. a temperature change.

B. a constant temperature.

C. a change of state.

2. A sloped line on a heating curve represents




Study Check


Karen C. Timberlake


1. A plateau (horizontal line) on a heating curve represents



2. A sloped line on a heating curve represents


Solution


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Use the cooling curve for water to answer each of the following:

1. Water condenses at a temperature of

A. 0 °C. B. 50 °C. C. 100 °C.

2. At a temperature of 0 °C, liquid water

A. freezes. B. melts. C. changes to a gas.

3. At 40 °C, water is a

A. solid. B. liquid. C. gas.

4. When water freezes, heat is

A. removed. B. added.

Study Check


Karen C. Timberlake


Use the cooling curve for water to answer each of the following:

1. Water condenses at a temperature of

C. 100 °C.

2. At a temperature of 0 °C, liquid water

A. freezes.

3. At 40 °C, water is a

B. liquid.

4. When water freezes, heat is

A. removed.

Solution


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A cooling curve for

water illustrates the

change in temperature

and changes of state

as heat is removed.

Steps on a Cooling Curve


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Calculate the total heat, in joules, needed to convert 15.0 g

of liquid ethanol at 25.0 °C to gas at its boiling point of

78.0 °C. Ethanol has a specific heat of 2.46 J/g °C and a

heat of vaporization of 841 J/g.

STEP 1 State the given and needed quantities.

ANALYZE Given Need

THE PROBLEM 15.0 g ethanol

Tinitial = 25.0 °C

Tfinal = 78.0 °C kilojoules

heat vaporization, 841 J/g released

specific heat, 2.46 J/ g °C

Combining Heat Calculations


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Total heat = joules needed to warm ethanol

(25.0 °C to 78.0 °C)

+ joules to change liquid to gas at 78.0 °C

Combined Heat Calculations


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metric factor.



Karen C. Timberlake



quantity.

Calculate the temperature change of the liquid.

ΔT = 78.0 °C − 25.0 °C = 53.0 °C

Calculate heat needed to warm ethanol.


× × × ×


Karen C. Timberlake



quantity.

Calculate the heat needed to vaporize ethanol.

Calculate the total energy needed.

Heating ethanol (25.0 °C to 78.0 °C) = 1 960 J

Changing liquid to gas = 12 600 J

Total heat needed = 14 600 J


×


Karen C. Timberlake


When a volcano erupts, 175 g of steam at 100.0 °C is

released. How many kilojoules are lost when the steam

condenses, then freezes, at 0.0 °C?

A. 396 kJ

B. 528 kJ

C. 133 kJ

Study Check


Karen C. Timberlake


When a volcano erupts, 175 g of steam at 100.0 °C is

released. How many kilojoules are lost when the steam

condenses, then freezes, at 0.0 °C?

STEP 1 State the given and needed quantities.

ANALYZE Given Need

THE PROBLEM 175 g steam at 100.0 °C

ice, at 0.0 °C kilojoules

heat vaporization, 2260 J/g released

specific heat, 4.184 J/ g °C

heat fusion, 334 J/g

Solution


Karen C. Timberlake


STEP 2 Write a plan to convert the given quantity to the

needed quantity.

Use the cooling curve to determine kilojoules released.

100.0 °C

0.0 °C

Steam at 100.0 °C

condenses to liquid

Liquid cools to 0.0 °C

Liquid turns to solid at 0.0 °C

Solution


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metric factor.

Solution


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quantity.

Calculate the heat released as steam is condensed.

Calculate the temperature change of the liquid.

ΔT = 100.0 °C − 0.0 °C = 100.0 °C

Solution

×


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quantity.

Calculate the heat released as the liquid is cooled.

Calculate the heat released as the liquid freezes.

Solution

×

×

×


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quantity.

Calculate the total energy needed.

Heat released as steam is condensed = 396 000 J

Heat released as liquid is cooled = 73 200 J

Heat released as liquid freezes = 58 500 J

Total heat needed = 528 000 J

Answer is B.

Solution

×


Karen C. Timberlake


Concept Map

Documents

Chapter 3 Matter and Energy