C HAPTER 1 The Foundations of Chemistry. What is Chemistry? Physical science that studies the composition, structure, and properties of matter and the

CHAPTER 1CHAPTER 1

The Foundations of ChemistryThe Foundations of Chemistry

What is Chemistry?What is Chemistry? Physical science that studies the composition, Physical science that studies the composition,

structure, and properties of matter and the structure, and properties of matter and the changes it undergoeschanges it undergoes Includes many different branches of study (focuses Includes many different branches of study (focuses

on a particular area, they do overlap)on a particular area, they do overlap) OrganicOrganic InorganicInorganic PhysicalPhysical AnalyticalAnalytical BiochemistryBiochemistry TheoreticalTheoretical

Chemistry is……Chemistry is……

A natural scienceA natural science A language with its A language with its

own vocabularyown vocabulary A way of thinkingA way of thinking

Click below to watch the Visual Concept.

Visual Concept

Chapter 1 ChemistryChemistry

Prediction

Experiment

Modify

Observations

Hypothesis

Experiment

Law

Theory(Model)

Scientific Method

What is Matter?What is Matter?

Matter is anything that takes up space and Matter is anything that takes up space and has masshas mass

Mass is the amount of matter in an objectMass is the amount of matter in an object Mass is resistance to change in motion Mass is resistance to change in motion

along a smooth and level surfacealong a smooth and level surface

MatterMatter

Atoms are the building Atoms are the building blocks of all matterblocks of all matter

An An atomatom is the smallest is the smallest particle of an element that particle of an element that maintains its chemical maintains its chemical identity through all identity through all chemical and physical chemical and physical changes.changes.

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Properties of MatterProperties of Matter

Physical properties-Physical propertiescharacteristic that can characteristic that can be observed without be observed without changing the identitychanging the identity Observed with the Observed with the

sensessenses Changes of stateChanges of state Density, color solubilityDensity, color solubility

Chemical properties-Chemical properties- indicates how a indicates how a substance reacts with substance reacts with something elsesomething else When observed original When observed original

substance is changedsubstance is changed Rusting or oxidationRusting or oxidation Chemical RxnChemical Rxn

Properties of MatterProperties of Matter


Visual Concept

Chapter 1Comparing Physical and Comparing Physical and Chemical PropertiesChemical Properties

Characteristic PropertiesCharacteristic Properties

Quality of a substance that Quality of a substance that never changes, used to identify never changes, used to identify substancesubstance

ExtensiveExtensive- depends on amount - depends on amount of matter presentof matter present MassMass volumevolume

IIntensiventensive- does not depend on - does not depend on amount of matter presentamount of matter present Melting pointMelting point Boiling pointBoiling point


Visual Concept

Chapter 1Comparing Extensive and Comparing Extensive and Intensive PropertiesIntensive Properties

Changes in MatterChanges in Matter

Physical change-Physical change- alter form of a alter form of a substance but NOT substance but NOT identityidentity Original substance Original substance

continues to existcontinues to exist

Chemical change-Chemical change- substances substances combine/break apart combine/break apart to form new to form new substancesubstance Original substance no Original substance no

longer existslonger exists

Chemical Changes, Chemical Changes, continuedcontinued

• The products are the substances that are formed by the

chemical change.

reactants product

• A change in which one or more substances are

converted into different substances is called a chemical

change or chemical reactionchemical reaction.

• The reactants are the substances that react in a

chemical change.

Carbon plus oxygen yields (or forms) carbon dioxide.

carbon + oxygen carbon dioxide

Evidence of a Chemical ChangeEvidence of a Chemical Change

Chapter 1


Chapter 1Chemical ReactionChemical Reaction

Visual Concept


Visual Concept

Chapter 1Comparing Chemical and Comparing Chemical and Physical ChangesPhysical Changes

Physical vs. ChemicalPhysical vs. Chemical

Examples:Examples:

rusting ironrusting iron

dissolving in waterdissolving in water

burning a logburning a log

melting icemelting ice

grinding spicesgrinding spices

chemical

physical

chemical

physical

physical

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Mixtures, Substances, Mixtures, Substances, Compounds, & ElementsCompounds, & Elements

SubstanceSubstance matter in which all samples have identical matter in which all samples have identical

composition and propertiescomposition and properties ElementsElements

substances that cannot be decomposed into substances that cannot be decomposed into simpler substances via chemical reactionssimpler substances via chemical reactions

Elemental symbolsElemental symbols found on periodic tablefound on periodic table


Visual Concept

Chapter 1ElementElement

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Mixtures, Substances, Mixtures, Substances, Compounds, & ElementsCompounds, & Elements

MixturesMixtures composed of two or more substances can be separated by composed of two or more substances can be separated by

physical meansphysical means homogeneous mixtureshomogeneous mixtures heterogeneous mixturesheterogeneous mixtures

CompoundsCompounds substances composed of two or more elements in a substances composed of two or more elements in a

definite ratio by massdefinite ratio by mass can be decomposed into the constituent elements by can be decomposed into the constituent elements by

chemical meanschemical means Water is a compound that can be decomposed into Water is a compound that can be decomposed into

simpler substances – hydrogen and oxygensimpler substances – hydrogen and oxygen


Visual Concept

Chapter 1 CompoundsCompounds


Visual Concept

Chapter 1Classification Scheme for Classification Scheme for MatterMatter

States of MatterStates of Matter

SolidsSolids Particles packed Particles packed

tightly togethertightly together Have definite volume Have definite volume

and definite shapeand definite shape Particles vibrateParticles vibrate

GasesGases Change volume very Change volume very

easilyeasily Particles spread apart, Particles spread apart,

filling all space available filling all space available to themto them

No definite shape nor No definite shape nor volumevolume

LiquidsLiquids No shape of its own, No shape of its own,

takes shape of its takes shape of its containercontainer

Has definite volumeHas definite volume

© 2009, Prentice-Hall, Inc.© 2009, Prentice-Hall, Inc.



Chapter 1LiquidLiquid

Section 2 Matter and Its Properties

Visual Concept

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Changes in state require Changes in state require changes in energy.changes in energy. heatingheating coolingcooling


Solid

Liquid

Gas

Definite Volume?

YES

YES

NO

Definite Shape?

YES

NO

NO

Temp. increase

Small Expans.

Small Expans.

Large Expans.

Compressible?

NO

NO

YES

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A Molecular ViewA Molecular ViewDaltonDalton’’s Atomic Theorys Atomic Theory

DaltonDalton’’s atomic theory summarized the nature of s atomic theory summarized the nature of matter as known in 1808matter as known in 1808

1)1) An element is composed of extremely small indivisible An element is composed of extremely small indivisible particles called atoms.particles called atoms.

2)2) All atoms of a given element have identical properties, All atoms of a given element have identical properties, which differ from those of other elements.which differ from those of other elements.

3)3) Atoms cannot be created, destroyed, or transformed into Atoms cannot be created, destroyed, or transformed into atoms of another element.atoms of another element.

4)4) Compounds are formed when atoms of different Compounds are formed when atoms of different elements combine with each other in small whole-elements combine with each other in small whole-number ratios.number ratios.

5)5) The relative numbers and kinds of atoms are constant in The relative numbers and kinds of atoms are constant in a given compound.a given compound.

Natural LawsNatural Laws

Scientific (natural) lawScientific (natural) law A general statement based the A general statement based the

observed behavior of matter to observed behavior of matter to which no exceptions are known.which no exceptions are known.

Law of Conservation of MassLaw of Conservation of Mass Law of Conservation of EnergyLaw of Conservation of Energy Law of Conservation of Mass Law of Conservation of Mass

and Energyand Energy Einstein’s Theory of Einstein’s Theory of

RelativityRelativity E=mcE=mc22

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Number vs. QuantityNumber vs. Quantity Quantity = number + unitQuantity = number + unit

UNITS MATTER!!

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Measurements in ChemistryMeasurements in Chemistry

QuantityQuantity UnitUnit SymbolSymbol lengthlength meter meter m m massmass kilogram kilogram kg kg timetime second second s s currentcurrent ampere ampere A A temperaturetemperature Kelvin Kelvin K K amt. substanceamt. substance mole mole mol mol

Measurements in ChemistryMeasurements in ChemistryMetric PrefixesMetric Prefixes

mega- M 106

deci- d 10-1

centi- c 10-2

milli- m 10-3

Prefix Symbol Factor

micro- 10-6

nano- n 10-9

pico- p 10-12

kilo- k 103

BASE UNIT --- 100

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Units of MeasurementUnits of Measurement

DefinitionsDefinitions Mass Mass

measure of the quantity of matter in a measure of the quantity of matter in a bodybody

WeightWeight measure of the gravitational attraction measure of the gravitational attraction

for a body for a body

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Units of MeasurementUnits of Measurement

Common Conversion FactorsCommon Conversion Factors Length Length

1 m = 39.37 inches1 m = 39.37 inches 2.54 cm = 1 inch2.54 cm = 1 inch

VolumeVolume 1 liter = 1.06 qt 1 liter = 1.06 qt 1 qt = 0.946 liter1 qt = 0.946 liter

See Table 1-8 for more conversion factorsSee Table 1-8 for more conversion factors

Use of NumbersUse of Numbers

Exact numbersExact numbers 1 dozen = 12 things1 dozen = 12 things

Accuracy Accuracy how closely measured how closely measured

values agree with the values agree with the correct valuecorrect value

PrecisionPrecision how closely individual how closely individual

measurements agree measurements agree with each otherwith each other

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Visual Concept

Accuracy and PrecisionAccuracy and Precision

Significant FiguresSignificant Figures

Indicate precision of a measurement.Indicate precision of a measurement. Consists of all the digits known with Consists of all the digits known with

certainty plus one final digit, which is certainty plus one final digit, which is somewhat uncertain or estimatedsomewhat uncertain or estimated

2.35 cm

Significant Figures RulesSignificant Figures Rules

Counting Sig Figs Count all numbers Counting Sig Figs Count all numbers EXCEPT:EXCEPT:

Leading zeros -- Leading zeros -- 0.000.002525

Trailing zeros Trailing zeros without without a decimal point -- 2,5a decimal point -- 2,50000

Calculating with Significant FiguresCalculating with Significant Figures

Exact NumbersExact Numbers do not limit the # of sig figs do not limit the # of sig figs in the answer.in the answer.

Counting numbers: 12 studentsCounting numbers: 12 students

Exact conversions: 1 m = 100 cmExact conversions: 1 m = 100 cm

““1” in any conversion: 1 in = 2.54 cm1” in any conversion: 1 in = 2.54 cm

Significant Figures, Significant Figures, continuedcontinuedRoundingRounding

Counting Sig Fig ExamplesCounting Sig Fig Examples

4. 0.080

3. 5,280

2. 402

1. 23.501. 23.50

2. 402

3. 5,280

4. 0.080

4 sig figs

3 sig figs

3 sig figs

2 sig figs

Calculating with Significant Calculating with Significant FiguresFigures

Multiply/DivideMultiply/Divide - The # with the fewest - The # with the fewest sig figs determines the # of sig figs in sig figs determines the # of sig figs in the answer.the answer.

(13.91g/cm3)(23.3cm3) = 324.103g

324 g

4 SF 3 SF3 SF

Calculating with Significant Calculating with Significant FiguresFigures

Add/SubtractAdd/Subtract - The # with the lowest - The # with the lowest decimal value determines the place of decimal value determines the place of the last sig fig in the answer.the last sig fig in the answer.

3.75 mL

+ 4.1 mL

7.85 mL

224 g

+ 130 g

354 g 7.9 mL 350 g

3.75 mL

+ 4.1 mL

7.85 mL

224 g

+ 130 g

354 g

Practice ProblemsPractice Problems

(15.30 g) ÷ (6.4 mL)(15.30 g) ÷ (6.4 mL)

= 2.390625 g/mL

18.1 g

18.9 g

- 0.84 g18.06 g

4 SF 2 SF

2.4 g/mL2 SF

Introduction to the Periodic TableIntroduction to the Periodic Table

• The vertical columns vertical columns of the periodic table are called

groups, or familiesgroups, or families. • Each group contains elements with similar

chemical properties.

• The horizontal rows horizontal rows of elements in the periodic

table are called periodsperiods. • Physical and chemical properties change

somewhat regularly across a period.

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The Unit Factor MethodThe Unit Factor Method

Simple but important method to get correct Simple but important method to get correct answers in word problems.answers in word problems.

Method to change from one set of units to Method to change from one set of units to another.another.

Visual illustration of the idea.Visual illustration of the idea.

B. Dimensional AnalysisB. Dimensional Analysis

Steps:Steps:

1. Identify starting & ending units.1. Identify starting & ending units.

2. Line up conversion factors so units cancel.2. Line up conversion factors so units cancel.

3. Multiply all top numbers & divide by each 3. Multiply all top numbers & divide by each bottom number.bottom number.

4. Check units & answer.4. Check units & answer.

B. Dimensional AnalysisB. Dimensional Analysis

How many milliliters are in 1.00 quart of How many milliliters are in 1.00 quart of milk?milk?

1.00 qt 1 L

1.057 qt= 946 mL

qt mL

1000 mL

1 L

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Example 1-2: Express 627 milliliters in gallons.Example 1-2: Express 627 milliliters in gallons.

You do it!You do it!

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Example 1-2: Express 627 milliliters in gallons.Example 1-2: Express 627 milliliters in gallons.

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Example 1-3: Express 2.61 x 10Example 1-3: Express 2.61 x 1044 cm cm22 in ft in ft22. .

Area is two dimensional, thus units must be in Area is two dimensional, thus units must be in squared terms.squared terms.

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Example 1-3: Express 2.61 x 10Example 1-3: Express 2.61 x 1044 cm cm22 in ft in ft22. .

Area is two dimensional, thus units must be in Area is two dimensional, thus units must be in squared terms.squared terms.

Derived UnitsDerived Units

Combination of units.Combination of units. VolumeVolume amount of space occupied by an object amount of space occupied by an object

length length length length length length (m(m33 or cm or cm33) )

D = MV

1 cm3 = 1 mL1 dm3 = 1 L

Density (kg/m3 or g/cm3)mass per volume

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Density and Specific GravityDensity and Specific Gravity

density = mass/volume density = mass/volume D = M / VD = M / V How heavy something is for its size.How heavy something is for its size. The ratio of mass to volume for a substance.The ratio of mass to volume for a substance. Independent of how much of it you haveIndependent of how much of it you have gold - high densitygold - high density air low density.air low density.

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Example 1-6: Calculate the density of a Example 1-6: Calculate the density of a substance if 742 grams of it occupies 97.3 cmsubstance if 742 grams of it occupies 97.3 cm33..

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Example 1-6: Calculate the density of a Example 1-6: Calculate the density of a substance if 742 grams of it occupies 97.3 cmsubstance if 742 grams of it occupies 97.3 cm33..

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Example 1-7: Suppose you need 125 g of a Example 1-7: Suppose you need 125 g of a corrosive liquid for a reaction. What volume do corrosive liquid for a reaction. What volume do you need? (you need? (liquid’s density = 1.32 g/mL)liquid’s density = 1.32 g/mL)


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Example 1-7 Suppose you need 125 g of a Example 1-7 Suppose you need 125 g of a corrosive liquid for a reaction. What volume do corrosive liquid for a reaction. What volume do you need? (you need? (liquid’s density = 1.32 g/mL)liquid’s density = 1.32 g/mL)

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Water’s density is essentially 1.00 at room T.Water’s density is essentially 1.00 at room T. Thus the specific gravity of a substance is Thus the specific gravity of a substance is

very nearly equal to its density.very nearly equal to its density. Specific gravity has no units.Specific gravity has no units.

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Example 1-8: A 31.0 gram piece of chromium is Example 1-8: A 31.0 gram piece of chromium is dropped into a graduated cylinder that contains 5.00 dropped into a graduated cylinder that contains 5.00 mL of water. The water level rises to 9.32 mL. What mL of water. The water level rises to 9.32 mL. What is the specific gravity of chromium?is the specific gravity of chromium?

You do itYou do it

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Example 1-8: A 31.0 gram piece of chromium is Example 1-8: A 31.0 gram piece of chromium is dropped into a graduated cylinder that contains dropped into a graduated cylinder that contains 5.00 mL of water. The water level rises to 9.32 mL. 5.00 mL of water. The water level rises to 9.32 mL. What is the specific gravity of chromium? What is the specific gravity of chromium?

18.7

mLg

mLg

1.00

7.18Cr of Gravity Specific

mLg 7.18mL

g 7.17593

mL 4.32

g 31.0 Cr of density

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Example 1-9: A concentrated hydrochloric acid Example 1-9: A concentrated hydrochloric acid solution is 36.31% HCl and 63.69% water by mass. solution is 36.31% HCl and 63.69% water by mass. The specific gravity of the solution is 1.185. What The specific gravity of the solution is 1.185. What mass of pure HCl is contained in 175 mL of this mass of pure HCl is contained in 175 mL of this solution?solution?


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Example 1-9: A concentrated hydrochloric acid Example 1-9: A concentrated hydrochloric acid solution is 36.31% HCl and 63.69% water by mass. solution is 36.31% HCl and 63.69% water by mass. The specific gravity of the solution is 1.185. What The specific gravity of the solution is 1.185. What mass of pure HCl is contained in 175 mL of this mass of pure HCl is contained in 175 mL of this solution?solution?

Heat and TemperatureHeat and Temperature

Heat and Temperature Heat and Temperature are not the same thingare not the same thing

Temperature- measure Temperature- measure of the average kinetic of the average kinetic energyenergy Temperature is which Temperature is which

way heat will flow. (from way heat will flow. (from hot to cold)hot to cold)

3 common temperature 3 common temperature scales - all use water as scales - all use water as a referencea reference

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MP waterMP water BP waterBP water Fahrenheit Fahrenheit 32 32 ooF F 212 212 ooFF Celsius Celsius 0.0 0.0 ooC C 100 100 ooCC Kelvin Kelvin 273 K 273 K 373 K373 K

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Relationships of the Three Relationships of the Three Temperature ScalesTemperature Scales

100ºC 212ºF0ºC 32ºF

100ºC = 212ºF

0ºC = 32ºF

100ºC = 180ºF

How much it changes

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Easy method to remember how to convert Easy method to remember how to convert from Centigrade to Fahrenheit.from Centigrade to Fahrenheit.1.1.Double the Centigrade temperature.Double the Centigrade temperature.

2.2.Subtract 10% of the doubled number.Subtract 10% of the doubled number.

3.3.Add 32.Add 32.

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Example 1-10: Convert 211Example 1-10: Convert 211ooF to degrees Celsius.F to degrees Celsius.

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Example 1-10: Convert 211Example 1-10: Convert 211ooF to degrees Celsius.F to degrees Celsius.

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Example 1-11: Express 548 K in Celsius degrees.Example 1-11: Express 548 K in Celsius degrees.

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Example 1-11: Express 548 K in Celsius degrees.Example 1-11: Express 548 K in Celsius degrees.

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Heat Transfer and the Heat Transfer and the Measurement of HeatMeasurement of Heat

HeatHeat is energy, ability to do work. is energy, ability to do work. SI unit J (Joule)SI unit J (Joule) caloriecalorie

Amount of heat required to heat 1 g of water 1 Amount of heat required to heat 1 g of water 1 ooCC1 calorie = 4.184 J1 calorie = 4.184 J

CalorieCalorieLarge calorie, kilocalorie, dietetic caloriesLarge calorie, kilocalorie, dietetic caloriesAmount of heat required to heat 1 kg of water 1 Amount of heat required to heat 1 kg of water 1 ooCC

English unit = BTUEnglish unit = BTU Specific HeatSpecific Heat

amount of heat required to raise the T of 1g of a substance by amount of heat required to raise the T of 1g of a substance by 11ooC C

unit = J/gunit = J/gooCC

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Heat capacityHeat capacityamount of heat required to raise the T of 1 mole amount of heat required to raise the T of 1 mole

of a substance by 1of a substance by 1ooC C unit = J/mol unit = J/mol ooCC

Heat transfer equationHeat transfer equationnecessary to calculate amounts of heatnecessary to calculate amounts of heat

amount of heat = amount of substance x amount of heat = amount of substance x specific heat x specific heat x TT

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Example 1-12: Calculate the amt. of heat to Example 1-12: Calculate the amt. of heat to raise T of 200.0 g of water from 10.0raise T of 200.0 g of water from 10.0ooC to C to 55.055.0ooCC

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Example 1-12: Calculate the amt. of heat to Example 1-12: Calculate the amt. of heat to raise T of 200.0 g of water from 10.0raise T of 200.0 g of water from 10.0ooC to C to 55.055.0ooCC

kJ 37.6 or J 103.76

C)10.0C(55.0 COH g 1

J 4.184OH g 200J ?

T C mq

4

ooo

22

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Example 1-13: Calculate the amount of heat to Example 1-13: Calculate the amount of heat to raise the temperature of 200.0 grams of mercury raise the temperature of 200.0 grams of mercury from 10.0from 10.0ooC to 55.0C to 55.0ooC. Specific heat for Hg is C. Specific heat for Hg is 0.138 J/g 0.138 J/g ooC.C.


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Example 1-13: Calculate the amount of heat to Example 1-13: Calculate the amount of heat to raise the temperature of 200.0 grams of mercury raise the temperature of 200.0 grams of mercury from 10.0from 10.0ooC to 55.0C to 55.0ooC. Specific heat for Hg is C. Specific heat for Hg is 0.138 J/g 0.138 J/g ooC.C.

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Heating Curve for 3 SubstancesHeating Curve for 3 Substances

Heating Curve

0

20

40

60

80

100

120

140

0 50 100 150 200 250 300

Tim e (s)

Tem

per

atu

re (

cels

ius

deg

ree)

Substance 1

Substance 2

Substance 3

Which substance has the largest specific heat?Which

substance’s T will decrease the most after the heat has been removed?

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Heating Curve for 3 SubstancesHeating Curve for 3 Substances

Heating Curve

020406080

100120140

0 200 400 600

Time (s)

Tem

per

atu

re (

deg

C)

Substance 1

Substance 2

Substance 3

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Synthesis QuestionSynthesis Question

It has been estimated that 1.0 g of seawater It has been estimated that 1.0 g of seawater contains 4.0 pg of Au. The total mass of contains 4.0 pg of Au. The total mass of seawater in the oceans is 1.6x10seawater in the oceans is 1.6x101212 Tg, If all of Tg, If all of the gold in the oceans were extracted and the gold in the oceans were extracted and spread evenly across the state of Georgia, spread evenly across the state of Georgia, which has a land area of 58,910 milewhich has a land area of 58,910 mile22, how tall, , how tall, in feet, would the pile of Au be?in feet, would the pile of Au be?Density of Au is 19.3 g/cmDensity of Au is 19.3 g/cm33. 1.0 Tg = 10. 1.0 Tg = 101212g. g.

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Documents

C HAPTER 1 The Foundations of Chemistry. What is Chemistry? Physical science that studies the composition, structure, and properties of matter and the