During Class Inventions and Computer Lab Activitiesgenchem1.chem.okstate.edu/APCHEMSITE/Vol2DCI_Workbook.pdfDuring Class Inventions and Computer Lab Activities GENERAL CHEMISTRY Volume

During Class Inventions and Computer Lab Activities

GE

NE

RA

L C

HE

MIS

TR

Y

Volume II

3RD EDITION

NOT FOR DISTRIBUTION - FOR INSTRCTORS USE ONLY

During Class Inventions and Computer Lab Activities

iii

TABLE OF CONTENTS

During Class Inventions

Kinetics . . . . . . . . . . . . . . . . . . . . . . . . . . . . 1 . . . . . . . . . . . . . .1

. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

. . . . . . . . . .

. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

Equilibrium . . . . . . . . . . . . . . . . . . . . . . . 27 . . . . . . . . . . . . . . . .

. . . . . . . . . . . . . . . . . .

. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

. . .

. . . . . . . . . . . .

Acids and Bases . . . . . . . . . . . . . . . . . . . . 49+ –

. . . . . . . . . . . . . . . . . . . . . . . . . .

. . . . . . . . . . . . . . . .

. . . . . . . . . . . .

. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

Aqueous Equilibrium . . . . . . . . . . . . . . . . 69 . . . . . . . . . . . . . . . . . . . . . . . .

. . . . . . . . . . . . . . .

. . . . . . . . . . . . . . . . . . . . . . . . . . . . .

. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

. . . . . . . .

Thermodynamics . . . . . . . . . . . . . . . . . . . 91 . . . . . . . . . .

. . . . . . . . . . . . . . . . . . . . .

. . . . . . . . . . .

Electrochemistry . . . . . . . . . . . . . . . . . . 105 .

. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

Computer Lab Activities

MoLEs . . . . . . . . . . . . . . . . . . . . . . . . . . 125 . . . . .

. . . . . . . . . . . . . . . . . . . . . . . . . . .

. . .


DURING CLASS INVENTIONS AND COMPUTER LAB ACTIVITIES

iv

. . . . . . . . . . . . . . . . . . . . . . . . . .

. . . . . . . . . . . . . .

. . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

. . . . . . . . . . . . . . . . . . . . . . . .

. . . .

. . . . . . . . . . . . . . . . . . . . . . .

. . . . . . . . . . . . . . . . . .

. . . . . . . .

Laboratory Simulations . . . . . . . . . . . . . . .239

. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

. . . . . . . . . . . . . . . . . .

. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

. . . . . . . . . . . . . . . . . . . . . . . . . . . .

. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .


During Class Inventions*

GE

NE

RA

L C

HE

MIS

TR

Y

Kinetics

Equilibrium

Acids and Bases+ –

Aqueous Equilibrium

Thermodynamics

Electrochemistry


Name Section

1

reaction rate.

(g) → (g) � (g)

I N T R O D U C T I O N T O K I N E T I C S


DURING CLASS INVENTIONS · KINETICS

2

average rate instantaneous rate, initial rate

Co

nce

ntr

atio

n (

M)

Time (minutes)

A

B

C

00

0.05

0.10

0.15

0.20

0.25

0.30

0.35

0.40

5 10 15 20 25 30 35 40 45


Name Section

3

Time (min)Exp. #1

[NO2] (M)Exp. #2

[NO2] (M)

(g) → (g) � (g)

Co

nce

ntr

atio

n (

M)

Time (minutes)

00

0.05

0.10

0.15

0.20

0.25

0.30

0.35

0.40

5 10 15 20 25 30 35 40 45

R A T E S O F R E A C T I O N



4

Co

nce

ntr

atio

n (

M)

Time (minutes)

00

0.2

0.4

0.6

0.8

1.0

1.2

5 10 15 20 25 30


Name Section

5

rate expression rate law

(g) � Cl (g) → (g)

M E T H O D O F I N I T I A L R A T E S



6

(g) � (g) → (g) � (g)

Experiment Number PNO

(mmHg) PH2(mmHg)Initial Rate mmHg

s

⎛⎝⎜

⎞⎠⎟

1

.


7

(g) � (g) → (g)

Exp. [NO2] [F2] Initial Rate (M/sec)

1 � �

� �

� �

.

METHOD OF INITIAL RATES



8 NOT FOR DISTRIBUTION - FOR INSTRCTORS USE ONLY

Name Section

9

(g) →

× � �1

�1

(l) → (l) � (g)

]

I N T E G R A T E D R A T E L A W P A R T I



10

� � � �

ln

(g) → (g) � (g)

Time (sec) [N2O5] (M)

� �

� �

� �

� �

� �

� �


11

INTEGRATED RATE LAW PART 1


Name Section

13

A(g) →

�

H A L F - L I F E



14

–1

(l) → (l) � (g)


Name Section

15

(g) →

� � �1

(g)

(g) → (g) � Cl (g)

�1 �1

I N T E G R A T E D R A T E L A W P A R T I I



16

(g)

ln


17

(g) → (g) � (g)

Time (sec) [NO2] (M)

INTEGRATED RATE LAW PART II


Name Section

19

(g) � (g) → (g) � (g)

Temperature (K) 1/T k (M�1·sec�1) ln k

ln y1

temperaturex

T E M P E R AT U R E D E P E N D E N C E O F T H E R AT E C O N S TA N T



20

activation energy.

CH2

CH2CH2

H2C=CH-CH3

� � �1 � � �1


21

� kJ

mol

(g) � (g) → (g) � (g)

TEMPERATURE DEPENDENCE OF THE RATE CONSTANT


Name Section

23

R � → �

ExperimentNumber

R (M) BG (M) Initial Rate (M) s

1 � 1

� 1

� 1

R E A C T I O N M E C H A N I S M S



24

reaction mechanism.

� →

�


25

(g) � (g) → (g)

� ]1 ]1

(g) � (g) → (g)

(g) � (g) → (g) � (g)

(g) � (g) → (g)

(g) � (g) → (g) � (g)

(g) � (g) → (g)

(g) → (g)

� 1.

REACTION MECHANISMS



26

� � → � �

� 1 �]1.

(g) � (g) → (g) � (g)

� ] .

(g) � (g) → (g) � (g)

(g) → Cl(g) � (g)

(g) → (g) � (g)


Name Section

27

†

�

EXPERIMENT #1: R � → �

‡

†

‡

E X T E N T O F A R E A C T I O N


DURING CLASS INVENTIONS · EQUILIBRIUM

28


†


Predicted

Predicted †

†


29


Predicted

Predicted †


†

†

EXTENT OF A REACTION



30

R � → �

chemical equilibrium

aA(g) � (g) � cC(g) � (g)


Name Section

31

(g) � (g) � (g)

Container BeforeReaction Started

Container After ReactionAchieves Equilibrium

CALCULATING THE EQUIL IBRIUM CONSTANT FOR A REACTION



32

(g) � (g) � (g)



(g) � (g) � (g)




CALCULATING THE EQUILIBRIUM CONSTANT FOR A REACTION

33

�



(g) � (g) � (g)

] � ] � � c



34

(g) � (g) � (g)

b. 12

(g) � 12

(g) � (g)

(g) � (g) � (g)

c

(g) � (g) � (g)


Name Section

35

A (g) � (g) � (g)



A (g) � (g) � (g)

CALCULATING THE EQUILIBRIUM CONCENTRATION OF ALL SPECIES



36

(g) � (g) � (g)

� �

c

(g) � (g) � Cl (g)

c

(g) � (g) � Cl (g)


Name Section

37

†


†

L E C H Â T E L I E R ’ S P R I N C I P L E



38

EXPERIMENT #2: Increase reactant R to 2.0 M R � � �

EXPERIMENT #3: Increase reactant BG to 1.0 M R � � �


39

EXPERIMENT #4: Decrease reactant R to 0.75 M R � � �

EXPERIMENT #5: Increase product RG to 2.0 M R � � �

LE CHÂTELIER’S PRINCIPLE



40

EXPERIMENT #6: Decrease product RG to 1.0 M R � � �

Experiment Stress Change in [Reactants]

Change in [Products] Reaction shift


Name Section

41

(g) � (g) � (g)

Measurement # [H2] (M) [I2] (M) [HI] (M) ratio [HI]2/[H2][I2]

1

HI

H I[ ]

[ ] [ ]2

2 2

N O N - E Q U I L I B R I U M R E A C T I O N Q U O T I E N T



42


43

(g) � (g) � (g)

c

� � ] �

� � ] �

� � ] �

� � ] �

� � ] �

NON-EQUILIBRIUM REACTION QUOTIENTS


Name Section

45

(g) � (g)

Temperature (K) 1/T (K) K ln (K)

TEMPERATURE DEPENDENCE OF THE EQUILIBRIUM CONSTANT



46

��

�


47

TEMPERATURE DEPENDENCE OF THE EQUILIBRIUM CONSTANT



48

(g) � (g)

� � – –1

(g) � (g) � Cl (g)

� � –1 c �

c


Name Section

49

(aq)

(aq)

A R R H E N I U S A C I D S [ H � ] , [ O H � ] , p H A N D p O H


DURING CLASS INVENTIONS · ACIDS AND BASES

50

ArrheniusAcids

ArrheniusBases

� �


51

� � �] �

� �

� �

� ��

� � � �

� � � �

� �

ARRHENIUS ACIDS [H�], [OH�], pH AND pOH



52

�] � � M.

� – �


Name Section

53

(aq)

(aq)

(aq) � →

B R Ø N S T E D – L O W R Y A C I D / B A S E T H E O R Y



54

�

�

�

�


Name Section

55

† � �

Solution pH Equilibrium [H�] or [OH�]

�

�

†

A C I D S , B A S E S A N D p H



56


Name Section

57

(aq) � �(aq) � Cl�(aq)

ICE � �. �.

(aq) � �(aq) � Cl�(aq)

I C E

�].

�

�].

(aq) �(aq).

(aq).

S T R O N G A C I D S A N D T H E E Q U I L I B R I U M C O N S TA N T


Name Section

59

(aq) � �(aq) � C �(aq)

ICE

� �

�.

(aq) � �(aq) � C �(aq)

I C E

�].

�

�].

(aq) �(aq).

W E A K A C I D S A N D T H E E Q U I L I B R I U M C O N S T A N T



60

(aq).

�

�

a � ��

b � ��


Name Section

61

�

.

�

a1

� �

P O L Y P R O T I C A C I D S



62

� � �11� � �]


Name Section

63

salt.

† � �

Solution pH Equilibrium [H�] or [OH�] Acidic, Basic, or Neutral

Cl

(aq) � (aq) →

(aq) � (aq) →

(aq) � (aq) →

†

S A L T S I



64

(s)

�(aq)

a�(aq).

�(aq)

b�(aq).

�(aq) �(aq)

(s)


65

Cl(s)

�(aq)

a�(aq).

�(aq)

b�(aq).

�(aq) �(aq)

(s)

SALTS I


Name Section

67

a � �� .

b � �� .

S A L T S I I


Name Section

69

Solution pH

.

a

†

†

T H E C O M M O N I O N E F F E C T


DURING CLASS INVENTIONS · AQUEOUS EQUILIBRIUM

70

.

.


Name Section

71

(aq) � (aq) → (l) � (aq)

(aq) � (aq) → (l) � (aq)

(aq) � (aq) → (aq)

N E U T R A L I Z A T I O N R E A C T I O N S


Name Section

73

TITRATION BETWEEN A STRONG ACID AND A STRONG BASE


75

TITRATION BETWEEN A STRONG ACID AND A STRONG BASE


Name Section

77

TITRATION BETWEEN A WEAK ACID AND A STRONG BASE


79



81

.

.



Name Section

83

I N T R O D U C T I O N T O B U F F E R S



84

.


Name Section

85

.

B U F F E R S


Name Section

87

Solubility TableIon Solubility Exceptions

�

�

Cl� � � ��

� � � � � � �

� �

� �

� � � �

� �

�

�

�

P R E C I P I T A T I O N A N D S O L U B I L I T Y



88

(g) (l) (s) (aq)

(aq) � (aq) →

(aq) � (aq) →

(aq) � (aq) →

2 (aq) � (aq) →

M m(s) �m�(aq) � �(aq)

solubility product constant.

�m

� �


Name Section

89

� 1.1 � � .

.

.

�

S O L U B I L I T Y E Q U I L I B R I A P R O B L E M S


Name Section

91

(l) → (g)

(s) � (g) → (s)

(s) � Cl(s) → (aq) � (l) � (aq)

(g) � 12

(g) → (l) (g)

(g) � (g) → (g) � (g)

(s) � 32

(l) → (s)

E N T H A L P Y A N D T H E F I R S T L A W


DURING CLASS INVENTIONS · THERMODYNAMICS

92

�


Thermodynamic Values (25°C)

Substance and State

Δ Δ

⎛⎝⎜

⎞⎠⎟

⎛

H G S

kJmol

kJmol

0f

0f

0

⎝⎝⎜⎞⎠⎟

⎛⎝⎜

⎞⎠⎟

JK moli

Substance and State

Δ Δ

⎛⎝⎜

⎞⎠⎟

⎛

H G S

kJmol

kJmol

0f

0f

0

⎝⎝⎜⎞⎠⎟

⎛⎝⎜

⎞⎠⎟

JK moli

Aluminum Iodine(s) � � (s)

Al(s) (g)(g)

Barium(aq) � � Magnesium

(s) � � (s)�(aq) � � �

Bromine (s) � �(l)

(g) � Oxygen(g)

Carbon (g)C(s) (g)C(s)

(g) � � Nitrogen(g) � � (g)(g) � � (g) �

(g) � � (g) � � �(l) � � (g) � �

(g) � � (aq) � � 111(g) � � (aq)

(g) (g)C (g) (g)C (g) (g)

(g) � � (g)C (l) � � (g) �

C (g) � � (l)C (g) (aq) � �111C (g) � � (l) � �

Cl(s) � �Chlorine (s) � �Cl (g)Cl (aq) � SilverCl�(aq) � � (s)

(g) � � �(aq)(s) � �

Fluorine (s) � �(g)

�(aq) � � � Sulfur(g) � �

Hydrogen (g) � �(g) (g) � �

(g) (g) � ��(aq)

�(aq) � � �11 Titanium(l) � � TiCl (g) � �(g) � � (s) � �


Name Section

95

entropy�

(l) → (g)

(s) � (g) → (s)

(s) � Cl(s) → (aq) � (l) � (aq)

(g) � 12

(g) → (l) (g)

(g) � (g) → (g) � (g)

(s) � 32

(l) → (s)

�

S P O N T A N E I T Y A N D E N T R O P Y



96

�

a.

b.

c.

.


Thermodynamic Values (25°C)

Substance and State

Δ Δ

⎛⎝⎜

⎞⎠⎟

⎛

H G S

kJmol

kJmol

0f

0f

0

⎝⎝⎜⎞⎠⎟

⎛⎝⎜

⎞⎠⎟

JK moli

Substance and State

Δ Δ

⎛⎝⎜

⎞⎠⎟

⎛

H G S

kJmol

kJmol

0f

0f

0

⎝⎝⎜⎞⎠⎟

⎛⎝⎜

⎞⎠⎟

JK moli

Aluminum Iodine(s) � � (s)

Al(s) (g)(g)

Barium(aq) � � Magnesium

(s) � � (s)�(aq) � � �

Bromine (s) � �(l)

(g) � Oxygen(g)

Carbon (g)C(s) (g)C(s)

(g) � � Nitrogen(g) � � (g)(g) � � (g) �

(g) � � (g) � � �(l) � � (g) � �

(g) � � (aq) � � 111(g) � � (aq)

(g) (g)C (g) (g)C (g) (g)

(g) � � (g)C (l) � � (g) �

C (g) � � (l)C (g) (aq) � �111C (g) � � (l) � �

Cl(s) � �Chlorine (s) � �Cl (g)Cl (aq) � SilverCl�(aq) � � (s)

(g) � � �(aq)(s) � �

Fluorine (s) � �(g)

�(aq) � � � Sulfur(g) � �

Hydrogen (g) � �(g) (g) � �

(g) (g) � ��(aq)

�(aq) � � �11 Titanium(l) � � TiCl (g) � �(g) � � (s) � �


Name Section

99

� � � �

� � �

(l) → (g)

(s) � (g) → (s)

(s) � Cl(s) → (aq) � (l) � (aq)

(g) � 12

(g) → (l) (g)

(g) � (g) → (g) � (g)

(s) � 32

(l) → (s)

S P O N T A N E I T Y A N D F R E E E N E R G Y



100

�

� �

� � � � T�

�

�

Sign of �H˚rxn (25 ˚C)

Sign of �S˚rxn (25 ˚C)

Sign of �G˚rxn (25 ˚C)

Sign of �G˚rxn at high temperature

Sign of �G˚rxn at low temperature

− �� −− −� �


101

�

a. Al(s) � 32

(l) → (s)

(g) → (g)

c. (g) � (l) → (g) � (g)

�

�

(g) � (g) → Cl(s)

SPONTANEITY AND FREE ENERGY


Name Section

103

A � � C � c � 1 M 1 M 1 M 1 M

� �

� �

� �

� � �

�

K �G˚

�

�

�

�

F R E E E N E R G Y A N D T H E E Q U I L I B R I U M C O N S T A N T



104

� (g) → (g).

�

� � � �


Name Section

105

Chemical Equation Reaction Type

(s) � (g) → (g)

(g) � (g) → (g)

(g) � (g) → (g) � (l)

(s) → (l) � (g)

I N T R O D U C T I O N T O O X I D A T I O N – R E D U C T I O N


DURING CLASS INVENTIONS · ELECTROCHEMISTRY

106

(aq) � (aq) → (s) � (g)

�(aq) � �(aq) → �(aq) � �(aq)

(s) � (g) → (g) � (s) � (s)


Name Section

107

†

©

Hay

den-

McN

eil,

LL

C

V

Volts

†

G A L V A N I C C E L L S



108

i. Zn Zn H H Pt(s) (aq) (aq) (g) (s)2 2� �

i. Cr Cr MnO H Mn Pt(s) (aq) (aq) (aq) (aq) (s3 42� � �– , , ))


Name Section

109

†

(s) � (aq) → (s) � (aq)

(s) � (aq) → (g) � (aq)

(s) � (aq) → 2 (s) � (aq)

electromotive force volt.

†

E M F F O R G A L V A N I C C E L L S



110

�(aq).

�(aq).


111

� (l)�(aq)

�

�

M �(aq) � � → M(s)

�(aq)�(aq).

EMF FOR GALVANIC CELLS



112

Standard Reduction Potentials at 25°C

Half–Reaction E°(g) � � → �(aq) �

(aq) � �(aq) � � → (l) ��(aq) � �(aq) � � → �(aq) � (l) �

�(aq) � � → (s) �Cl (g) � � → �(aq) �

Cr �(aq) � �(aq) � � → �(aq) � (l) �(g) � �(aq) � � → (l) �

(l) � � → �(aq) ��(aq) � �(aq) � � → (g) � (l) �

�(aq) � 1e� → (s) �(s) � � → �(aq) �

(g) � (l) � � → �(aq) ��(aq) � � → (s) �

(s) � 1e� → (s) � Cl�(aq) ��(aq) � � → (s)�(aq) � � → (s) ��(aq) � � → (s) ��(aq) � � → (s) ��(aq) � � → (s) ��(aq) � � → (s) ��(aq) � � → (s) �

(l) � � → (g) � �(aq) �Cr �(aq) � � → Cr(s) �

�(aq) � � → (s) �Al �(aq) � � → Al(s) �

�(aq) � � → (s) ��(aq) � 1e� → (s) �

Ca �(aq) � � → Ca(s) ��(aq) � � → (s) ��(aq) � 1e� → (s) ��(aq) � 1e� → (s) �


Name Section

113

cell�(aq) �(aq)

Experiment Ecell E˚ [Zn2�] [Cu2�]

1 1 11.1

11

cell logZn

Cu

2

2

�

�

⎡⎣ ⎤⎦⎡⎣ ⎤⎦

⎛

⎝⎜

⎞

⎠⎟

cell � � 0 0591.

n log

Zn

Cu

2

2

�

�

⎡⎣ ⎤⎦⎡⎣ ⎤⎦

⎛

⎝⎜

⎞

⎠⎟

cell

N E R N S T E Q U A T I O N



114

(s) � �(aq) → �(aq) � (s)

cell�] �

1 � � �] �

cell�] �

1 � � �] �

�

�

�

�

�

cell

Cu Cu (3.00 M) Cu (0.100 M) Cu2 2(s) (aq) (aq) (s)� �


Name Section

115

Cathode(graphite rod)

Anode(zinc inner case)

Paste of MnO2,NH4Cl, and carbon

©Hayden-McNeil, LLC

B A T T E R I E S



116


Name Section

117

(g)

(l) (aq).

E L E C T R O L Y S I S I



118

(aq)

(aq)

(l)


Name Section

119

� �

� �

� �

E L E C T R O L Y S I S I I



120

(l) � (g) � (g)

Time of current flow in

minutes

Time of current flow in

seconds

Current (amperes)

Number of Coulombs that flow

Number of mol of electrons that flow

Half-reaction Mass of gas/metal produced (grams)

� � � � → (g) � �

� �

� � → (g) � � � �

� �1

� � → (g) � �

→ (g) � � � �

e� � �(aq) → (s)

� � � (aq) → (s)

� � � (aq) → (s)


STOICHIOMETRY · MASS AND PARTICLE RELATIONSHIPS

121

.

ELECTROCHEMISTRY · ELECTROLYSIS


Computer Lab Activities

GE

NE

RA

L C

HE

MIS

TR

Y

MoLEs

Laboratory Simulations


MoLEs

AC

TI

VI

TI

ES

125

˙Introduction to MoLEs Activities—Computer Simulations*


COMPUTER LAB ACTIVITIES · MoLEs

126

Particulate Simulations

Figure 1.

Control Bar

Region

Module Display

Region

Sample Region


INTRODUCTION TO MoLEs ACTIVITIES

127

Figure 2.



128

Graphic Simulations

Figure 3.


INTRODUCTION TO MoLEs ACTIVITIES

129NOT FOR DISTRIBUTION - FOR INSTRCTORS USE ONLY

M E C H A N I S M S O F A C H E M I C A L R E A C T I O N

131

Name Section

˙

Figure 1.



132

Problem Statement: How does a chemical reaction proceed from reactants to products?

I. Data Collection

R BG B RG

# of Particles

Concentration (M)

R BG B RG

# of Particles

Concentration (M)


KINETICS · MECHANISMS OF A CHEMICAL REACTION

133

II. Data Analysis and Interpretation



134

III. Data Collection

Collisions Between

Particle 1 Particle 2 Result Speed Orientation Comments

R R No reaction — — —

R BG

R B

R RG

BG B

BG BG

BG RG

B B

B RG

RG RG

IV. Data Analysis and Interpretation



135

V. Conclusions

Reactants Collision Products

VI. Data Collection

G B G2 GB G2B B2

# of Particles

Concentration (M)



136

G B G2 GB G2B B2

# of Particles

Concentration (M)

VII. Data Analysis and Interpretation



137

VIII. Data Collection

Reactant 1 Reactant 2 Result Comments

B B

B G

G G



139

IX. Conclusions

� →


S P E E D S O F A C H E M I C A L R E A C T I O N

141

Name Section

Figure 1.



142

Problem Statement: What factors influence how fast a chemical reaction proceeds?

I. Data Collection

R R2

# of Particles

Concentration (M)

R R2

# of Particles

Concentration (M)

Time (in sec)

Time (in mm)

Formula 1mm � __ seconds


KINETICS · SPEEDS OF A CHEMICAL REACTION

143

i

i � �

Trial 1 Trial 2 Trial 3 Average

Temperature

Time (mm)

Time (sec)

i � �


Temperature

Time (mm)

Time (sec)

i � �


Temperature

Time (mm)

Time (sec)



144


i

� � i

I. D I. E I. F

[R]i

[R]f

[R]


KINETICS · SPEEDS OF A CHEMICAL REACTION

145

�

�

�


R A T E S O F A C H E M I C A L R E A C T I O N

147

Name Section

Figure 1.



148

Problem Statement: How is the rate of a chemical reaction related to the initial concentration of the reactants?

I. Data Collection


KINETICS · RATES OF A CHEMICAL REACTION

149

�

Experiment # [RG]0 (M)Initial Rate

(M time-1),�[RG]/time

1



150




151


Experiment # [RG]0 (M)Initial Rate

(M time�1),�[RG]/time



152




154

V. Data Collection

Experiment # [ ] Initial Rate Reactant,�[ ]/t

1 1.0mol/40L � 0.0250M

2 2.0mol/40L � 0.0500M

3 0.333mol/40L � 0.008325M



155

VI. Data Analysis and Interpretation



157

VII. Data Collection



158

Experiment # [ ] [ ] Initial Rate, [G2B]/time

VIII. Data Analysis and Interpretation



159

IX. Data Collection

http://introchem.chem.okstate.edu/DCICLA/

X. Data Analysis and Interpretation



160

Step One

Step Two


C A T A L Y S T S

163

Name Section

Figure 1.



164

Problem Statement: What factors influence how fast a chemical reaction proceeds?

I. Data Collection

B G BG R RB

# of Particles

Concentration (M)

B G BG R RB

# of Particles

Concentration (M)


KINETICS · CATALYSTS

165


Time (in sec)

Time (in mm)

Formula: 1mm � _______ seconds


Time (in sec)

Time (in mm)




166

III. Data Collection: Add Particle R as a Reactant

B G BG R RB

# of Particles

Concentration (M)

B G BG R RB

# of Particles

Concentration (M)



167

Collisions Between

Particle 1 Particle 2 Result Comments

B G

B R

G R

B RB

G RB


Time (in mm)

Time (in sec)



A C T I V A T I O N E N E R G Y

171

Name Section

Figure 1.



172

Problem Statement: How does the activation energy affect a chemical reaction?

I. Data Collection


KINETICS · ACTIVATION ENERGY

173


Time (in sec)

Time (in mm)

Formula: 1mm � _______ seconds

[R2] [B] [R2B]

Initial [ ]

Final [ ]

[ ]

Time (sec)

Average Rate



174

[R2] [B] [R2B]

Initial [ ]

Final [ ]

[ ]

Time (sec)

Average Rate

[R2] [B] [R2B]

Initial [ ]

Final [ ]

[ ]

Time (sec)

Average Rate



175





179




180

V. Data Collection




181


Experiment # [ ] [ ] Initial Rate,[R2G]/time




182

IX. Data Collection

R

Experiment # [ ] [ ] Initial Rate, [B2R]/time



183



K I N E T I C S Y S T E M S

185

System 1

� → �

→ R�

C. R� →

→ R�

System 2

System 3� →

� → �

� →

→ �

� →



186

System 4

System 5

System 6

R E S E A R C H S T A T E M E N T S


S H I F T I N G R E A C T I O N S A

187

Name Section

Figure 1.



188

Problem Statement: What are the characteristics of a hypothetical chemical reaction?

I. Data Collection

Figure 2.


EQUILIBRIUM · SHIFTING REACTIONS A



190

II. Data Analysis




192

IV. Data Analysis

V. Interpretation and Conclusions



193

(s) → (s) � (g)


S H I F T I N G R E A C T I O N S B

195

Name Section

Figure 1.



196

Problem Statement: How can concentration changes affect a chemical reaction?

I. Data Collection



EQUILIBRIUM · SHIFTING REACTIONS B

197


Initial Ending



198


EXPERIMENT #2: Increase Reactant R to 2.0 M

R � → �



199

EXPERIMENT #3: Increase Reactant BG to 1.0 M

R � → �

EXPERIMENT #4: Decrease Reactant R to 0.75 M

R � → �



200

EXPERIMENT #5: Increase product RG to 2.0 M

R � → �

Your Prediction: Your Observation:



201

EXPERIMENT #6: Decrease product RG to 1.0 M

R � → �

Your Prediction: Your Observation:



202


Experiment Stress Change in [Reactants]

Change in [Products] Reaction shift

#2 Add reactant [R]Concentrations

decreasedConcentrations

increasedLeft to Right

#3

#4

#5

#6

2.0

1.0

0

BG

R

RG

B

1 2 3

Time



203

V. Conclusions

15

10

5

0

Con

cent

ratio

n

Time

1 2 3 4

C

BA

� � �

time � 1 time � 2 time � 3

� �


E X T E N T O F A C H E M I C A L R E A C T I O N

205

Name Section

Figure 1.



206

Problem Statement: What is the relationship between reactant and product concentrations at the end of a reaction?

I. Data Collection�




207

EQUILIBRIUM · EXTENT OF A CHEMICAL REACTION






208

R � → �

V. Data Collection




209


R � → �






210

R � → �

IX. Data Collection



211



XI. Data Collection




212




213


XII. Data Analysis

R� → �



214

XIII. Data Interpretations and Conclusions

R � → �


E Q U I L I B R I U M S Y S T E M S

215

System 1 � → �

� →

→ �

→ R�

System 2→ �

→ R�

System 3

System 4

System 5

System 6

System 7



216

� →

→ �

→ R�


217

Name Section

Figure 1.

A C I D / B A S E C L A S S I F I C A T I O N S



218

Problem Statement: What are the characteristics of acid solutions?

I. Data Collection

[HG] [H2O] [H3O�] [G�]

Before Reaction

After Reaction


ACID/BASE CHEMISTRY · ACID/BASE CLASSIFICATIONS

219


.



220


[HG] [H2O] [H3O�] [G�]

Before Reaction

After Reaction

[HG] [H2O] [H3O�] [G�]

Before Reaction

After Reaction



221


�

�



222

V. Data Collection



223

[HB] [H2O] [H3O�] [B�]

Before Reaction

After Reaction

� �

[H3O�] [B�] [HB] [H2O]

Before Reaction

After Reaction

VI. Interpretation and Conclusions



224


� � � �

� � � � � �



225

VIII. Interpretation and Conclusions

�

�

�



226

a

a


227

Name Section

�

Figure 1.

A C I D / B A S E I N T E R A C T I O N S



228

Problem Statement: How do acids and bases interact?

I. Data Collection

[H2O] [HG] [H3O�] [G�] [OH�]

Initial – I

Change – C

Ending – E


ACID/BASE CHEMISTRY · ACID/BASE INTERACTIONS

229

�




230


�

[H2O] [HG] [H3O�] [G�] [OH�]

I

C

E



231




232

V. Data Collection�

�

�

[H2O] [HB] [H3O�] [B�] [OH�]

I —

C —

E —

�



233

VI. Interpretation and Conclusions


�

� � � � �



234

�

[H2O] [HB] [H3O�] [B�] [OH�]

I

C

E

�

[H2O] [HB] [H3O�] [B�] [OH�]

I

C

E

VIII. Interpretation and Conclusions

�

�



235

�

a


Name

Lab Section

237

System 1

�

�

System 2

System 3

A C I D / B A S E S Y S T E M S



238

�


Introduction to Laboratory Simulations

AC

TI

VI

TI

ES

239


COMPUTER LAB ACTIVITIES · LABORATORY SIMULATIONS


241

Name Section

Problem Statement: How do concentration and temperature influence the rate of a chemical reaction?

I. Data Collection

I O D I N E C L O C K



242

�(aq) � �(aq) → �(aq) � �(aq)

�(aq) � �(aq) → �(aq) � �(aq)

�(aq) � → � �(aq)

� �

�

�

(aq) (aq)

TRIAL 1.0 M KI(aq) 0.1 M (NH4)2S2O8(aq)

Time @ 25 °C Time @ 45 °C Time @ 5 °C

1

2

3


KINETICS · IODINE CLOCK

243

II. Data Analysis and Interpretation� �

� �

TRIAL [I�] [S2O82�]

Ave Rate @ 25 °C

Ave Rate @ 45 °C

Ave Rate @ 5 °C

1

2

3

�1

�

�


KINETICS · IODINE CLOCK

245

III. Conclusions


247

Name Section

Problem Statement: How do concentration and temperature influence the rate of a chemical reaction?

I. Data Collection

C O N C E N T R A T I O N / T E M P E R A T U R E E F F E C T S



248

�(aq) � (aq) � �(aq) → �(aq) � (l)

TRIAL H2O(l)0.010 M H2O2(aq)

1.0 M HCl(aq)

0.050 M KI(aq) Time @ 25 °C

1 60 mL 10 mL 20 mL 10 mL

2

3

4

5

6

7

8


KINETICS · CONCENTRATION/TEMPERATURE EFFECTS

249


� � � �

TRIAL [H2O2] [H�] [I�] Rate @ 25 °C

1

2

3

4

5

6

7

8



250

�

�


TRIAL [H2O2] [H�] [I�]

Rate @ 5 °C

Rate @ 15 °C

Rate @ 25 °C

Rate @ 35 °C

Rate @ 45 °C

1


KINETICS · CONCENTRATION/TEMPERATURE EFFECTS

251




252

V. Conclusions


253

Name Section

Problem Statement: How do catalysts influence the rate of a chemical reaction?

I. Data Collection

(aq) → (l) � (g)

D E C O M P O S I T I O N O F H 2 O 2



254

.

Rate with 0.5M KI (mL/sec)

Rate with 1.0 M KCl (mL/sec)

Rate with 0.1M FeCl3 (mL/sec)

0mL 2mL 0 mL 2mL 0 mL 2mL

5mL H2O210mL H2O2

.


KINETICS · DECOMPOSITION OF H2O2

255



257

Name Section

Problem Statement: What are the acid and base properties of solutions?

I. Data Collection

A C I D / B A S E p H



258

� �

Solution Concentration (M) pH [H�]

HCl(aq) 1.00 � 10�2

HCl(aq) 1.00 � 10�3

HCl(aq) 1.00 � 10�5

HCl(aq) 1.00 � 10�6

II. Data Analysis and Interpretation� � � �

�


ACID/BASE · ACID/BASE pH

259

III. Data Collection � �


HC2H3O2(aq) 1.00 � 10�2

HC2H3O2(aq) 1.00 � 10�3

HC2H3O2(aq) 1.00 � 10�5

HC2H3O2(aq) 1.00 � 10�6

IV. Data Analysis and Interpretation�

�



260

V. Data Collection� �


H2SO4(aq) 1.00 � 10�2

H2SO4(aq) 1.00 � 10�3

H2SO4(aq) 1.00 � 10�5

H2SO4(aq) 1.00 � 10�6

VI. Data Analysis and Interpretation�

�



261

VII. Data Collection and Analysis� �

Solution Concentration (M) pH

[H�] Strong/Weak

HCl(aq) 1.00 � 10�2

H2SO4(aq) 1.00 � 10�2

HC2H3O2(aq) 1.00 � 10�2

HF(aq) 1.00 � 10�2

HC3H5O3(aq) 1.00 � 10�2

HNO3(aq) 1.00 � 10�2

HClO2(aq) 1.00 � 10�2

HNO2(aq) 1.00 � 10�2

�



262

VIII. Data Collection� �

Solution Concentration (M) pH[H�] [OH�]

NaOH(aq) 1.00 � 10�2

NaOH(aq) 1.00 � 10�3

NaOH(aq) 1.00 � 10�5

NaOH(aq) 1.00 � 10�6

IX. Data Analysis and Interpretation�

� �

1 � � � � �]

�



263

�

X. Data Collection and Analysis� �

Solution Concentration (M) pH

[H�] [OH�] Strong/Weak

NaOH(aq) 1.00 � 10�2

KOH(aq) 1.00 � 10�2

NH3(aq) 1.00 � 10�2

Ca(OH)2(aq) 1.00 � 10�2

(CH3)2NH(aq) 1.00 � 10�2

C6H5NH2(aq) 1.00 � 10�2

HONH2(aq) 1.00 � 10�2

� �


265

Name Section

Problem Statement: How do acids and bases interact?

I. Data Collection

A C I D / B A S E T I T R A T I O N S



266

Acid, HCl Base, KOH

Volume (mL)

Concentration (M)


ACID/BASE · ACID/BASE TITRATIONS

267

Acid, HCl Base, KOH

Volume (mL)

Concentration (M)

Acid, HCl Base, Ba(OH)2

Volume (mL)

Concentration (M)


(aq) � (aq) →



268

Acid/Base Indicator pH Range Color change

Methyl Red 4.8–6.0 Yellow to Red

Bromothymol Blue 6.0–7.6 Yellow to Blue


ACID/BASE · ACID/BASE TITRATIONS

269


Acid, CH3COOH Base, KOH

Volume (mL)

Concentration (M)



270



271

Name Section

Problem Statement: What are the acid and base properties of salt solutions?

I. Data Collection

A C I D / B A S E S A L T S



272

� �

Solution Concentration (M) pH [H�] [OH�]

NaCl(aq) 1.00 � 10�2

NH4NO3(aq) 1.00 � 10�2

NaC2H3O2(aq) 1.00 � 10�2

NH4Cl(aq) 1.00 � 10�2

Na2SO4(aq) 1.00 � 10�2

NaCN(aq) 1.00 � 10�2

NaNO3(aq) 1.00 � 10�2

NaF(aq) 1.00 � 10�2

(NH4)2SO4(aq) 1.00 � 10�2

� �

II. Data Analysis and Interpretation� � � �

� �

1 � � � � �]

�


ACID/BASE · ACID/BASE SALTS

273

Solution Acid/Base/Neutral Ions

NaCl(aq)

NH4NO3(aq)

NaC2H3O2(aq)

NH4Cl(aq)

Na2SO4(aq)

NaCN(aq)

NaNO3(aq)

NaF(aq)

(NH4)2SO4(aq)


B U F F E R S

275

Name Section

Problem Statement: What are the characteristics of buffer solutions?

I. Data Collection

� � �

� � � � �


276

� �

�

� �

Solution Concentration (M) pH Acid, Base, Neutral

HC2H3O2(aq) 0.10

HCl(aq) 0.10

NaCl(aq) 0.10

NaC2H3O2(aq) 0.10

.




ACID/BASE · BUFFERS

277

III. Data Collection � �

� �

Solution pH Concentration of Acid (M)

Concentration of Salt (M)

HCl(aq) � NaCl(aq)

HC2H3O2(aq) � NaCl(aq)

HC2H3O2(aq) � NaC2H3O2(aq)

� �

� �

� � � �



278




280

V. Data Collection� �

�

Solution pH pH after adding 1 � 10�3 mol acid

pH after adding 1 � 10�3 mol base

1.82 � 10�5 M in HCl(aq)

1.82 � 10�5 M in HCl(aq) and

1.82 � 10�5 M in NaCl(aq)4.74 2.3 11.7

3.8 � 10�5 M in HC2H3O2(aq)

3.8 � 10�5 M in HC2H3O2(aq) and

3.8 � 10�5 M in NaCl(aq)4.74 2.3 11.7

0.1 M in HC2H3O2(aq) and

0.1 M in NaC2H3O2(aq)

� � � �

� �

� �

VI. Data Analysis and Interpretation� � � �

� �



281

� � � � � �



282

(aq) � (l) � �(aq) � W�(aq)

.1M .1M


A C T I V I T I E S O F M E T A L S

283

Name Section

Problem Statement: How do metals and metal ions react?

I. Data Collection: Eight Solutions

Figure A.



284

II. Data Analysis

III. Interpretation

Figure B.


ELECTROCHEMISTRY · ACTIVITIES OF METALS

285

IV. Data Collection: Activity One

Mg2�(aq) Zn2�(aq) Cu2�(aq) Ag�(aq)

Mg(s)

Cu(s)

Zn(s)

Ag(s)

Table 1



286

V. Data Analysis

Example:

(s) � (aq) → (aq) � (s)

(s) � �(aq) → �(aq) � (s)



287

Most Reactive

Least Reactive

Metal Ion MetalLeast Reactive

Most Reactive

Column 2a Column 2b

VI. Interpretation

Metal Selected in Column 2bMetal Ions in Column 2a

that React with Metal from Column 2b

Metal Ions in Column 2a that Do Not React with Metal

from Column 2b

Table 2



289

VII. Data Collection: Activity Two

Fe2�(aq) Zn2�(aq) Cu2�(aq) Pb2�(aq)

Fe(s)

Cu(s)

Zn(s)

Pb(s)

Table 3



290


Most Reactive

Least Reactive

Metal Ion MetalLeast Reactive

Most Reactive

Column 4a Column 4b

Table 4



291

IX. Data Collection: Activity Three

Fe2�(aq) Pb2�(aq) Ni2�(aq) Sn2�(aq)

Fe(s)

Pb(s)

Ni(s)

Sn(s)

Table 5



292

X. Data Analysis and Conclusions

Metal Ion Metal

Most Reactive Least Reactive

Least Reactive Most Reactive

Column 6a Column 6b



293

XI. Data Collection: Activity Four

XII. Data Analysis



294

XIII. Interpretation and Conclusions A. Add the hydrogen gas/hydrogen ion combination in the correct location in the tables from section X.

Metal Ion Metal

Most Reactive Least Reactive

Least Reactive Most Reactive

Column 7a Column 7b



295

B. Use the information in Columns 7a and 7b to predict the products of the following reactions.

a. Ag�(aq) � Ni(s) →

b. Ni2�(aq) � Ag(s) →

c. Ag�(aq) � Sn(s) →

d. Mg2�(aq) � Ni(s) →

e. Mg(s) � Sn(NO3)2(aq) →

f. H�(aq) � Mg(s) →

g. HCl(aq) � Sn(s) →

h. Fe2�(aq) � H2(g) →

i. Ag�(aq) � Mg2�(aq) →

j. H2(g) � Cu2�(aq) →

C. Mental Model: Draw a picture(s) that illustrates what happens at the molecular level when Ag� ion and Sn metal are mixed. In words, explain what is happening in your picture(s).



296

D. An unknown metal, M, not studied in this experiment, is found to react with Ag� ion, Pb2� ion, and Cu2� ion, but not with Ni2� ion, Mg2� ion, or Zn2� ion. Where does the unknown metal, M, appear in your activity series?


V O L T A I C C E L L S

297

Name Section

Problem Statement: What are the electrical properties of chemical reactions?

I. Data Collection



298

(aq) (aq)


ELECTROCHEMISTRY · VOLTAIC CELLS

299




300

III Data Collection

Left Cell Right Cell Voltage (Eº) Direction of Electrons

Ag/AgNO3 Cu/Cu(NO3)2 From to

Ag/AgNO3 Zn/Zn(NO3)2 From to

Ag/AgNO3 H2/HCl From to

Cu/Cu(NO3)2 Zn/Zn(NO3)2 From to

Cu/Cu(NO3)2 H2/HCl From to

Zn/Zn(NO3)2 H2/HCl From to


→ �(aq) � � �

+(aq) � 1e� → �


ELECTROCHEMISTRY · VOLTAIC CELLS

301

V. Conclusions�

�

�



302

�


C O N C E N T R A T I O N C E L L S

303

Name Section

Problem Statement: How does concentration affect the electrical properties of chemical reactions?

I. Data Collection



304

(aq) (aq)

Trial [AgNO3] right half-cell

[AgNO3] left half-cell Voltage (Eº)

1 2.0 M 2.0 M

2 2.0 M 1.0 M

3 2.0 M 0.1 M

4 2.0 M 0.01M

5 2.0 M 0.001M


ELECTROCHEMISTRY · CONCENTRATION CELLS

305


� �

�] �] �] �]



306

� �


Trial [Cu(NO3)2] right half-cell

[Cu(NO3)2] left half-cell Voltage (Eº)

1 2.0 M 2.0 M

2 2.0 M 1.0 M

3 2.0 M 0.1 M

4 2.0 M 0.01M

5 2.0 M 0.001M



307


� �

� �



308

�] �]�] �]



309

� �


E L E C T R O L Y S I S

311

Name Section

Problem Statement: How is electrical energy absorbed in a chemical reaction?

I. Data Collection



312

(aq)

TrialMass Ag

(left) Before

Mass Ag (left) After

Mass Ag (right) Before

Mass Ag (right) After

Voltage (E)

Current (amps) Time

1 10 g 10 g 0.20 v 0.50 amps 300 sec

2 10 g 10 g 0.20 v 0.50 amps 600 sec

3 10 g 10 g 0.20 v 1.00 amps 300 sec

4 10 g 10 g 0.40 v 0.50 amps 300 sec

5 10 g 10 g 0.20 v 1.50 amps 600 sec

(aq)

TrialMass Zn

(left) Before

Mass Zn (left) After

Mass Zn (right) Before

Mass Zn (right) After

Voltage (E)

Current (amps) Time

6 10 g 10 g 0.20 v 0.50 amps 300 sec


ELECTROCHEMISTRY · ELECTROLYSIS

313

II. Data Analysis and Interpretationcurrent.

�

�


Documents

During Class Inventions and Computer Lab Activitiesgenchem1.chem.okstate.edu/APCHEMSITE/Vol2DCI_Workbook.pdfDuring Class Inventions and Computer Lab Activities GENERAL CHEMISTRY Volume