Exam 2 Objectives

Front 1

[A] versus t

Back 1

Linear for a zero order reaction

Front 2

ln[A] versus t

Back 2

Linear for a second order reaction

Front 3

1 / [A] versus t

Back 3

Linear for a second order reaction

Front 4

M / s

Back 4

Zero order

Front 5

M * s^ -1

Back 5

Zero order

Front 6

1 / s

Back 6

First order

Front 7

s^-1

Back 7

First order

Front 8

1 / M * s

Back 8

Second order

Front 9

M^-1 * s^-1

Back 9

Second order

Front 10

What happens to the reaction of the rate when the number of collisions increases?

Back 10

The rate increases

Front 11

Should the collision energy be greater than or less than the activation energy for the reaction?

Back 11

Greater

Front 12

What happens to the rate if the orientation is very precise?

Back 12

Proceeds at a slower rate

Front 13

If the temperature changes, the ________ will change too.

Back 13

Constant

Front 14

Higher temperatures result in changes in the ________ of collisions, and the ________ energy of these collisions.

Back 14

Frequency, average

Front 15

If the concentration increases, what happens to the rate of the reaction?

Back 15

The rate increases as well

Front 16

If the energy of reactants is SMALLER than the energy of products, the overall reaction is _________.

Back 16

Endothermic

Front 17

If the energy of reactants is GREATER than the energy of products, the reaction is _____________.

Back 17

Exothermic

Front 18

A —> products

Back 18

Unimolecular

Front 19

A + A —> products

Back 19

Bimolecular

Front 20

A + B —> products

Back 20

Bimolecular

Front 21

A + A + A —> products

Back 21

Termolecular

Front 22

A + A + B —> products

Back 22

Termolecular

Front 23

A + B + C —> products

Back 23

Termolecular

Front 24

What is the rate determining step in a reaction?

Back 24

The SLOWEST step

Front 25

__________ appear first as a reactant and then as a product

Back 25

Catalysts

Front 26

__________ appear first as a product and then as a reactant.

Back 26

Intermediates

Front 27

Rate laws are written using ________ only.

Back 27

Reactants

Front 28

0 Celsius

Back 28

273.15 K

Front 29

A catalyst does not affect the position of ___________ of a chemical reaction.

Back 29

Equilibrium

Front 30

A catalyst does not affect the position of ___________ of a chemical reaction.

Back 30

Equilibrium

Front 31

K stands for the…

Back 31

Equilibrium constant

Front 32

Keq >> 1

Back 32

Favors products

Front 33

Keq <<< 1

Back 33

Favors reactants

Front 34

K = 1 means…

Back 34

K is somewhere between reactants and products but we can’t tell

Front 35

The larger the k….the farther the reaction proceeds to the _______ before equilibrium is reached

Back 35

Right

Front 36

Q stands for

Back 36

Reaction quotient at ANY other point of time but NOT at equilibrium

Front 37

What do these stand for?

- starting point

- certain point

- when equilibrium is reached

Back 37

Key words for Q

Front 38

Kp stands for…..

Back 38

Pressure

Front 39

Kc stands for…..

Back 39

Concentration

Front 40

If K is small and Q is big, the reaction goes to the ______ side

Back 40

Left

Front 41

If Q is small and K is big, the reaction goes to the _________ side.

Back 41

Right

Front 42

What is the formula used to cancel the x out?

Back 42

Ao / K > 400

Front 43

If you increase the pressure, you __________ the volume.

Back 43

Decrease

Front 44

The reaction will shift to the _______ side if you increase the pressure and decrease the volume.

Back 44

Right

Front 45

In order to decrease the pressure, you must _______ the volume.

Back 45

Increase

Front 46

If you decease the pressure and increase the volume, the reaction shifts to the _______ side.

Back 46

Left

Front 47

Endothermic q =

Back 47

Reaction goes left

Front 48

Exothermic q =

Back 48

Reaction goes to the right

Front 49

Why doesn’t a catalyst affect the equilibrium of a reaction?

Back 49

The addition of a catalyst doesn’t affect the equilibrium of a reaction because a catalyst speeds up both forward and reverse rates.

Front 50

Why doesn’t a catalyst affect the equilibrium of a reaction?

Back 50

The addition of a catalyst doesn’t affect the equilibrium of a reaction because a catalyst speeds up both forward and reverse rates.

Front 51

HCl

Back 51

Strong acid - Hydrochloric acid

Front 52

Why doesn’t a catalyst affect the equilibrium of a reaction?

Back 52

The addition of a catalyst doesn’t affect the equilibrium of a reaction because a catalyst speeds up both forward and reverse rates.

Front 53

HCl

Back 53

Strong acid - Hydrochloric acid

Front 54

HBr

Back 54

Strong acid - hydrobromic acid

Front 55

HI

Back 55

Strong acid- hydroiodic acid

Front 56

H2SO4

Back 56

Strong acid - sulfuric acid

Front 57

HNO3

Back 57

Strong acid - nitric acid

Front 58

HClO4

Back 58

Strong acid - perchloric acid

Front 59

HClO4

Back 59

Strong acid - perchloric acid

Front 60

NaOH

Back 60

Strong base - sodium hydroxide

Front 61

LiOH

Back 61

Strong base - lithium hydroxide

Front 62

KOH

Back 62

Strong base - potassium hydroxide

Front 63

Ca(OH)2

Back 63

Strong base - calcium hydroxide

Front 64

Sr(OH)2

Back 64

Strong base - strontium hydroxide

Front 65

Ba(OH)2

Back 65

Strong base - barium hydroxide

Front 66

________ ________ complete dissociate

Back 66

Strong acids

Front 67

________ ________ complete dissociate

Back 67

Strong acids

Front 68

________ ________ partially dissociate

Back 68

Strong bases

Front 69

Why does water dissociate slightly?

Back 69

One molecule in half a billion splits into an OH- ion by losing a proton to another water molecule. That other molecule becomes H3O+.

Front 70

pH =

Back 70

- log[H3O+]

Front 71

[H3O+] =

Back 71

10^-pH

Front 72

pH + pOH =

Back 72

14

Front 73

pOH =

Back 73

-log[OH-]

Front 74

[OH-] =

Back 74

10^-pOH

Front 75

Kw =

Back 75

[H3O+][OH-]

Front 76

Kw =

Back 76

[H3O+][OH-]

Front 77

pH 0-6 =

Back 77

Acidic

Front 78

Kw =

Back 78

[H3O+][OH-]

Front 79

pH 0-6 =

Back 79

Acidic

Front 80

pH of 7

Back 80

Neutral

Front 81

Kw =

Back 81

[H3O+][OH-]

Front 82

pH 0-6 =

Back 82

Acidic

Front 83

pH of 7

Back 83

Neutral

Front 84

pH 8 - 14

Back 84

Basic

Front 85

Kw =

Back 85

[H3O+][OH-]

Front 86

pH 0-6 =

Back 86

Acidic

Front 87

pH of 7

Back 87

Neutral

Front 88

pH 8 - 14

Back 88

Basic

Front 89

Brønsted-Lowry Acid

Back 89

Proton (H*) donor

Front 90

Kw =

Back 90

[H3O+][OH-]

Front 91

pH 0-6 =

Back 91

Acidic

Front 92

pH of 7

Back 92

Neutral

Front 93

pH 8 - 14

Back 93

Basic

Front 94

Brønsted-Lowry Acid

Back 94

Proton (H*) donor

Front 95

Brønsted-Lowry Base

Back 95

Proton (H+) acceptor

Front 96

Kw =

Back 96

[H3O+][OH-]

Front 97

pH 0-6 =

Back 97

Acidic

Front 98

pH of 7

Back 98

Neutral

Front 99

pH 8 - 14

Back 99

Basic

Front 100

Brønsted-Lowry Acid

Back 100

Proton (H*) donor

Front 101

Brønsted-Lowry Base

Back 101

Proton (H+) acceptor

Front 102

Conjugate base is formed when…

Back 102

Acid loses H+

Front 103

Conjugate acid is formed when…..

Back 103

Base gains H+

Front 104

What is an amphiprotic species?

Back 104

A species that can act as both an acid or base.

Front 105

What is an amphiprotic species?

Back 105

A species that can act as both an acid or base.

Front 106

What is the most common anohiprotic species?

Back 106

H2O

Front 107

What is an amphiprotic species?

Back 107

A species that can act as both an acid or base.

Front 108

What is the most common anohiprotic species?

Back 108

H2O

Front 109

K >1

Reaction goes to the ____ side

Back 109

Right

Front 110

K < 1… reaction goes to the _____ side.

Back 110

Left