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Chemistry 115 > Chapter 13 > Flashcards

Chapter 13 Flashcards

1
Q

Chemical kinetics

A

Study of rate of change of concentrations of substances involved in chemical reactions.

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2
Q

Study of rate of change of concentrations of substances involved in chemical reactions.

A

Chemical kinetics

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3
Q

Reaction rate

A

How fast a reaction happens, related to change in concentration of reactants and products over time.

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4
Q

How fast a reaction happens, related to change in concentration of reactants and products over time.

A

Reaction rate

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5
Q

Rate of change

A

Change in concentration of a single compound within a reaction.
Change in concentration/change in time

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6
Q

Change in concentration of a single compound within a reaction.
Change in concentration/change in time

A

Rate of change

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7
Q

Reaction rate

A

1[change in compound A]/ a(change in time)

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8
Q

1[change in compound A]/ a(change in time)

A

Reaction rate

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9
Q

Average rate

A

Change in concentration of reactant or product over a specific time interval.

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10
Q

Change in concentration of reactant or product over a specific time interval.

A

Average rate

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11
Q

Instantaneous rate

A

Reaction rate at a specific time.

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12
Q

Reaction rate at a specific time.

A

Instantaneous reaction rate

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13
Q

Rate law

A

Equation defining relationship between reactant concentrations and the rate of the reaction. Determined experimentally.

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14
Q

Equation defining relationship between reactant concentrations and the rate of the reaction. Determined experimentally.

A

Rate law

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15
Q

Reaction order

A

Number defining the dependence of the reaction rate on reactant concentration.

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16
Q

Number defining the dependence of the reaction rate on reactant concentration.

A

Reaction order

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17
Q

Rate constant

A

k, proportionality constant that relates the reaction rate to reactant concentration.

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18
Q

k, proportionality constant that relates the reaction rate to reactant concentration.

A

Rate constant

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19
Q

Overall order

A

Orders of individual reactants added up. Determines effects of concentration in reaction rate.

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20
Q

Orders of individual reactants added up. Determines effects of concentration in reaction rate.

A

Overall order

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21
Q

First order reaction

A

Doubling reactant concentration doubles the reaction rate.

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22
Q

Doubling reactant concentration doubles the reaction rate.

A

First order reaction

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23
Q

Second order reaction

A

Doubling the reactant concentration increases the reaction rate by a factor of four.

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24
Q

Doubling the reactant concentration increases the reaction rate by a factor of four.

A

Second order reaction

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25
Zero order
Reaction rate is independent of reactant concentration.
26
Reaction rate is independent of reactant concentration.
Zero order
27
Integrated rate law
Dependance of concentration of reactants on time
28
Dependance of concentration of reactants on time
Integrated rate law
29
Half life
Time it takes for reactants to react to half their original concentration
30
Time it takes for reactants to react to half their original concentration
Half life
31
First order half life
Independent of initial concentration
32
Independent of initial concentration
First order half life
33
Increase in temperature during a reaction
Increases reaction rate
34
Increase of 10•C
Doubles reaction rate
35
Temperatures affects on reaction rate
As one increases the other does as well
36
Frequency factor
2 factors including collision frequency factor (z), and orientation factor (p)
37
2 factors including collision frequency factor (z), and orientation factor (p)
Frequency factor
38
Collision frequency factor (z)
Frequent and energetic collisions must occur to break bonds. Kinetic energy must be sufficient
39
Frequent and energetic collisions must occur to break bonds. Kinetic energy must be sufficient
Collision frequency factor (z)
40
Orientation factor (p)
Molecules must come into contact at the right spot to make new bonds. More complex molecules collide with the proper orientation less frequently
41
Molecules must come into contact at the right spot to make new bonds. More complex molecules collide with the proper orientation less frequently
Orientation factor (p)
42
Activated complex or transition state
Effective collision, when unstable chemical species is formed
43
Effective collision, when unstable chemical species is formed
Activated complex or transition state
44
Reaction mechanics
Most reactions happen in small steps between two molecules.
45
Most reactions happen in small steps between two molecules.
Reaction mechanics
46
Reaction mechanism
Outline of observed steps in a reaction
47
Outline of observed steps in a reaction
Reaction mechanism
48
Elementary step
A small reaction part of a full reaction. Rate law is determined by stoichiometry
49
A small reaction part of a full reaction. Rate law is determined by stoichiometry
Elementary step
50
Molecularity
Number of reactant particles in an elementary step
51
Number of reactant particles in an elementary step
Molecularity
52
Unimolecular step
One reactant present
53
One reactant present
Unimolecular
54
Bimolecular
Involves 2 reactant particles of the same species, or of different species
55
Involves 2 reactant particles of the same species, or of different species
Bimolecular step
56
Temoleculer step
Three reactant particles, extremely rare
57
Three reactant particles, extremely rare
Trimolecular step
58
Reaction intermediate
A species produced in one step then consumed in a subsequent step, not present at beginning or end of reaction
59
A species produced in one step then consumed in a subsequent step, not present at beginning or end of reaction
Reaction intermediate
60
Rate determining step (RDS)
Slowest step of reaction. Product production cannot happen any faster than this step. Has the largest activation energy. Rate law of overall reaction is equal to rate law of this step
61
Slowest step of reaction. Product production cannot happen any faster than this step. Has the largest activation energy. Rate law of overall reaction is equal to rate law of this step
Rate determining step (RLS)
62
Validation of mechanism
Not proving it. Elementary steps sum to the overall reaction. Rate law of predicted mechanism is consistent with observed rate law
63
Not proving it. Elementary steps sum to the overall reaction. Rate law of predicted mechanism is consistent with observed rate law
Validation of mechanism
64
Catalysts
Affect reaction rate (speed) positively or negatively. Not consumed in a reaction (used then remade). Chemical in nature.
65
Affect reaction rate (speed) positively or negatively. Not consumed in a reaction (used then remade). Chemical in nature.
Catalysts
66
Homogenous catalyst
Present in the same phase
67
Present in the same phase as reactants
Homogenous catalysts
68
Heterogeneous catalysts
Present in a different phase
69
Present in a different phase than reactants
Heterogeneous catalyst
70
Positive catalysts
Speed up the reaction
71
Speed up the reaction
Positive catalysts
72
Inhibitors
Slow a reaction (negative catalysts)
73
Slow a reaction (negative catalysts)
Inhibitors

Chemistry 115 (8 decks)

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