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Chemistry 115 > Chapter 13 > Flashcards

Chapter 13 Flashcards

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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
Q

Zero order

A

Reaction rate is independent of reactant concentration.

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26
Q

Reaction rate is independent of reactant concentration.

A

Zero order

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27
Q

Integrated rate law

A

Dependance of concentration of reactants on time

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28
Q

Dependance of concentration of reactants on time

A

Integrated rate law

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29
Q

Half life

A

Time it takes for reactants to react to half their original concentration

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30
Q

Time it takes for reactants to react to half their original concentration

A

Half life

31
Q

First order half life

A

Independent of initial concentration

32
Q

Independent of initial concentration

A

First order half life

33
Q

Increase in temperature during a reaction

A

Increases reaction rate

34
Q

Increase of 10•C

A

Doubles reaction rate

35
Q

Temperatures affects on reaction rate

A

As one increases the other does as well

36
Q

Frequency factor

A

2 factors including collision frequency factor (z), and orientation factor (p)

37
Q

2 factors including collision frequency factor (z), and orientation factor (p)

A

Frequency factor

38
Q

Collision frequency factor (z)

A

Frequent and energetic collisions must occur to break bonds. Kinetic energy must be sufficient

39
Q

Frequent and energetic collisions must occur to break bonds. Kinetic energy must be sufficient

A

Collision frequency factor (z)

40
Q

Orientation factor (p)

A

Molecules must come into contact at the right spot to make new bonds. More complex molecules collide with the proper orientation less frequently

41
Q

Molecules must come into contact at the right spot to make new bonds. More complex molecules collide with the proper orientation less frequently

A

Orientation factor (p)

42
Q

Activated complex or transition state

A

Effective collision, when unstable chemical species is formed

43
Q

Effective collision, when unstable chemical species is formed

A

Activated complex or transition state

44
Q

Reaction mechanics

A

Most reactions happen in small steps between two molecules.

45
Q

Most reactions happen in small steps between two molecules.

A

Reaction mechanics

46
Q

Reaction mechanism

A

Outline of observed steps in a reaction

47
Q

Outline of observed steps in a reaction

A

Reaction mechanism

48
Q

Elementary step

A

A small reaction part of a full reaction. Rate law is determined by stoichiometry

49
Q

A small reaction part of a full reaction. Rate law is determined by stoichiometry

A

Elementary step

50
Q

Molecularity

A

Number of reactant particles in an elementary step

51
Q

Number of reactant particles in an elementary step

A

Molecularity

52
Q

Unimolecular step

A

One reactant present

53
Q

One reactant present

A

Unimolecular

54
Q

Bimolecular

A

Involves 2 reactant particles of the same species, or of different species

55
Q

Involves 2 reactant particles of the same species, or of different species

A

Bimolecular step

56
Q

Temoleculer step

A

Three reactant particles, extremely rare

57
Q

Three reactant particles, extremely rare

A

Trimolecular step

58
Q

Reaction intermediate

A

A species produced in one step then consumed in a subsequent step, not present at beginning or end of reaction

59
Q

A species produced in one step then consumed in a subsequent step, not present at beginning or end of reaction

A

Reaction intermediate

60
Q

Rate determining step (RDS)

A

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
Q

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

A

Rate determining step (RLS)

62
Q

Validation of mechanism

A

Not proving it. Elementary steps sum to the overall reaction. Rate law of predicted mechanism is consistent with observed rate law

63
Q

Not proving it. Elementary steps sum to the overall reaction. Rate law of predicted mechanism is consistent with observed rate law

A

Validation of mechanism

64
Q

Catalysts

A

Affect reaction rate (speed) positively or negatively. Not consumed in a reaction (used then remade). Chemical in nature.

65
Q

Affect reaction rate (speed) positively or negatively. Not consumed in a reaction (used then remade). Chemical in nature.

A

Catalysts

66
Q

Homogenous catalyst

A

Present in the same phase

67
Q

Present in the same phase as reactants

A

Homogenous catalysts

68
Q

Heterogeneous catalysts

A

Present in a different phase

69
Q

Present in a different phase than reactants

A

Heterogeneous catalyst

70
Q

Positive catalysts

A

Speed up the reaction

71
Q

Speed up the reaction

A

Positive catalysts

72
Q

Inhibitors

A

Slow a reaction (negative catalysts)

73
Q

Slow a reaction (negative catalysts)

A

Inhibitors

Chemistry 115 (8 decks)

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