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Chemistry 1040 - NSULA Fall 2016 > Chapter 14 - Chemical Kinetics > Flashcards

Chapter 14 - Chemical Kinetics Flashcards

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1
Q

What is studied in chemical kinetics?

A

the rate (or speed) at which a chemical process occurs

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2
Q

Define reaction mechanism.

A

a molecular-level view of the path from reactants to products

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3
Q

List four factors that affect reaction rates.

A
  1. Physical state of the reactants.
  2. Reactant concentrations.
  3. Reaction temperature.
  4. Presence of a catalyst.
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4
Q

The more readily the reactants collide, the more (rapidly/slowly) they react.

A

rapidly

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5
Q

Homogeneous reactions are often (faster/slower).

A

faster

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6
Q

Heterogeneous reactions that involve solids are faster if the surface area is (increased/decreased).

A

increased

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7
Q

Increases reactant concentration generally (increases/decreases) reaction rate.

A

increases

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8
Q

Why does increasing reaction concentration generally increase reaction rate?

A

Since there are more molecules, more collisions occur.

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9
Q

Reaction rate generally (increases/decreases) with increased temperature.

A

increases

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10
Q

_____ energy of molecules is related to temperature.

A

kinetic

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11
Q

At (higher/lower) temperatures, molecules move more quickly, (increasing/decreasing) numbers of collisions and the energy of the molecules possesses during the collisions.

A

higher, increasing

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12
Q

Catalysts affect rate (while/without) being in the overall balanced equation.

A

without

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13
Q

Catalysts affect the __________, changing the individual reactions that are part of the pathway from reactants to products.

A

kinds of collisions

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14
Q

Define rate.

A

a change in concentration over a time period Δ[ ]/Δt

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15
Q

Define Δ in the statement Δ[ ]/Δt.

A

change in

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16
Q

Define [ ] in the statement Δ[ ]/Δt.

A

molar concentration

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17
Q

Define t in the statement Δ[ ]/Δt.

A

time

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18
Q

List three types of rate measured.

A
  1. Average rate.
  2. Instantaneous rate.
  3. Initial rate.
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19
Q

How is the rate of a reaction measured?

A

using the concentration of a reactant or a product over time

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20
Q

How is a plot graph of reaction rate data useful?

A

it gives more information about the rate

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21
Q

What does the slope of the curve at one point in time on a rate data graph tell us?

A

the instantaneous rate

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22
Q

Define initial rate.

A

the instantaneous rate at time zero on a rate data graph

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23
Q

How do we determine what effect the concentration of each reactant has on the rate of the reaction?

A

We keep every concentration constant except for one reactant and see what happens to the rate. Then we change a different reactant. We do this until we have seen each reactant has affected the rate.

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24
Q

Define rate law as stated by the equation rate= k[A]^x[B]^y.

A

a statement of the relationship between rate and concentration for all reactions

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25
Q

Define k in the statement rate=k[A]^x[B]^y.

A

the rate constant

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26
Q

What is the rate constant dependent on?

A

temperature

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27
Q

Define the exponents in the statement rate=k[A]^x[B]^y.

A

the order of the reaction with respect to each reactant

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28
Q

How is the overall reaction’s order determined?

A

by adding up all of the reactants’ orders

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29
Q

Define [A] and [B] in the statement rate=k[A]^x[B]^y.

A

the reaction rates of reactants [A] and [B]

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30
Q

Define first order reactions.

A

reaction rates that depend only on one reactant to the first power

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31
Q

What is the rate law for a first order reaction?

A

rate=k[A]

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32
Q

How is k related to [A] in a first order reaction?

A 
rate = k [A]
rate = −Δ [A] / Δt
So:  k [A]  = −Δ [A] / Δt
Rearrange to:  Δ [A] / [A]  =  − k Δt
Integrate:  ln ([A] / [A]o)  =  − k t
Rearrange:  ln [A]  =  − k t  +  ln [A]o
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33
Q

How does a plot of ln [A] vs t appear?

A

linear

34
Q

How can a rate constant be found from a plot of ln [A] vs. t?

A

When the integrated rate law, ln [A] = − k t + ln [A]o, is plotted as a line, its slope will equal -k.

35
Q

Define half life.

A

the amount of time it takes for one half of a reactant to be used up in a chemical reaction

36
Q

How is half-life calculated in a first order reaction?

A 
ln [A]  =  − k t  +  ln [A]o 
ln ([A]o/2)  =  − k t½  + ln [A]o 
− ln ([A]o/2)  +  ln [A]o  =  k t½
ln ([A]o / [A]o/2)  =  k t½ 
ln 2  = k t½   or t½ = 0.693/k
37
Q

Define second order reaction.

A

a reaction rate that depends only on a reactant to the second power

38
Q

What is the rate law for a second order reaction?

A

rate=k[A]^2

39
Q

How is k related to [A] for a second order reaction?

A 
rate = k [A]^2 
rate = − Δ [A] / Δ t
So, k [A]2 = − Δ [A] / Δ t
Rearranging:  Δ [A] / [A]2  =  − k  Δ t
Using calculus:  1/[A] = 1/[A]o + k t
40
Q

How is half-life derived in a second order reaction?

A 
Using the integrated rate law, we can see how half-life is derived:
1/[A] = 1/[A]o + k t
1/([A]o/2)  =  1/[A]o + k t½
2/[A]o −1/[A]o  =  k t½ 
t½  =  1 / (k [A]o)
41
Q

Half-life is a ____________ dependent quantity for second order reactions.

A

concentration

42
Q

Define zero order reaction.

A

a reaction in which the reaction rate is independent of the concentration of the reactant

43
Q

Zero order reactions are _________ in concentration.

A

linear

44
Q

The rate constant is temperature dependent; it (increases/decreases) as temperature increases.

A

increases

45
Q

Rate constant _____ (approximately) with every 10 C temperature increase.

A

doubles

46
Q

The collision model is based on the _________ theory.

A

kinetic molecular

47
Q

Molecules must _____ to react.

A

collide

48
Q

If there are more ______, more ______ can occur. If there are _____ molecules, the __________ is faster.

A

collisions, reactions

more, reaction rate

49
Q

If the temperature is higher, molecules move _______, causing more collisions and a ____________ of reaction.

A

faster, higher rate

50
Q

What occurs in a chemical reaction?

A

bonds are broken and new bonds are formed

51
Q

Molecules can only react ___________.

A

if they collide with each other

52
Q

Can molecules collide without forming products?

A

yes

53
Q

Define activation energy.

A

the minimum energy needed for a reaction to take place

54
Q

What must be overcome for a reaction to take place?

A

an energy barrier

55
Q

Reactants gain ______ as the reaction proceeds until the particles reach the _______________.

A

energy, maximum energy state

56
Q

Define transition state.

A

the organization of the atoms at the maximum energy state

57
Q

Name another term for transition state.

A

activated complex

58
Q

What is the energy needed to form a transition state?

A

activation energy

59
Q

Reactions can be _____ or _____ after the transition state is formed.

A

endothermic, exothermic

60
Q

Gases have an average temperature, but each individual molecule has ________.

A

its own energy

61
Q

At __________, more molecules possess the energy needed for the reaction to occur.

A

higher energies

62
Q

Define the Arrhenius equation.

A

the relationship between activation energy as temperature stated as k = Ae−Ea/RT

63
Q

How can activated energy be determined graphically using the Arrhenius equation?

A

by reorganizing the equation ln k = −Ea/RT + ln A

64
Q

Define reaction mechanism.

A

a series of stepwise reactions that show how reactants become products

65
Q

What are the individual steps of a reaction mechanism called?

A

an elementary reaction or elementary process

66
Q

Define molecularity.

A

tells how many molecules are involved in that step of the mechanism

67
Q

Nearly all reaction mechanisms use only ___________.

A

unimolecular or bimolecular reactions

68
Q

Termolecular reactions are ________.

A

rare, if they occur at all

69
Q

Define rate-determining state.

A

the slowest reaction in the reaction mechanism

70
Q

What is required of a plausible reaction mechanism?

A

The rate law must be able to be devised from the rate-determining step.
The stoichiometry must be obtained when all steps are added up.
Each step must balance, like any equation.
All intermediates are made and used up.
Any catalyst is used and regenerated.

71
Q

Define catalyst?

A

a component which increases the rate of a reaction by decreasing the activation energy of the reaction

72
Q

Catalysts _________.

A

change the mechanism by which the process occurs

73
Q

List three types of catalysts.

A
  1. Homogeneous catalysts
  2. Heterogeneous catalysts
  3. Enzymes
74
Q

Define homogeneous catalyst.

A

a catalyst in the same phase as the reactant

75
Q

How are many homogeneous catalysts seen?

A

dissolved in the same solvent as the reactant

76
Q

Define heterogeneous catalyst.

A

a catalyst in a different phase then the reactant

77
Q

What is frequently the rate determining step in reactions involving heterogeneous catalysts?

A

the adsorption of the reactants

78
Q

Define enzymes.

A

biological catalysts

79
Q

Define active site.

A

a region on an enzyme where the reactants attach

80
Q

Define substrates.

A

the reactants affected by an enzyme

81
Q

Define the enzyme-substrate model.

A

in the enzyme-substrate model the substrate fits into the active site of an enzyme much like a key fits into a lock

Chemistry 1040 - NSULA Fall 2016 (8 decks)

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