TOPIC 8- CHEMICAL KINETICS Flashcards

1
Q

the area of chemistry concerned with the
speeds, or rates, at which a chemical reaction occurs.

A

Chemical Kinetics

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2
Q

refers to the rate of a reaction, or the reaction rate which is the change in the concentration of a product or reactant with time.

A

Kinetics

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3
Q

What are the factors affecting reaction rate?

A
  1. Concentration
  2. Physical State
  3. Temperature
  4. Catalysts
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4
Q

Most chemical reactions proceed faster if the concentration
of one or more of the reactants is

A

increased

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5
Q

The more ready molecules collide with each other,

A

the more rapid they react

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6
Q

Raising the temperature increases the

A

number and the energy of collisions

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7
Q

Molecules must collide with enough energy to

A

react

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8
Q

are agents that increase reaction rates without being
used up.

A

catalysts

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9
Q

Catalysts catalyze chemical reaction rates by lowering the

A

activation energy

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10
Q

is the energy needed for the chemical
reaction to begin.

A

activation energy

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11
Q

is a change in some variable per unit time.

A

Rate

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12
Q

is the change in concentrations of reactants or
product in a chemical reaction per unit time.

A

Reaction Rate

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13
Q

Reactant concentration decrease as

A

solution concentration increase

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14
Q

is the reaction rate between any two intervals.

A

Average Rate

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15
Q

is the reaction rate at a specific point in
time.

A

Instantaneous rate

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16
Q

is the instantaneous rate at the moment the
reactants are mixed.

A

Initial rate

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17
Q

expresses the rate as a function of reactant
concentrations and temperature.

A

rate law

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18
Q

are used to measure the concentration
of a reactant or product that absorbs (or emits) light of a narrow
range of wavelengths.

A

spectrometric methods

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19
Q

are used to measure the rate when
nonionic reactants for ionic products, or vice versa since the
conductivity of the solution changes over time.

A

Conductometric methods

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20
Q

are used if the reaction involves a
change in the number of moles of gas.

A

Manometric methods

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21
Q

In manometric methods, The rate can be determined from the change in ___________
(at constant volume and temperature) over time.

A

pressure

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22
Q

are used to measure the rates of
slow reactions, or of those that can be easily slowed.

A

Direct Chemical Methods

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23
Q

A small, measured portion called _______ of the reaction
mixture is removed, and the reaction in this portion is
stopped by rapid cooling.

24
Q

We can
determine the reaction order and then the rate constant of the
reaction from

A

reactant concentration

25
Note that the exponents of L and mol in the unit of the rate constant is equal to the
overall reaction order minus one
26
enable us to calculate the rate of a reaction from the rate constant and reactant concentrations
Rate law expressions
27
The rate laws can also be used to determine the concentrations of reactants at anytime during a reaction by employing different forms,
integrated rate laws
28
These are reactions whose rate depends on the reactant concentration raised to the first power.
First Order Rate Laws
29
are reactions whose rate depends on the concentration of one reactant raised to the second power or on the concentrations of two different reactants, each raised to the first power.
Second Order Rate Laws
30
These are reactions whose rate is a constant, independent of reactant concentration.
Zeroth Order Rate Laws
31
time required for the reactant concentration to reach half its initial value.
Half-life of a reaction
32
is a constant, independent of reactant concentration.
Half-life of a First-Order Reaction
33
does depend on reactant concentration and the half-life is inversely proportional to the initial concentration.
Half-life of a second-order reaction
34
is directly proportional to the initial reactant concentration.
Half-Life of a Zero-Order Reaction
35
Most chemical reactions occur by a series of steps called the
reaction mechanism
36
a species that is canceled from both sides of the reaction (not a reactant or product.)
intermediate
37
Each of these two reactions is called an
elementary Step
38
The sequence of elementary steps that leads to product formation is the
reaction mechanism
39
is always formed in an early elementary step and consumed in a later elementary step.
intermediate
40
is the number of molecules reacting in an elementary step.
Molecularity of a reaction
41
elementary step with 1 molecule
Unimolecular reaction
42
elementary step with 2 molecule
Bimolecular reaction
43
elementary step with 3 molecule
Termolecular reaction
44
The rate law of a reaction mechanism is derived from the slowest step called
rate-determining step
45
A reaction mechanism must satisfy the following:
1. The sum of the elementary steps must give the overall balanced equation for the reaction. 2. The mechanism must agree with the experimentally determined rate law.
46
is built around the central idea that molecules must collide to react.
Collision model
47
proposed the existence of the activation energy that must be overcome to produce a chemical reaction.
Svante Arhenius
48
The higher the activation energy, the ___________________ at a given temperature.
slower the reaction
49
Many collisions, even though they have the required energy, still do not produce a reaction due to
molecular orientation during collisions
50
Two requirements must be satisfied for reactants to collide:
1. The collision must involve enough energy to produce the reaction; that is, the collision energy must equal or exceed the activation energy. 2. The relative orientation of the reactants must allow formation of any new bonds necessary to produce products.
51
what are the types of catalysts?
1. Homogeneous catalyst 2. Heterogeneous catalyst
52
is one that is present in the same phase as the reacting molecules.
Homogeneous Catalyst
53
exists in a different phase, usually as a solid.
Heterogeneous Catalyst
54
refers to the collection of one substance on the surface of another substance
Adsorption
55
refers to the penetration of one substance into another.
Absorption