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CHM012 > TOPIC 8- CHEMICAL KINETICS > Flashcards

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 f 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

22
Q

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

A

Direct Chemical Methods

23
Q

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

A

aliquot

24
Q

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

A

reactant concentration

25
Q

Note that the
exponents of L and mol in the unit of the rate constant is equal to the

A

overall reaction order minus one

26
Q

enable us to calculate the rate of a reaction
from the rate constant and reactant concentrations

A

Rate law expressions

27
Q

The rate laws can also be used to determine the concentrations
of reactants at anytime during a reaction by employing different
forms,

A

integrated rate laws

28
Q

These are reactions whose rate depends on the reactant concentration
raised to the first power.

A

First Order Rate Laws

29
Q

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.

A

Second Order Rate Laws

30
Q

These are reactions whose rate is a constant, independent of reactant
concentration.

A

Zeroth Order Rate Laws

31
Q

time required for the reactant
concentration to reach half its initial value.

A

Half-life of a reaction

32
Q

is a constant, independent of
reactant concentration.

A

Half-life of a First-Order Reaction

33
Q

does depend on reactant
concentration and the half-life is inversely proportional to the initial
concentration.

A

Half-life of a second-order reaction

34
Q

is directly proportional to the initial reactant concentration.

A

Half-Life of a Zero-Order Reaction

35
Q

Most chemical reactions occur by a series of steps called the

A

reaction mechanism

36
Q

a species that is canceled from
both sides of the reaction (not a reactant or product.)

A

intermediate

37
Q

Each of these two reactions is called an

A

elementary Step

38
Q

is defined as the number of species that must
collide to produce the reaction indicated by that step.

A

Molecularity

39
Q

The rate law of a reaction mechanism is derived from the
slowest step called

A

rate-determining step

40
Q

A reaction mechanism must satisfy the following:

A
  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.
41
Q

is built around the central idea that
molecules must collide to react.

A

Collision model

42
Q

proposed the existence of the activation
energy that must be overcome to produce a chemical reaction.

A

Svante Arhenius

43
Q

The higher the activation energy, the ___________________ at a
given temperature.

A

slower the reaction

44
Q

Many collisions, even though they have the required energy, still
do not produce a reaction due to

A

molecular orientation during collisions

45
Q

Two requirements must be satisfied for reactants to collide:

A
  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.
46
Q

what are the types of catalysts?

A
  1. Homogeneous catalyst
  2. Heterogeneous catalyst
47
Q

is one that is present in the same
phase as the reacting molecules.

A

Homogeneous Catalyst

48
Q

exists in a different phase, usually as
a solid.

A

Heterogeneous Catalyst

49
Q

refers to the collection of one substance on the
surface of another substance

A

Adsorption

50
Q

refers to the
penetration of one substance into another.

A

Absorption

CHM012 (9 decks)

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