Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What are the factors affecting reaction rate?

A
  1. Concentration
  2. Physical State
  3. Temperature
  4. Catalysts
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

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

A

increased

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

The more ready molecules collide with each other,

A

the more rapid they react

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Raising the temperature increases the

A

number and the energy of collisions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Molecules must collide with enough energy to

A

react

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

are agents that increase reaction rates without being
used up.

A

catalysts

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Catalysts catalyze chemical reaction rates by lowering the

A

activation energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

is the energy needed for the chemical
reaction to begin.

A

activation energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

is a change in some variable per unit time.

A

Rate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

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

A

Reaction Rate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Reactant concentration decrease as

A

solution concentration increase

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

is the reaction rate between any two intervals.

A

Average Rate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

is the reaction rate at a specific point in
time.

A

Instantaneous rate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

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

A

Initial rate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

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

A

rate law

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

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

A

Manometric methods

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

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

A

pressure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

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

A

Direct Chemical Methods

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

The sequence of elementary steps that leads to product formation is the

A

reaction mechanism

39
Q

is always formed in an early elementary step and consumed in a later elementary step.

A

intermediate

40
Q

is the number of molecules reacting in an elementary step.

A

Molecularity of a reaction

41
Q

elementary step with 1 molecule

A

Unimolecular reaction

42
Q

elementary step with 2 molecule

A

Bimolecular reaction

43
Q

elementary step with 3 molecule

A

Termolecular reaction

44
Q

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

A

rate-determining step

45
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.
46
Q

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

A

Collision model

47
Q

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

A

Svante Arhenius

48
Q

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

A

slower the reaction

49
Q

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

A

molecular orientation during collisions

50
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.
51
Q

what are the types of catalysts?

A
  1. Homogeneous catalyst
  2. Heterogeneous catalyst
52
Q

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

A

Homogeneous Catalyst

53
Q

exists in a different phase, usually as
a solid.

A

Heterogeneous Catalyst

54
Q

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

A

Adsorption

55
Q

refers to the
penetration of one substance into another.

A

Absorption

CHM012 (13 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions