Brainscape's Knowledge GenomeTM

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


See full index

AP Chemistry > Chapter 12 > Flashcards

Chapter 12 Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

Chemical kinematics

A

The study of the speed that reactants are converted to products in a chemical reaction.

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

Factors that have a role in the speed of a reaction and its effectiveness

A

state of matter, particle size, temperature, concentration, presence of catalyst

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

Spontaneity is not related to?

A

speed

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

Spontaneity

A

a measurement of possibility that the reaction will happen at the current conditions

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

What is maintained when a reactant is converted into a product in a chemical reaction?

A

stoichiometry ratio

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

Reaction rate is based on?

A

a change in concentration over time

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

Rate always _______ with time

A

decreases

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

Why do expressions involving reactants have negative values?

A

because rate always decreases with time

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

Calculated rates will always have?

A

positive values

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

Rates do not have to be?

A

constant

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

Rates follow an?

A

pattern or predictable pathway

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

The reverse reaction affects?

A

the rate of change in concentrations

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

If we take the reverse reaction into consideration, the overall change in concentration depends on?

A

the difference in the rates of the forward and reverse reaction

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

What is the issue when looking at reverse reactions?

A

where to study the reactions when looking to calculate a rate law

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

To avoid confusion, we study the rate of a reaction under what kind of conditions?

A

where the reverse reaction is negligible

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

The rate law depends on?

A

REACTANTS ONLY

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

Rates will be ______ rates.

A

instantaneous

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

instantaneous rates will be measured at a time where?

A

the reverse reaction has not contributed to the overall rate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

In the rate equation, O order means?

A

there is a catalyst

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

The rate equation is _____ dependent.

A

reactant

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

In the rate equation, the order of the reactant is determined how?

A

experimentally via data and calculations

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

In the rate equation, k is?

A

the proportionality constant or rate constant.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

In the rate equation, n is?

A

the order of the reactant

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

In the rate equation, the integer value can be?

A

0 or even a fraction.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

What are the types of rate laws?

A

differential and integrated

26
Q

differential rate law is also called?

A

rate law

27
Q

differential rate law involves only?

A

reactant concentrations

28
Q

integrated rate law involves only?

A

time and entire reaction

29
Q

differential rate law

A

expresses how the rate of a reaction is dependent on the concentration of the elements or compounds in the experiment.

30
Q

integrated rate law

A

expresses how the concentration of a species in a reaction changes with time.

31
Q

species

A

reactant or product

32
Q

choice of rate law type depends on?

A

what data is easiest to collect.

33
Q

the value of n also tells us?

A

what power to raise the law to

34
Q

3 options of integrated rate law?

A

0, 1, 2

35
Q

reaction mechanism

A

series of steps a reaction takes

36
Q

2 key components of a reaction mechanism

A

must use a balanced equation and mechanisms have to match the rate law

37
Q

intermediates

A

elements or compounds formed and consumed during a reaction that do not make it in the final equation.

38
Q

When looking at rate orders you should not pay attention to?

A

stoichiometry ratio

39
Q

elementary steps

A

unfinished reaction mechanism

40
Q

molecularity

A

the number of species that must collide to produce the reaction indicated by that step

41
Q

unimolecular step

A

a reaction involving 1 molecule

42
Q

bimolecular step

A

a reaction involving the collisions of two species

43
Q

termolecular step

A

a reaction involving the collisions of three species

44
Q

Which is the most important step?

A

rate determining step

45
Q

Rate determining step

A

slowest step in the process and all reactions must get past this step before they can produce products

46
Q

the rate determining step determines

A

the rate for the reaction

47
Q

collision model

A

molecules must collide in order to react, they must collide with sufficient energy and proper orientation

48
Q

In the collision model, if the proper conditions are not met the molecules will?

A

attempt to react again until they get things right

49
Q

activation energy

A

the energy required to convert atoms or molecules to the activated complex

50
Q

activated complex

A

transition state

51
Q

the activation energy is the minimum energy required for?

A

an effective collision

52
Q

The activation energy value is influenced by factors such as

A

temperature, catalysts, and pressure

53
Q

catalysts

A

substances that speed up a reaction without being consumed or changed themselves

54
Q

Catalysts are mostly?

A

metals

55
Q

catalysts can also?

A

lower activation energy and keep rate constant

56
Q

heterogeneous catalysis

A

scenario where the catalyst is in a different phase than the reacting substances

57
Q

heterogeneous catalysis are usually?

A

gaseous reactants on a solid surface

58
Q

uses of a heterogeneous catalysis

A

-conversion of alkenes to alkanes
-conversion of CO and NO in auto exhaust to CO₂ and N₂
-process is referred to as adsorption

59
Q

homogeneous catalysis

A

reactants and catalysts are in the same phase

60
Q

example of homogeneous catalysts

A

decomposition of Ozone by CFC’s

AP Chemistry (16 decks)

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