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AP Chemistry Unit 5 Review

Total questions: 67

Worksheet time: 1hrs 17mins

Name
Class
Date
1.
a)
A. is most exothermic
b)
B. is most exothermic
c)
C. is most exothermic
d)
D. is most exothermic
2.
Consider the following rate law: Rate = k[A]n[B]m
How are the exponents n and m determined?
a)
by using balanced chemical equation
b)
By using the subscripts for the formulas
c)
By educated guess
d)
By experiment 
3.

Ignoring D, which has the largest Ea?

a)

A. has largest Ea

b)

B. has largest Ea

c)

C. has largest Ea

d)

E. has largest Ea

4.
step 1: O3 → O2 + O
step 2: O3 + O → 2 O2

The oxygen atom (O) is considered to be a(n)...
a)
reactant
b)
catalyst
c)
reaction intermediate
d)
activated complex
5.
a)

rate = k[CO]2[O2]2

b)

rate = k[CO]2[O2]

c)

rate = k[CO][O2]2

d)

rate = k[CO][O2]1/2

6.
Multi-step (Consecutive) Reactions:
Mechanisms in which one elementary step is followed by another are very common.
step 1:              A + B → Q
step 2:              B + Q → C
net reaction:    A + 2B → C
Which of the following is false?
a)
The net reaction is just the sum of its elementary steps.
b)
The species Q is an intermediate, usually an unstable or highly reactive species. 
c)
Intermediates such as Q can appear in the rate law of a net reaction.
d)
If both steps proceed at similar rates, rate law experiments on the net reaction would not reveal that two separate steps are involved here.The rate law for the reaction would berate=k[A][B]2
7.
The rate law for a reaction is rate = k [A][B]2 Which one of the following statements is false? 
a)
A) If [B] is doubled, the reaction rate will increase by a factor of 4. 
b)
B) The reaction is second order in B.
c)
C) The reaction is first order in A.
d)
D) The reaction is second order overall.
8.

The graph shown depicts the relationship between concentration and time. What is the slope of this line?

a)

-k

b)

-1/k

c)

k

d)

ln[A]o

9.

What is the rate law for this reaction?

a)

rate = k[X]0

b)

rate = k[X]

c)

rate = k[X]2

d)

rate = -k[X]2

10.
The reaction of (CH3)3CBr with hydroxide ion proceeds:
(CH3)3CBr(aq) + OH-(aq) → (CH3)3COH(aq) + Br-(aq)
What will the initial rate (in mol/L*s) be in Experiment 4?
a)
0.003
b)
0.006
c)
0.009
d)
0.018
11.
a)
IO-, because it was used as a reactant in an earlier step and reproduced in a subsequent step
b)
I-, because it was used as a reactant in an earlier step and reproduced in a subsequent step
c)
IO-, because it was produced in an earlier step and used up in a subsequent step
d)
I-, because it was produced in an earlier step and used up in a subsequent step
12.
Under the collision theory, the particles must collide with  ____ and ____ for a reaction to occur.
a)
sufficient rate and sufficient energy
b)
sufficient surface area and correct orientation
c)
sufficient catalyst and sufficient energy
d)
sufficent energy and correct orientation
13.
Under the collision theory, the particles must collide with  ____ and ____ for a reaction to occur.
a)
sufficient rate and sufficient energy
b)
sufficient surface area and correct orientation
c)
sufficient catalyst and sufficient energy
d)
sufficent energy and correct orientation
14.

Given the following rate law,

rate = k[A]2[B]

if [A] were doubled, what must happen to [B] to keep the rate constant?

a)

[B] must quadruple

b)

[B] must double

c)

[B] must be havled

d)

[B] must be quartered

15.
A possible rate law for a third overall order of a reaction is __________________
a)
Rate = k [A]2[B]2
b)
Rate = k [A][B]3
c)
Rate = k [A]3 [B]
d)
Rate = k [A]2[B]
16.

The following data were measured for the reaction

BF3(g) + NH3(g) ⟶ F3BNH3(g)

What is the rate law for the reaction?

a)

rate = k[NH3]

b)

rate = k[BF3]2[NH3]

c)

rate = k[BF3][NH3]

d)

rate = k[BF3][NH3]2

17.

The catalyst alters the rate of a chemical reaction by,

a)

providing an alternative pathway with a lower Ea

b)

changing the products formed in the direction of the reaction

c)

providing a surface on which the molecules react

d)

increasing the frequencies of collisions between molecules

18.

What would the rate constant of the reaction be given the following set of experiments?

a)
b)
c)
d)
19.
a)

rate = k[CO]2[O2]2

b)

rate = k[CO]2[O2]

c)

rate = k[CO][O2]2

d)

rate = k[CO][O2]1/2

20.
A catalyst:
a)
should be eliminated when we solve elementary reaction steps of a proposed reaction mechanism simultaneously
b)
should always be introduced and eliminated in the first elementary step of a proposed reaction mechanism
c)
lowers the amount of energy released by an exothermic reaction
d)
lowers the amount of energy added to a reaction 
21.
Increasing temperature of a chemical reaction:
a)
increases the number of collisions per second of chemical reactants
b)
increases the speed of reaction
c)
can increase the pressure of reactants
d)
all of the above
22.
For a 1st order reaction, the half-life ("t1/2") is equal to:
a)
t1/2 = 0.693/k
b)
t1/2 = k/0.693
c)
t1/2 = 1/k[A]o 
d)
t1/2 = k 
23.
The mechanism for formation of the product X is:
           A + B -> C + D (slow)
           B + D -> X        (fast)
The intermediate reactant in the reaction is ___. 
a)
A
b)
B
c)
C
d)
D
24.

Suppose the reaction: A + 2B AB2 occurs by the following mechanism: Step 1:  A + B--> AB     slow Step 2:  AB + B -->AB2 fast

Overall: A + 2B --> AB2

The rate law expression must be Rate =______.

a)

(a) k[A]

b)

(b) k[B]

c)

(c) k[A][B]

d)

(d) k[B]2

25.
Consider the following mechanism.
Step 1:     O3        → O2 + O (fast)
Step 2:     O3 + O → 2 O2 (slow)
What is the overall balanced equation?
a)
4 O3 → 3 O2
b)
  O3 → 3 O2
c)
3 O3 → 2 O2
d)
2 O3 → 3 O2
26.

What is the symbol for the rate constant

(a)  

27.

Reaction Energy Profiles that are Endothermic have ______

a)

-Reactants are lower than products

-Gained Energy

b)

-Reactants are higher than products

-Lost Energy

c)

-Reactants and Products are the same

28.

Reaction Energy Profiles that are Exothermic have _______

a)

-Reactants are lower than products

-Gained Energy

b)

-Reactants are higher than products

-Lost Energy

c)

-Reactants and Products stay the same

29.

Intermediate

a)

Series/Collectio of baby reactions that add up to give a reaction equation

b)

Something created in an early step that is used later on

c)

Appears first as a reaction, regenerated first appear as product after later step

30.

How to find the overall rate of a mechanism

a)

Choose a fast equation with the most compounds

b)

The slowest reaction in the mechanism

c)

The fastest reaction in the mechanism

d)

Findind the overall reaction and using it to find the overall rate

31.

In a Multistep reaction energy profile, Each hill represents an _________

a)

Rate law

b)

Overall Reaction

c)

Elementary step

d)

Not here

32.

What are the 3 ways a Catalyst works

a)

Catalyst could bind to a reactant

-Orient the reactants more favorably

-Create lower energy transition state

-How Enzymes function

b)

Involve Covalent Bonding

-Acid-base catalysts

-Reactant or intermediate

-Introduces new rxn intermediate and new elementary rxns

c)

Surface Catalysts

-Reactant/ Intermediate binds to solid surface

33.

Step 1:2⁢NO⇄(NO)2(fast)

Step 2:(NO)2+O2⇄2NO2(slow)

The elementary steps in a proposed mechanism for the reaction 2 NO(g)+O2(g)→2NO2(g) are represented by the equations above. Which of the following is the rate law for the overall reaction that is consistent with the proposed mechanism?

a)

rate=k[NO]2

b)

rate=k[NO][O2]

c)

rate=k[NO]2[O2]

d)

rate=k[(NO)2][O2]

34.
More collisions correspond to a: 
a)
Faster reaction rate  
b)
Slower reaction rate
c)
Constant reaction rate 
d)
None of the above
35.
Which of the following is NOT a factor affecting reaction rate?
a)
temperature
b)
catalysts
c)
particle size
d)
polarity
36.
Reaction rate means...
a)
amount of product formed
b)
speed of reaction
c)
concentration of reacting particles
d)
combining reactants with products
37.
Decreasing the particle size increases the reaction rate because
a)
It makes particles move faster
b)
It increases the likelihood of collisions with the correct geometry
c)
It decreases the surface area available to react
d)
It increases the number of collisions
38.
What would be my the overall order of this rate law? 
Rate=[A]2[B]1
a)
0 Order
b)
1st Order
c)
2nd Order
d)
3rd Order
39.
What does kinetics mainly study?
a)
concentration of (aq) mixtures 
b)
pressure of (g) mixtures
c)
how much products are produced
d)
reaction rates
40.
A chemical reaction can occur:
a)
if the particles collide with enough energy
b)
if the particles collide with sufficient activation energy
c)
if the particles collide with correct orientation
d)
all of the above
41.
A "zeroth" order reaction for A-->B, will show:
a)
a straight line for a graph: time vs. ln [A]
b)
a straight line for a graph:  time vs. [A].
c)
a straight line for a graph:  time vs. 1/[A]
d)
none of the above
42.
A first order rate law for reaction A--> B will match a graph:
a)
which looks linear and positive in slope for time vs. ln [A].
b)
which looks non-linear and positive in slope for time vs. ln [A].
c)
which looks non-linear and negative in slope for time vs. ln [A].
d)
which looks linear and negative in slope for time vs. ln [A].
43.
A 2nd  order rate law for reaction A--> B will match a graph:
a)
which looks linear and positive in slope for time vs. 1/ [A].
b)
which looks linear and negative in slope for time vs. 1/ [A].
c)
which looks non-linear and positive in slope for time vs. 1/ [A].
d)
which looks non-linear and negative in slope for time vs. 1/[A].
44.

The minimum energy to break bonds in kinetics is called the...

a)

bond strength

b)

IMFs

c)

bond energy

d)

activation energy

45.

1st order is linear for ______; 2nd order is linear for _______

a)

ln[A] vs time

1/[A] vs time

b)

[A] vs time

ln[A] vs time

c)

1/[A] vs time

ln[A] vs time

d)

1/[A] vs time

[A] vs time

46.

A catalyst _______ the activation energy

a)

raises than lowers

b)

raises

c)

stays the same

d)

lowers

47.

If you increase the temperature, there are _____ collisions AND _____ of them have the ______ activation energy.

a)

less

less

minimum

b)

more

less

maximum

c)

more

more

minimum

d)

less

more

maximum

48.

The taller the "hill" (or activation energy) the _____ the reaction.

a)

Faster

b)

Slower

c)

same speed

d)

faster than slower

49.

Catalysts are_______

a)

Used up in one step and produced in a later step

b)

Produced in one step and used up in a later step

c)

Not used in the steps

d)

Produced in one step and left alone in the next step

50.

What step indicates the speed of the reaction and rate law?

a)

Fast step

b)

No steps

c)

Medium step

d)

Slow step

51.

If you increase the pressure of gases, you _____ the concentration of the gas, so there are ______ collisions.

a)

Increase

less

b)

Decrease

less

c)

Increase

more

d)

Decrease

more

52.

Which one is endothermic and which is exothermic?

a)

The left one is exothermic

The right one is endothermic

b)

Both are endothermic

c)

Both are exothermic

d)

The left one is endothermic

The right one is exothermic

53.

Examine the following proposed mechanism for 2H2O2 --> 2H2O+O2

Step 1: H2O2+I- --> H2O+IO- (slow)

Step 2: H2O2+IO- --> H2O+O2+I- (fast)

Select the correct statement below:

a)

H2O and IO- are intermediates

b)

IO- is an intermediate and I- is a catalyst

c)

IO- and I- are intermediates

d)

There are no intermediates or catalysts in this mechanism

54.

Which letter represents the activation energy?

a)

A

b)

B

c)

C

d)

D

e)

E

55.

Which letter 
represent the intermediates?

a)

A

b)

B

c)

C

d)

D

e)

E

56.

Which letter represent the reactants?

a)

A

b)

B

c)

C

d)

D

e)

E

57.

Which letter represents the products?

a)

A

b)

B

c)

C

d)

D

e)

E

58.

Which letter represents the  ΔH\Delta H  ?

a)

A

b)

B

c)

C

d)

D

e)

E

59.

Is this endothermic or exothermic?

a)

Endothermic

b)

Exothermic

60.

Which order of reaction is has a positive slope?

a)

first order

b)

second order

c)

zeroth order

61.

What is the order for the Br ion?

a)

zeroth

b)

first

c)

second

62.

What is the order for the BrO3 ion?

a)

zeroth

b)

first

c)

second

63.

What is the order of the H3O ion?

a)

zeroth

b)

first

c)

second

64.

What was the overall order?

(a)  

65.

What is the overall reaction?

a)

H22ICl→2HCl+I2H_22ICl→2HCl+I_2

b)

H+ICl→HCl+IH+ICl→HCl+I

c)

K[BrO3]1[Br]1[H3O]2K\left[BrO_3\right]^1\left[Br\right]^1\left[H_3O\right]^2

66.

What is/are the intermediates in the reaction?

a)

Pt

b)

H

c)

HCl

d)

I

67.

What is the catalyst in the reaction?

a)

H

b)

Pt

c)

HCl

d)

I

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