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AP Chemistry unit 5-6 Review

Total questions: 100

Worksheet time: 2hrs 20mins

Name
Class
Date
1.

condensing

a)

exothermic

b)

endothermic

2.
If the reactant particles collide with less than the activation energy, the particles will be rebound, and no reaction will occur.
a)
True
b)
False
3.
Temperature is a measure of the...
a)
total energy in a substance
b)
total kinetic energy in a substance
c)
average potential energy in a substance
d)
average kinetic energy of molecules in a substance
4.
A substance with a high specific heat:
a)
Is always extremely hot.
b)
Requires a lot of energy to become hot.
c)
Is not heavy.
d)
Does not requires a lot of energy to become hot.
5.
The first law of thermodynamics states that energy is
a)
created
b)
destroyed
c)
conserved
d)
created and destroyed
6.
What is the activation energy?
a)
The energy of the products
b)
The energy of the reactants
c)
The minimum energy needed by the reactants to form the products.
d)
The energy lost in the reaction
7.
Which letter corresponds to the energy of the products?
a)
A
b)
B
c)
C
d)
D
8.
Which letter corresponds to the activation energy of the forward reaction?
a)
A
b)
B
c)
C
d)
D
9.
In an endothermic reaction the system is releasing energy.
a)
True
b)
False
10.
Refer the the following question:
2N2 + 3H2 --> 2NH3 + 46 kJ
How much energy would be produced if only 1 mol of nitrogen was reacted?
a)
92 kJ
b)
0.143 kJ
c)
23 kJ
d)
15 kJ
11.

This reaction is most likely

a)

endothermic.

b)

exothermic.

12.

Which change is exothermic?

a)

negative delta H

b)

heat is absorbed by system

c)

temperature decreases

d)

bubbles form

13.

which is exothermic?

a)

temperature decreases

b)

breaking bonds

c)

system releasing heat to surroundings

d)

chemical reaction

14.

Which is exothermic?

a)

temperature decreases

b)

heat is released by system

c)

liquid changes to gas

d)

products are at higher energy than reactants

15.

which is endothermic?

a)

IMFs broken

b)

negative delta H

c)

products are lower energy than reactants

d)

temperature increases

16.

Which substance would be able to absorb the most energy if each sample experiences the same temperature change?

a)

50 grams of aluminum

b)

5 grams of aluminum

c)

150 grams of aluminum

d)

1000 gram of aluminum

17.

Which substance would experience the biggest temperature change if each sample absorbed the same energy?

a)

100 grams of water

b)

25 grams of water

c)

5 grams of water

d)

2500 grams of water

18.

condensing

a)

exothermic

b)

endothermic

19.

2NaCl + 35 kJ --> 2Na + Cl2

a)

exothermic

b)

endothermic

20.

positive delta H

a)

exothermic

b)

endothermic

21.

The specific heat of liquid bromine is 0.2 J/gK. How much heat is required to raise the temperature of 100. grams of bromine from 15 K to 25 K?

a)

30 J

b)

500 J

c)

20 J

d)

200 J

22.

How much heat is released when 36 grams of water is frozen at 0 C? The heat of solidification is 6.02 kJ/mol.

a)

18 kJ

b)

220 kJ

c)

12 kJ

d)

2 kJ

23.

The enthalpy change for 2Na + Cl2 --> 2NaCl is -35 kJ. What is the heat of reaction for 2NaCl --> 2Na + Cl2

a)

- 35 kJ

b)

35 kJ

c)

70 kJ

d)

- 70 kJ

24.

How much heat is released when 3 moles of methane is reacted? CH4 + O2 --> CO2 + H2O + 80 kJ

a)

1300 kJ

b)

0.038 kJ

c)

27 kJ

d)

240 kJ

25.
H2 + Cl2 --> 2 HCl + 1845 kJ
Is this reaction endothermic or exothermic?
a)
Endothermic 
b)
Exothermic
26.
H2 + 2 C + N2 + 270.3 kJ --> 2 HCN
Is this reaction endothermic or exothermic?
a)
Endothermic 
b)
Exothermic
27.
If ΔH is positive, heat would be shown on the _____ side of the thermochemical equation.
a)
Reactant
b)
Product
28.
How much heat does an aluminum block absorb if 10.00 grams ae heated from 25.0oC to 50.0oC? the specific heat of aluminum is .900J/goC
a)
450
b)
-450
c)
225
d)
-225
29.
Some average bond enthalpies, in kJ/mol, are as follows:
H-H = 436
Cl-Cl = 242
H-Cl = 431
What is the enthalpy change for the decomposition of hydrogen chloride?
2 HCl --> H2 + Cl2
a)
-184 kJ
b)
+ 184 kJ
c)
- 247 kJ
d)
+ 247 kJ
30.
The enthalpy change for the reaction
C(s, graphite) + 1⁄2O2(g) --> CO(g) cannot be measured directly since some carbon dioxide is always formed in the reaction.
It can be calculated using Hess’s Law and the enthalpy changes of combustion of graphite and of carbon monoxide.
C(s, graphite) + O2(g) --> CO2    ΔH=-394 kJmol–1
CO(g) + 1⁄2O2(g) --> CO2  ΔH=-283 kJmol–1  
The enthalpy change for the reaction of graphite with oxygen to give carbon monoxide is 
a)
-677 kJmol–1 
b)
+111 kJmol–1 
c)
-111 kJmol–1 
d)
+677 kJmol–1 
31.
The standard enthalpy changes of combustion of carbon, hydrogen and methane are shown in the table. 
 Which one of the following expressions gives the correct value for the standard enthalpy change of formation of methane in kJ mol–1?
C(s) + 2H2(g) → CH4(g) 
a)
394 + (2 × 286) – 891 
b)
–394 – (2 × 286) + 891 
c)
394 + 286 – 891 
d)
–394 – 286 + 891 
32.
During the vaporization of water, the kinetic energy...
a)
increases, while potential energy decreases
b)
increases, while potential energy stays the same
c)
stays the same, while potential energy increases
d)
stays the same, while potential energy decreases
33.

Which 1 g sample will have the highest temperature after the addition of 200 J of energy?

a)

H2O(l)

b)

H2O(g)

c)

Cu

d)

Pb

34.
A 5.00 gram sample of a metal at 85.0 °C comes in contact with 100.0 grams of water at 25.0 °C.  What is the direction of the heat flow and why?
a)
Metal to water, since heat flows from low mass to high mass
b)
Water to metal, since heat flows from high mass to low mass
c)
Metal to water, since heat flows from high temp. to low temp.
d)
Water to metal, since heat flows from low temp. to high temp.
35.
If 5.00 grams of water is cooled from 65.2 °C to 35.6 °C, what is the heat change?
a)
619 J
b)
-619 J
c)
148 J
d)
-148 J
36.
If 2.50 grams of a solute are added to    50.0 grams of water, the temperature increases by 4.5 °C.  Assuming the specific heat of the solution is the same as that of water, what is the heat of reaction?
a)
940 J
b)
-940 J
c)
990 J
d)
-990 J
37.

From the following enthalpy changes,

H2 (g) + F2 (g) → 2HF (g) ∆H° = -542.2 kJ

2H2 (g) + O2 (g) → 2H2O (l) ∆H° = -571.6 kJ calculate the value of ∆H° for the reaction: 2F2 (g) + 2H2O (l) → 4HF (g) + O2 (g)

a)

-1113.8 kJ

b)

-1656.0 kJ

c)

-512.8 kJ

d)

29.4 kJ

38.
Which of the following would have a nonzero enthalpy of formation?
a)
Fe(s)
b)
Br2(s)
c)
O2(g)
d)
Hg(l)
39.
Which of the following would have a standard enthalpy of formation value of zero?
a)
H2O(l)
b)
H2O(g)
c)
F2(g)
d)
O3(g)
40.
Given the chemical equation:
C4H9OH+6O2 → 4CO2+5H2O
What is the sign for the heat of reaction and why?
a)
+, since the reaction is single replacement
b)
+, since the reaction is combustion
c)
-, since the reaction is single replacement
d)
-, since the reaction is combustion
41.
Thermodynamically favorable reactions...
a)
are very fast
b)
occur only with the addition of work
c)
occur without the addition of work
d)
are always exothermic
42.

How much energy is required to boil 125 g of C6H6 at its boiling point of 80.1oC. The heat of vaporization of C6H6 is 30.8 kJ/mol.

a)

4.06 kJ

b)

49.3 kJ

c)

165 kJ

d)

3850 kJ

43.

The enthalpy of combustion of methanol (CH3OH) is -711 kJ⋅mol-1. What mass of methanol must be completely burned in oxygen in order to produce 71.1 kJ of energy?

a)

32.0 g

b)

3.20 g

c)

72.0 g

d)

720. g

e)

None of the above

44.

The standard enthalpies of formation for ethene (C2H4), water (H2O) and ethanol (C2H5OH) are +52, -286 and -277 kJ/mol respectively. Calculate ∆Ho for the reaction Ethene + Water → Ethanol

a)

+61 kJ

b)

-43 kJ

c)

-61 kJ

d)

-511 kJ

e)

-615 kJ

45.

which is endothermic?

a)

IMFs broken

b)

negative delta H

c)

products are lower energy than reactants

d)

temperature increases

46.
Some average bond enthalpies, in kJ/mol, are as follows:
H-H = 436
Cl-Cl = 242
H-Cl = 431
What is the enthalpy change for the decomposition of hydrogen chloride?
2 HCl --> H2 + Cl2
a)
-184 kJ
b)
+ 184 kJ
c)
- 247 kJ
d)
+ 247 kJ
47.

The 1st Law of Thermodynamics indicates that

a)

work is force exerted over a distance.

b)

energy in the universe is finite.

c)

an increase in disorder is part of any spontaneous process.

d)

work is a state function.

48.

Breaking bonds is _________________. Forming bonds is ______________________

a)

endothermic, exothermic

b)

exothermic, endothermic

49.

If a reaction is exothermic, then the bonds formed in the products are ___________________ than the reactant bonds.

a)

stronger/more stable

b)

weaker/less stable

50.

According to Hess' Law, if you double the coefficients of a reaction, ΔH will ________________________

a)

Stay the same

b)

Double

c)

Quadruple

d)

Halve

51.

According to Hess' Law, if you reverse a reaction, ΔH will ________________________

a)

Change signs

b)

Double

c)

Be inversed

d)

Halve

52.

Bond enthalpy is the amount of energy is takes to break __________ of a bond.

a)

one mole

b)

one gram

c)

the activation energy

d)

the binding energy

53.

What are the units of ΔHrxn?

a)

kJ

b)

J

c)

kJ/mol

d)

J/mol

54.

Endothermic

a)

absorb energy

b)

release energy

55.

Exothermic

a)

absorb energy

b)

release energy

56.

In the dissolution process, the increase in separation between ions in the solute is

a)

endothermic

b)

exothermic

57.

In a system, the energy lost by the reacting species must be ________________ the energy gained by the surrounding

a)

greater than

b)

less than

c)

equal to

58.

On a potential energy diagram for an endothermic reaction,

a)

the potential energy of the reactants is greater than the potential energy of the products

b)

the potential energy of the reactants is less than the potential energy of the products

c)

the potential energy of the reactants is equal to the potential energy of the products

59.

A thermometer is placed in a calorimeter. A solid is dissolved in water in the calorimeter and the temperature of the thermometer increases. The dissolution reaction must be

a)

endothermic

b)

exothermic

60.

Using bond energies to solve for enthalpy, 

a)

ΔH\Delta H  =  Bond broken - bonds formed

b)

undefined =  Bond formed- bonds broken

c)

undefined =  products - reactants

d)

undefined =  reactants- products

61.

The enthalpy of formation for a lone element is

a)

a number

b)

zero

62.

I feel I am prepared to do well on this exam. (I will have a review day when I return)

a)

Yes, I have completed my work, studied, and have a fairly good grasp of the concepts.

b)

No, I have not done the work. I still need to study and am not understanding the material.

c)

What class is this for?

d)

I am nearly there. I have been working on the the materials and studying and with a little more practice, I think I'll do okay.

63.

What is the reaction rate of:

2 AgI + Na2S → Ag2S + 2 NaI

a)

Rate= -Δ[AgI]/2(Δt)=-Δ[Na2S]/Δt= Δ[Ag2S]/Δt= Δ[NaI]/2(Δt)

b)

Rate= Δ[AgI]/2(Δt)= Δ[Na2S]/Δt= Δ[Ag2S]/Δt= Δ[NaI]/2(Δt)

c)

Rate= Δ[AgI]/2(Δt)=Δ[Na2S]/Δt= -Δ[Ag2S]/Δt= -Δ[NaI]/2(Δt)

d)

None

64.
a)
A. is most exothermic
b)
B. is most exothermic
c)
C. is most exothermic
d)
D. is most exothermic
65.
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 
66.

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

67.
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
68.
In any first order reaction, as the reaction proceeds at constant temperature, which describes the corresponding effects on k (the rate constant) and rate?
a)
k remains the same; rate decreases
b)
k and rate both remain the same
c)
k remains the same; rate increases
d)
k decreases; rate remains the same
69.
A compound has a half-life of 14 min. How much time will it take a 12 mol sample to decay to 1.5 mol?
a)
14 min
b)
28 min
c)
42 min
d)
56 min
70.
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
71.
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

72.
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 
73.
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
74.
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
75.
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.
76.

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

77.

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

78.

If the reaction rate increases by a factor of 4 when the concentration of reactant A is increased by a factor of 2 (assuming any other reactants remain constant), the order of the reaction with respect to reactant A must be

a)

zero order

b)

first order

c)

second order

d)

fourth order

79.

If a graph of concentration versus time is linear, the order of the reaction must be

a)

zero order

b)

first order

c)

second order

80.

If a graph of ln(concentration) versus time is linear, the order of the reaction must be

a)

zero order

b)

first order

c)

second order

81.

If a graph of 1/concentration (reciprocal concentration) versus time is linear, the order of the reaction must be

a)

zero order

b)

first order

c)

second order

82.

Given

Step 1: AB + C2 → ABC + C (slow)

Step 2: C + AB → ABC (fast)

What would be the overall reaction?

a)

2AB + C3 → 2ABC + C

b)

2AB + C2 + C → 2ABC + C

c)

2AB + C2 → 2ABC

83.

Given

Step 1: AB + C2 → ABC + C (slow)

Step 2: C + AB → ABC (fast)

What would be the rate law

a)

Rate = k[AB]2[C2]

b)

Rate = k[AB][C2]

c)

Rate = k[AB]2[C2][ABC]

d)

Rate = k[AB]2[C2][ABC]2

84.
Which one of the following is a first order, overall reaction
a)
k1= 1.000 M s-1
b)
k1= 5403.2 M½ s½
c)
k1= 1.23 x 10-6 M-1 s-1
d)
k1= 10.7 s-1
85.
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
86.

The decomposition of nitrous oxide :


2N2O(g) → 2N2(g) + O2(g)


is believed to occur by two-step mechanism


N2O(g) → N2(g) + O(g) (slow)

N2O(g) + O(g) → N2(g) + O2(g) (fast)


the consistent rate equation based for the mechanism above is ____

a)

rate = k [N2O]2

b)

rate = k [N2O]

c)

rate = k [N2O]2 [N2]

d)

rate = k

87.

What is NOT a way to speed up a reaction

a)

Add a catalyst

b)

Decrease the volume

c)

Increase the concentration of reactants

d)

Increase surface area of the solid

e)

Decrease the pressure

88.

Which curve represents the most particles in this Maxwell-Boltzmann curve (# of particles vs. speed)?

a)

Black (peak on the left)

b)

Red (peak in the middle)

c)

Blue (peak on the right)

d)

They all have the same number of particles

89.

Which curve in this Maxwell-Boltzmann distribution represents the highest proportion of particles moving the fastest (# of particles vs. speed)?

a)

Black (peak on the left)

b)

Red (peak in the middle)

c)

Blue (peak on the right)

d)

All particles are moving at the same speed

90.

Which of the following plots will show a linear relationship for a second order reaction?

a)

[A] vs time

b)

1/[A] vs time

c)

ln[A] vs time

d)

[A]2 vs time

91.
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
92.

A reaction is found to be second order with respect to carbon monoxide. If the concentration of carbon monoxide is doubled, the rate of reaction __________.

a)

doubles

b)

remains unchanged

c)

increases by a factor of 4

d)

is reduced by a factor of 2

93.

Which of the following are true of reaction rates?

I. The overall rate law is determined by the fastest step of a reaction

II. The presence of a catalyst will increase the number of molecules entering the transition state

III. An increase in temperature will increase the rate of a reaction

IV. Decreasing the concentration of reactants will increase the rate at which products yield

a)

II+III+IV

b)

I+IV

c)

II + III

d)

I+II+III

94.

rate = k[A]

The rate constant in the rate law above is 0.5 1/s. If the initial concentration of A is 0.1 M, how long will it take for [A] to drop to 0.025 M?

a)

0.7 s

b)

1.4 s

c)

2.8 s

d)

There is not enough information given.

95.
A reaction has the rate law: Rate = k [A][B].
What is the overall order of reaction?
a)
1st
b)
2nd
c)
3rd
d)
4th
96.
A reaction has the rate law: Rate = k [A][B].
What is the overall order of reaction?
a)
1st
b)
2nd
c)
3rd
d)
4th
97.
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]
98.

Activation energy is the amount of energy required to

a)

break the bonds between the reacting molecules

b)

convert the reactants into the activated complex

c)

make the reacting particles collide

d)

form the bonds between the product molecules

99.
A catalyst facilitates a reaction by
a)
making the reaction more exothermic
b)
lowering the activation energy of the reaction.
c)
decreasing the temperature at which the reaction will proceed spontaneously. 
d)
shifting the position of the equilibrium of the reaction. 
100.
Which species would be a catalyst in the mechanism shown?
a)
Pt
b)
CO
c)
Cl
d)
ClCO

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