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AP Chemistry Exam Review

Total questions: 61

Worksheet time: 1hrs 6mins

Name
Class
Date
1.

Which of the following will conduct electricity? Select all that apply

a)

Acidic solutions

b)

Basic solutions

c)

Ionic solutions

d)

Neutral covalent solutions

2.

Neutralization is the process of an acid and a base reacting to form what? Select all that apply

a)

An ionic salt

b)

Hydronium ions

c)

NaCl

d)

Water

3.

Which of the following are strong acids? Select all that apply

a)

HI

b)

H2SO4

c)

HF

d)

HCl

e)

HClO3

4.

Which of the following is NOT a strong base?

a)

NaOH

b)

RbOH

c)

Al(OH)3

d)

Ca(OH)2

5.

A bronsted lowry acid

a)

produces hydroxide ions in a solution

b)

is a proton donor

c)

produces hydrogen ions in a solution

d)

is a proton acceptor

6.

A bronsted lowry base

a)

produces hydroxide ions in a solution

b)

is a proton donor

c)

produces hydrogen ions in a solution

d)

is a proton acceptor

7.

Water can act as both an acid and a base according to the bronsted lowry model. This means water is

a)

neutral

b)

conjugate

c)

ionic

d)

amphoteric

8.

Identify the true statement about the following reaction:

F- + H2O --> HF +OH-

a)

H2O is a bronsted lowry base

b)

H2O is not an acid or base according to either model

c)

H2O is a bronsted lowry acid

d)

H2O is an arrhenius acid

9.
HCl + NaOH → 
a)
NaH + ClOH
b)
NaCl + H2
c)
NaCl + H2O
d)
NaCl + Cl2
10.
I am titrating 1M HCl with 1M NaOH.  I have 25mL of HCl. How much NaOH will I need?
a)
2.5mL
b)
5mL
c)
25mL
d)
50mL
11.
what is the reading on this burette?
a)
4.40mL
b)
3.50mL
c)
3.60mL
d)
4.50mL
12.
I have 25mL of 1M HCl which neutralises 20mL of NaOH. What is the concentration of the NaOH?
a)
0.8 M
b)
1 M
c)
1.25 M
13.
Identify the products of the chemical equation
3 LiOH + H3PO4 →
a)
Li3PO4 + 3 H2O
b)
LiPO4 + 3 H2O
c)
Li(PO4)3 + 3 H2O
d)
BOY + La + N2
14.
A 50.0 mL sample of Ca(OH)2 is neutralized by 300.0 mL of HCl solution with a pH of 1.3. Calculate the molarity of the Ca(OH)2 solution.
a)
1.0 M
b)
0.50 M
c)
0.15 M 
d)
0.30 M
15.
How many moles of Ca(OH)2 are needed to neutralize three moles of HCl? 
a)
8
b)
1.5
c)
6
d)
3
16.
For the acid-base titration combination of NaOH with 0.79 mol HCl, find the number of moles of NaOH that would be the chemically equivalent amount of HCl.
a)
0.79 mol
b)
1.6 mol
c)
0.38 mol
d)
3.2 mol
17.
Which of the following is a conjugate acid/base pair?
a)
HCl/OCl-
b)
H2SO4/SO42-
c)
NH4+/NH3
d)
H3O+/OH-
18.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
19.

Which of the following has hydrogen bonding?

a)

HBr

b)

NO2

c)

H2S

d)

NH3

20.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

21.

Intermolecular forces for: CO2

a)

London Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

22.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
23.
What is the basis of a metallic bond?
a)
the attraction of neutral metal atoms.
b)
the attraction between protons and neutrons.
c)
the attraction between positive metal ions and interlocking electrons.
d)
the attraction between positive metal ions and free floating electrons.
24.

This picture most likely depicts the arrangement of atoms in a

a)

diamond

b)

salt

c)

metal

d)

gas

25.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
26.
a)
A. is most exothermic
b)
B. is most exothermic
c)
C. is most exothermic
d)
D. is most exothermic
27.
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 
28.
a)
A. has largest Ea
b)
B. has largest Ea
c)
C. has largest Ea
d)
E. has largest Ea
29.
a)
A. is the slowest reaction
b)
B. is the slowest reaction
c)
C. is the slowest reaction
d)
E. is the slowest reaction
30.
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
31.
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
32.
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

33.
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
34.
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 
35.

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

36.

What order is this?

a)

Zero order

b)

1st order

c)

2nd order

37.

bonds broken

a)

exothermic

b)

endothermic

38.

temperature increases

a)

exothermic

b)

endothermic

39.

products have lower potential energy than reactants

a)

exothermic

b)

endothermic

40.

bonds form

a)

exothermic

b)

endothermic

41.

What is the driving force of a reaction that has a + H and a + S?

a)

temperature

b)

enthalpy

c)

entropy

d)

this reaction is never spontaneous

42.

NH4NO3(s) → N2O(g) + 2 H2O(g)


A 0.03 mol sample of NH4NO3(s) is placed in a 1 L evacuated flask, which is then sealed and heated. The NH4NO3(s) decomposes completely according to the balanced equation above. The total pressure in the flask measured at 400 K is closest to which of the following? ( The value of the gas constant, R, is 0.082 L atm mol–1 K–1)

a)

3 atm

b)

1 atm

c)

0.5 atm

d)

0.1 atm

43.
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
44.

The enthalpies of combustion of C(s), H2(g) and C4H9OH(l) (in kJmol-1) are as follows

C(s) + O2(g) -> CO2(g) ∆H=a

H2(g) + ½O2(g) -> H2O(l) ∆H=b

C4H9OH(l) + 6O2(g) -> 4CO2(g) + 5H2O(l) ∆H=c

What is the enthalpy change for the reaction shown below?

4C(g) + 5H2(l) + ½O2(g) -> C4H9OH(l)

a)

c – 4a – 5b

b)

2a + 10b - c

c)

4a + 5b - c

d)

2a + 5b + c

45.

All alkaline earth metals have the following number of valence electrons:

a)

1

b)

3

c)

6

d)

2

e)

none of these

46.

Order the elements S, Cl, and F in terms of increasing atomic radii.

a)

S, Cl, F

b)

Cl, F, S

c)

F, S, Cl

d)

F, Cl, S

e)

S, F, Cl

47.

Of the following elements, which is most likely to form a negative ion with a charge of 1-?

a)

Ba

b)

Ca

c)

Si

d)

P

e)

Cl

48.

Given the Kc for a forward reaction, how can you find Kc for the reverse reaction?

a)

Divide Kc by 1

b)

Divide 1 by Kc

c)

Square Kc

d)

Take the square root of Kc

49.

This endothermic reaction is at equilibrium.

If its temperature is increased (at constant volume and pressure), which way will the equilibrium shift?

a)

To products (right)

b)

To reactants (left)

50.
Le Chatelier's Principle states that if a chemical system at equilibrium is stressed,
a)
the system will adjust to increase the stress
b)
the system will adjust to reduce the stress
c)
the system will not adjust
51.
When the rate of the forward reaction is equal to the rate of backward reaction, the system is said to be in
a)
Chemical Equilibrium
b)
Chemical Balance
c)
Stoichiometry
d)
Chemical Reaction
52.

For the reaction...

SO2 + O2 <−> SO3

If the concentration of SO2 is increased, the system will shift ___________.

a)

left

b)

right

c)

left and right

d)

neither left nor right

53.

For the reaction...

heat + N2 + O2 ↔ 2NO

If heat is added to the chemical system, the system will shift _______.

a)

left

b)

right

c)

left and right

d)

neither left nor right

54.

2SO2 (g) + O2 (g) ⇌ 2SO3 (g)

Decreasing the volume of container will

a)

shift the system right

b)

shift the system left

c)

change K

d)

have no effect

55.

At what time (in seconds) is equilibrium established?

a)

0 seconds

b)

1 second

c)

5 seconds

d)

10 seconds

56.

2SO2 (g) + O2 (g) ⇌ 2SO3 (g)

Using a catalyst will...

a)

shift the system right

b)

shift the system left

c)

increase the rate of reaction

d)

have no effect

57.
What is the Kc expression for this reaction?
   2 NO(g)  +  O2(g) ⇌  2 NO2(g)
a)
Kc = [NO2]2 / [NO]2 [O2]
b)
Kc =  [NO]2 [O2] / [NO2]2
c)
Kc = [NO]2 [O2] [NO2]2
d)
Kc = [NO2]2 / [NO]2 +  [O2]
58.

Consider the following reaction:

2SO2(g) + O2(g) <=> 2SO3(g) ΔΗ = - 197 kJ

Which of the following will NOT shift the equilibrium position to the right?

a)

Adding more O2

b)

Adding a catalyst

c)

Decreasing the volume

d)

Lowering the temperature

59.
What is [H2O] if K = 1.2,
[CO2] = 0.846M, & [CH4]= 0.0713M?
4CuO(s)+CH4(g)↔CO2(g)+4Cu(s) +2H2O(g)
a)
0.101 M
b)
0.318 M
c)
0.0102 M
d)
3.77 M
60.

What is the correct equilibrium expression for the following reaction:

2H2O2 (aq) ↔ 2H2O (l) + O2 (g)

a)

[H2O]2[O2] / [H2O2]2

b)

[H2O2]2 / [H2O]2[O2]

c)

[O2] / [H2O2]2

d)

[H2O]2 / [H2O2]2

61.

0.40 M SO2 and 0.60 M O2 are in a flask when the following reaction occurs:

2SO2 (g) + O2 (g) ↔ 2SO3 (g)

At equilibrium, the flask is found to contain 0.30 M SO3. Based on these results, the equilibrium constant, Kc, for the reaction is...

a)

20

b)

10

c)

6.7

d)

2.0

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