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AP Chemistry

Total questions: 60

Worksheet time: 2hrs 43mins

Name
Class
Date
1.
For the reaction...
SO2 + O2 <−>  SO3
If the equilibrium shifts to the right, the concentration of O2 will ___________.
a)
increase
b)
decrease
c)
remain the same
d)
double
2.
For the reaction...
SO2 + O2 <−>  SO3
If the concentration of O2 is decreased, the equilibrium of the reaction will shift ___________.
a)
left
b)
right
c)
left and right
d)
neither left nor right
3.
Which of the following is NOT true at equilibrium?
a)
The forward and reverse reactions proceed at the same rate.
b)
The concentrations of reactants and products do not change.
c)
The concentration of the reactants is equal to the concentration of the products.
d)
The forward and reverse reactions continue to occur.
4.
What is the equilibrium expression for:
Fe3O4(s) + 4H2(g) <--> 3Fe(s) + 4H2O(g)
a)
([Fe]3[H2O]4 ) / ([Fe3O4][H2]4)
b)
([Fe3O4][H2]4)/ ([Fe]3[H2O]4)
c)
[H2O]4 / [H2]4
d)
([Fe][H2O]) / ([Fe3O4][H2])
5.

Consider the following equation: CO(g) + 2H2(g) ⇌ CH3OH(g) + Heat

Which of the factors below would decrease the concentration of CH3OH at equilibrium?

a)

adding CO

b)

incresing H2

c)

decrease in the temperature

d)

increasing the temperature

6.
Predict the effect of decreasing the volume of the container on the following reaction: 
2NH3(g) ⇋ N2(g) + 3H2(g) 
a)
shift left
b)
shift right
c)
no change 
d)
all the above
7.
What is the proper Keq for the following reaction? 
   2 NO(g)  +  O2(g) ⇌2 NO2(g)
a)
Keq = [NO2]2 / [NO]2[O2]
b)
Keq =  [NO]2[O2] / [NO2]2
c)
Keq = [NO]2[O2][NO2]2
d)
Keq = 2[NO][O2] / 2[NO2]
8.
What are [A] and [B]?
a)
concentration of reactants
b)
concentration of products
c)
energy of reactants
d)
energy of products
9.

For reaction a<-- --> b. Use the graph to determine what the Keq will be.

a)

K > 1

b)

K < 1

c)

K = 1

d)

Not enough information

10.

(Calculator Allowed) 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

11.

(Calculator Allowed) The solubility of CuI is 2 x 10-6 molar. What the the solubility product constant, Ksp, for CuI?

a)

8 x 10-18

b)

2 x 10-6

c)

4 x 10-12

d)

2 x 10-12

12.
When Keq > 1, 
a)
There are more products than reactants when the reaction reached equilibrium.
b)
There are more reactant than products when the reaction reached equilibrium.
c)
The amount of reactants is equal to the amount of products.
13.
The reaction quotient for a system is 7.2 × 102. If the equilibrium constant for the system is 36, what will happen as equilibrium is approached?
a)
There will be a net gain in product
b)
There will be a net gain in reactant.
c)
There will be a net gain in both product and reactant
d)
There will be no net gain in either product or reactant.
14.

Which one of the following will change the value of an equilibrium constant?

a)

changing temperature

b)

adding other substances that do not react with any of the species involved in the equilibrium

c)

varying the initial concentrations of reactants

d)

varying the initial concentrations of products

e)

changing the volume of the reaction vessel

15.

(Calculator allowed) The concentration of iodide ions in a saturated solution of silver iodide is ________ M. The solubility product constant of AgI is ksp = 8.3 x 10-17.

a)

3.8 × 10-11

b)

3.0 × 10-10

c)

9.1 × 10-9

d)

3.5 × 10-9

e)

1.4 × 10-8

16.

2 BaO2(s) ⇄ 2 BaO(s) + O2(g)

ΔH°= 162 kJ/molrxn

APMCQ: A sealed rigid vessel contains BaO2(s) in equilibrium with BaO(s) and O2(g) as represented by the equation above. Which of the following changes will increase the amount of BaO2(s) in the vessel?

a)

Removing a small amount of O2(g)

b)

Removing a small amount of BaO(s)

c)

Adding He gas to the vessel

d)

Lowering the temperature

17.

APMCQ: A 0.10 mol sample of each of the four species in the reaction represented above is injected into a rigid, previously evacuated 1.0 L container. Which of the following species will have the highest concentration when the system reaches equilibrium?

a)

H2S(g)

b)

CH4(g)

c)

CS2(g)

d)

H2(g)

18.

2 S(s) + 2 O2(g) ⇄ 2 SO2(g) K1 = 2 x 10105

2 SO2(g) + O2(g) ⇄ 2 SO3(g) K2 = 7 x 1024

APMCQ: Given the value of the equilibrium constants K1 and K2 for the reactions represented above, what is the value of the equilibrium constant, K3, for the following reaction?

2 S(s) + 3 O2(g) ⇄ 2 SO3(g) K3 = ?

a)

1 x 10130

b)

3 x 1080

c)

1 x 1065

d)

2 x 1040

e)

7 x 1024

19.

2 XY(g) ⇄ X2(g) + Y2(g) Kp = 230

A certain gas, XY(g), decomposes as represented by the equation above. A sample of each of the three gases is put in a previously evacuated container. The initial partial pressures of the gases are shown in the table above.


APMCQ: The temperature of the reaction mixture is held constant. In which direction will the reaction proceed?

a)

The reaction will form more products.

b)

The reaction will form more reactant.

c)

The mixture is at equilibrium, so there will be no change.

d)

It cannot be determined unless the volume of the container is known.

20.

2X(g) + Y(g) ⇄ 3Z(g)

APMCQ: The reaction mixture represented above is at equilibrium at 298 K, and the molar concentrations are [X] = 2.0 M, [Y] = 0.5 M, and [Z] = 4.0 M. What is the value of the equilibrium constant for the reaction at 298 K ?

a)

0.5

b)

2

c)

4

d)

16

e)

32

21.

CaCO3(s) ⇄ CaO(s) + CO2(g) ΔH° = 178 kJ/molrxn

APMCQ: The reaction system represented above is at equilibrium. Which of the following will decrease the amount of CaO(s) in the system?

a)

Increasing the volume of the reaction vessel at constant temperature

b)

Lowering the temperature of the system

c)

Removing some CO2(g) at constant temperature

d)

Removing some CaCO3(s) at constant temperature

22.

COCl2(g) ⇄ CO(g) + Cl2(g)

APMCQ: COCl2(g) decomposes according to the equation above. When pure COCl2(g) is injected into a rigid, previously evacuated flask at 690 K, the pressure in the flask is initially 1.0 atm. After the reaction reaches equilibrium at 690 K, the total pressure in the flask is 1.2 atm. What is the value of Kp for the reaction at 690 K?

a)

0.2

b)

0.05

c)

0.8

d)

1.0

23.

CdF2(s)⇄Cd2+(aq)+2F−(aq)

APMCQ: A saturated aqueous solution of CdF2 is prepared. The equilibrium in the solution is represented above. In the solution, [Cd2+]eq=0.0585 M and [F−]eq=0.117 M. Some 0.90M NaF is added to the saturated solution. Which of the following identifies the molar solubility of CdF2 in pure water and explains the effect that the addition of NaF has on this solubility?

a)

The molar solubility of CdF2 in pure water is 0.0585 M, and adding NaF decreases this solubility because the equilibrium shifts to favor the precipitation of some CdF2.

b)

The molar solubility of CdF2 in pure water is 0.0585 M, and adding NaF has no effect on the solubility because only changes in temperature can increase or decrease the molar solubility of an ionic solid.

c)

The molar solubility of CdF2 in pure water is 0.117M, and adding NaF decreases this solubility because the equilibrium shifts to favor the precipitation of some CdF2.

d)

The molar solubility of CdF2 in pure water is 0.176 M, and adding NaF increases this solubility because the Na+ ions displace the Cd2+ ions, causing the equilibrium to shift to favor the products.

24.

APMCQ: For which of the equilibrium systems represented below will the amount of product(s) at equilibrium increase if the volume of the reaction vessel is increased at a constant temperature?

a)

PCl5(g) ⇄ PCl3(g) + Cl2(g)

b)

2 NO(g) + O2(g) ⇄ 2 NO2(g)

c)

N2(g) + O2(g) ⇄ 2 NO(g)

d)

2 CO(g) ⇄ C(s) + CO2(g)

25.

2 BaO2(s) ⇄ 2 BaO(s) + O2(g)


ΔH°= 162 kJ/molrxn



A sealed rigid vessel contains BaO2(s) in equilibrium with BaO(s) and O2(g) as represented by the equation above. Which of the following changes will increase the amount of BaO2(s) in the vessel?

a)

Removing a small amount of O2(g)

b)

Removing a small amount of BaO(s)

c)

Adding He gas to the vessel

d)

Lowering the temperature

26.

2 H2O(l) ⇄ H3O+(aq) + OH-(aq)


The autoionization of water is represented by the equation above. Values of pKw at various temperatures are listed in the table above:


Based on the information above, which of the following statements is true?

a)

The dissociation of water is an exothermic process.

b)

The pH of pure water is 7.00 at any temperature.

c)

As the temperature increases, the pH of pure water increases.

d)

As the temperature increases, the pH of pure water decreases.

27.
Which of the following shows the correct dissolution reaction for BaCl2?
a)
Ba 2+(aq) + Cl2-(aq) -> BaCl2(s)
b)
BaCl2(aq) -> Ba 2+(aq) + 2Cl-(aq)
c)
 BaCl2(s) -> Ba 2+(aq) + 2Cl-(aq)
d)
Ba 2+(aq) + 2Cl-(aq) -> BaCl2(s)
28.
If K < Q, which part of the reaction will speed up?
a)
forward
b)
reverse
c)
none
29.
An unknown salt, M2Z, has a Ksp of 3.3 x 10-9. Calculate the solubility in mol/L of M2Z.
a)
2.9 x 10-5 M
b)
5.7 x 10-5 M
c)
9.4 x 10-5 M
d)
3.7 x 10-5 M
30.
The molar solubility of PbI2 is 1.52 x 10-3 M. Calculate the value of Ksp for PbI2.
a)
3.51 x 10-9
b)
1.40 x 10-8
c)
4.62 x 10-6
d)
1.52 x 10-3
31.
Calculate the [H+] in a solution that has a pH of 2.73.
a)
5.4 x 10-12 M
b)
1.9 x 10-3 M
c)
2.7 M
d)
11.3 M
32.
The pH at the equivalence point of the titration of a strong acid with a strong base is:
a)
3.9
b)
4.5
c)
7.0
d)
8.2
33.
Which of the following is a conjugate acid/base pair?
a)
HCl/OCl-
b)
H2SO4/SO42-
c)
NH4+/NH3
d)
H3O+/OH-
34.
Silver chromate, Ag2CrO4, has a Ksp of 8.96 x 10-12. Calculate the solubility in mol/L of silver chromate.
a)
1.31 x 10-4M
b)
1.65 x 10-4M
c)
2.25 x 10-12M
d)
2.08 x 10-4M
35.
The pH of a solution at 25ₒC in which [OH-] = 3.9 x 10-5M is:
a)
4.41
b)
3.90
c)
9.59
d)
4.80
36.
A weak acid, HF, is in solution with dissolved sodium fluoride, NaF. If HCl is added, which ion will react with the extra hydrogen ions from the HCl to keep the pH from changing?
a)
OH-
b)
Na+
c)
F-
d)
Na-
37.
The correct mathematical expression for finding the molar solubility (s) of Sn(OH)2 is:
a)
2s2 = Ksp
b)
2s3 = Ksp
c)
4s3 = Ksp
d)
8s3 = Ksp
38.
An unknown salt, M2Z, has a Ksp of 3.3 x 10-9. Calculate the solubility in mol/L of M2Z.
a)
2.9 x 10-5 M
b)
5.7 x 10-5 M
c)
9.4 x 10-5 M
d)
3.7 x 10-5 M
39.
When the chemical reaction A + B ↔ C+ D is at equilibrium,
a)
both the forward and reverse reactions have stopped.
b)
the sum of the concentrations of A and B equals the sum of the concentrations of C and D.
c)
all four concentrations are equal.
d)
neither the forward nor the reverse reactions have stopped.
40.
A substance that ionizes completely in solution is
a)
an insulator.
b)
a strong electrolyte. 
c)
a weak acid.
d)
a non-electrolyte.
41.
Equilibrium for 2CrO42- + 2H+→Cr2O72- + H2O. What happen when OH- ions are added to the system?
a)
Position of equilibrium will shift to right
b)
Color of system will turn from orange to yellow
c)
Kc will decrease
d)
OH- ions will not react, and thus no change is seen.
42.

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

43.
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)
44.
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
45.
2SO2(g)+O2(g)⇌2SO3(g)
Using a catalyst
a)
shift equilibrium right
b)
shift equilibrium left
c)
increase rate of reaction
d)
have no change
46.
At what time (in seconds) is equilibrium established?
a)
0 seconds
b)
1 second
c)
5 seconds
d)
10 seconds
47.
For the reaction...
N2  +  O2  <=>  2NO
If  O2 is removed, the  concentration of N2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
double
48.

Consider the following reaction:

2SO2(g) + O2(g) <=> 2SO3(g): ΔΗ = - 197 kJ mol-1

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

a)

Adding more O2

b)

Adding a catalyst

c)

increasing the pressure

d)

Lowering the temperature

49.
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
50.

H2C2O4 + 2 H2O ↔ 2 H3O+ + C2O4 2–


Oxalic acid, H2C2O4, is a diprotic acid with K1 = 5 x 10–2 and K2 = 5 x 10–5. Which of the following is equal to the equilibrium constant for the reaction represented above?

a)

5 x 10–2

b)

5 x 10–5

c)

2.5 x 10–6

d)

5 x 10–7

51.
Which of the following is an example of an acid anhydride.
a)
MgO
b)
Na2O
c)
CO2
d)
CaO
52.
WHen 200 mL of 2.0 M NaOH(aq) is added to 500 mL of 1.0 M HCl(aq), the pH of the resulting mixture is closest to 
a)
1.0
b)
3.0
c)
7.0
d)
13.0
53.

Of the following, which is the strongest acid

a)

HClO

b)

HClO2

c)

HClO3

d)

HClO4

54.

What is the conjugate acid of CO3-2?

a)

CO2-2

b)

HCO22-2

c)

H2CO3

d)

HCO3-1

55.
A compound that donates H+ ions is 
a)
A Bronsted-Lowry Acid
b)
An Arrhenius Acid
c)
A Bronsted-Lowry Base
d)
An Arrhenius Base
56.

Water can act as both an acid and a base in an ionization reaction to form H+ and OH– ions. What is this phenomenon called?

a)

neutralization

b)

self-ionization

c)

base dissociation

d)

acid dissociation

57.

Hydrochloric acid (HCl) and acetic acid (HC2H3O2) are both acids. HCl completely dissociates in water, while HC2H3O2 does not. Which of the following statements best describes these two acids?

a)

HCl is a weak acid, HC2H3O2 is a weak acid.

b)

HCl is a strong acid, HC2H3O2 is a strong acid.

c)

HCl is a strong acid, HC2H3O2 is a weak acid.

d)

HCl is a weak acid, HC2H3O2 is a strong acid.

58.

Which of the following is a Brønsted-Lowry base but not an Arrhenius base?

a)

Ca(OH)2

b)

NH3

c)

NaOH

d)

KOH

59.
The Kw constant is:
a)
1.0 x 10-14
b)
1.0 x 1014
c)
6.022 x 1023
d)
6.0634 x 10-34
60.
If 25 mL of a Ca(OH)2 solution is needed to neutralize 15 mL of 0.18 M HC2H3O2, what is the concentration of the Ca(OH)2 solution?
a)
0.216 M
b)
0.108 M
c)
0.3 M
d)
0.054 M

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