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AP Chemistry Equilibrium

Total questions: 32

Worksheet time: 3585secs

Name
Class
Date
1.

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

2.
For the reaction...
SO2 + O2  <−>  SO3
If the concentration of SO2 is increased, the equilibrium of the reaction will shift ___________.
a)
left
b)
right
c)
left and right 
d)
neither left nor right
3.

For the reaction...

heat + N2 + O2 ↔ 2NO

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

a)

left

b)

right

c)

left and right

d)

neither left nor right

4.

2SO2(g)+O2(g)⇌2SO3(g)

Decreasing the volume of container will

a)

shift equilibrium right

b)

shift equilibrium left

c)

change K

d)

have no change

5.
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
6.

The following reaction :

SO2 (g) + NO2 (g) <=> SO3 (g) + NO (g)

had reached a state of equilibrium, was found to contain

0.40 mol L-1 SO3 , and 0.30 mol L-1 NO,

0.15 mol L-1NO2 , and 0.20 mol L-1 SO2.

Calculate the equilibrium constant for this reaction.

a)

4.0

b)

0.42

c)

0.25

d)

1.0

7.
What are the two factors to look for when determining if the reaction is at equilibrium?
a)
Forward reaction rate is faster than the reverse and concentrations are equal
b)
Forward and reverse reaction rates are equal and concentration is conctant
c)
Forward and revers reaction rates are equal and concentration is equal
d)
Forward reaction rate is faster than the reverse and concentration is equal
8.
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
9.
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
10.

When 0.40 mole of SO2 and 0.60 mole of O2 are placed in an evacuated 1.00–liter flask, the reaction represented below occurs.

2SO2 (g) + O2 (g) ↔ 2SO3 (g)

After the reactants and the product reach equilibrium and the initial temperature is restored, the flask is found to contain 0.30 mole of SO3. Based on these results, the equilibrium constant, Kc, for the reaction is

a)

20

b)

10

c)

6.7

d)

2.0

11.

In which of the following systems would the number of moles of the substances present at equilibrium NOT be shifted by a change in the volume of the system at constant temperature?

a)

CO(g) + NO(g) ↔ CO2(g) + ½N2(g)

b)

N2(g) + 3H2(g) ↔ 2NH3(g)

c)

N2(g) + 2O2(g) ↔ 2 NO2(g)

d)

NO(g) + O3(g) ↔ NO2(g) + O2(g)

12.

H2(g) +I2(g) ↔ 2HI(g)

All gases begin with an initial concentration of 2.0 M. Equilibrium is established, and the concentration of HI is known to be 4.8 M. What is the value of the equilibrium constant?

a)

1.2

b)

2.4

c)

32

d)

64

13.
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)
14.
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
15.
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
16.
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
17.
Which of the following is a conjugate acid/base pair?
a)
HCl/OCl-
b)
H2SO4/SO42-
c)
NH4+/NH3
d)
H3O+/OH-
18.
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
19.
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
20.
The solubility of CaSO4 in pure water at 0ₒC is 1.14 g/L. The value of the solubility product is
a)
8.37 x 10-3
b)
1.14 x 10-3
c)
9.15 x 10-2
d)
7.01 x 10-5
21.
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-
22.
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
23.
A substance that ionizes completely in solution is
a)
an insulator.
b)
a strong electrolyte. 
c)
a weak acid.
d)
a non-electrolyte.
24.
When citric acid is produced by the cells of an orange and dissolves in water, it produces a relatively small number of hydronium ions. Citric acid is best described as a
a)
concentrated acid. 
b)
weak acid. 
c)
dilute acid.
d)
strong acid.
25.
Which is the weakest acid?
a)
HF
b)
HNO2
c)
CH3COOH
d)
HClO
26.
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.
27.
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])
28.

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

29.

(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

30.
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.
31.
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.
32.

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

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