Chemical Equilibrium
Practice Test
1.
For the reaction, 2SO
2
g
+O
2
g
→ 2SO
3
g
at equilibrium, the removal of O
2
would cause _______________.
SC.A.1.4.4
a.
the concentration of SO
2
to increase, and the concentration of SO
3
to increase
b.
the concentration of SO
2
to increase, and the concentration of SO
3
to decrease
c.
the concentration of SO
2
to decrease, and the concentration of SO
3
to decrease
d.
the concentration of SO
2
to decrease, and the concentration of SO
3
to increase
2.
Which of the following states that an equilibrium system that is disturbed will respond in a manner to restore equilibrium?
SC.A.1.4.4
a.
Le Châtelier’s principle
b.
Boyle’s law
c.
Charles’s law
d.
Dalton’s law
3.
The molar solubility for BaCO
3
is 9.0 x 10
-5
M
at 25°C. What is the solubility product constant,
K
sp
, for BaCO
3
?
SC.A.1.4.5
a.
4.0 x 10
-15
b.
8.1 x 10
-9
c.
1.2 x 10
-8
d.
5.3 x 10
-12
4.
Which of the following would force the forward reaction to completion?
CaCO
3
s
+2H
3
O
+
aq
→ Ca
2+
aq
+3H
2
O
l
+CO
2
g
SC.A.1.4.4
a.
add more Ca
2+
to the mixture
b.
add CO
2
to the mixture
c.
add base to neutralize the H
3
O
+
d.
conduct the experiment in an open container
5.
For the reaction, 2A+B→ C+2Dat 35°C, the value of the forward rate constant,
K
f, is 3.0 × 10
-3
M
-1
s
-1
and the value of the reverse rate constant,
K
r, is 1.5 × 10
-2
M
-2
s
-1
. Calculate the value of
K
eq
for this reaction.
SC.A.1.4.4
a.
2
b.
0.5
c.
0.2
d.
5
6.
When Δ G is zero, ______________.
SC.B.1.4.7
a.
the reaction is not spontaneous
b.
the reaction has no energy
c.
the reaction is at equilibrium
d.
the reaction is spontaneous
7.
Which of the solubility product expressions is incorrect?
SC.A.1.4.4
a.
K
sp
Ag
2
S
=
Ag
+
2
S
2-
b.
K
sp
CuS
=
Cu
2+
S
2-
c.
K
sp
CaF
2
=
Ca
2+
F
-
2
d.
K
sp
Sb
2
S
3
=
Sb
2+
3
S
3-
2
8.
For the gas phase reaction, SO
2
g
+ ½O
2
g
→ SO
3
g
, ΔH° = -1.6 × 102 kJ for the forward reaction. To increase the yield of SO
3
, the reaction should be run at ________.
SC.A.1.4.4
a.
high pressure and high temperature
b.
low pressure and high temperature
c.
high pressure and low temperature
d.
low pressure and low temperature
9.
What is the equilibrium constant expression for the following reaction?
2NH
4
NO
3
s
→ 2NH
3
g
+2NO
g
+H
2
g
+ 2O
2
g
SC.A.1.4.4
a.
K
eq
=
NH
3
NO
H
2
O2
/
NH
4
NO
3
b.
K
eq
=
NH
3
2
NO
2
H
2
O2
2
c.
K
eq
=
NH
3
2
NO
2
H
2
O2
2
/
NH
4
NO
3
2
d.
K
eq
=
NH
3
NO
H
2
O2
10.
The value of the
K
sp
for SrSO
4
is 2.8 x 10
-7
. What is the molar solubility of SrSO
4
?
SC.A.1.4.5
a.
7.6 x 10
-7
M
b.
5.3 x 10
-4
M
c.
5.7 x 10
-3
M
d.
5.8 x 10
-13
M
11.
What is the equilibrium constant expression for the following reaction?
2SO
3
‹–› 2SO
2
+ O
2
SC.A.1.4.4
a.
K
eq
=
2SO
2
2O
/
2SO
3
b.
K
eq
=
SO
2
2
O
2
/
SO
3
2
c.
K
eq
=
SO
3
2
/
SO
2
2
O
2
d.
K
eq
= 2
SO
2
2
O
2
/2
SO
3
12.
For the reaction, 2Cl
2
g
+2H
2
O
g
+ heat→4HCl
g
+O
2
g
, which of the following will shift the equilibrium to produce more HCl?
SC.A.1.4.4
a.
lower the temperature of the reaction
b.
decrease the volume of the reaction vessel
c.
add more Cl
2
d.
add more O
2
13.
What is the equilibrium constant expression for the following reaction?
H
2
+ I
2
‹–› 2HI
SC.A.1.4.4
a.
K
eq
=
H
2
I
2
/
HI
2
b.
K
eq
=
2HI
/ /
H
2
I
2
c.
K
eq
=
HI
2
/
H
2
I
2
d.
K
eq
=
HI
2
/
H
2
I
2
14.
How many grams of MgF
2
will dissolve in 150 mL of 0.100
M
NaF solution? Ksp for MgF
2
is 6.4 x 10
-9
.
SC.A.1.4.4
a.
1.0 x 10
-5
g
b.
4.1 x 10
-6
g
c.
6.0 x 10
-6
g
d.
6.4 x 10
-7
g
15.
If NaCl is added to a 0.010M solution of AgNO
3
in water at 25°C, what will be
Cl
-
when precipitation of AgCl begins? The Ksp for AgCl is 1.8 x 10
-10
.
SC.A.1.4.5
a.
1.8 x 10
-8
M
b.
1.0 x 10
-10
M
c.
1.3 x 10
-6
M
d.
1.8 x 10
-12
M
