[Skip Breadcrumb Navigation]
:
[Skip Breadcrumb Navigation]
Home
Chapter 13: Chemical Equilibrium
Problem Solving Center
Self Quiz 2
Self Quiz 2
This activity contains 20 questions.
An action that will
not
cause a decrease in the concentration of CO in the reaction CH
4
(
g
) + CO(
g
) + 18.8 kJ
CH
3
CHO(
g
) is
increasing the pressure by decreasing the volume.
adding CH
4
.
increasing the temperature.
removing CH
3
CHO.
using a catalyst.
An action that will cause an increase in the concentration of NO in the reaction 2NO(
g
) + Br
2
(
g
)
2NOBr(
g
) + 16.8 kJ is
increasing the pressure by decreasing the volume.
using a catalyst.
adding helium.
decreasing the temperature.
adding NOBr.
Cu(C
2
O
4
)
2
2-
(
aq
) + 4NH
3
(
aq
)
Cu(NH
3
)
4
2+
(
aq
) + 2C
2
O
4
2-
(
aq
). In this example Cu(C
2
O
4
)
2
2-
is light blue and Cu(NH
3
)
4
2+
is dark blue. Which concentration stress correctly matches the color change?
adding H
3
O
+
, which reacts with NH
3
to form NH
4
+
: becomes light blue
removing C
2
O
4
2-
: becomes light blue
adding Na
2
C
2
O
4
: becomes dark blue
adding NH
3
: becomes light blue
removing NH
3
: becomes dark blue
If k
r
= 6.2 x 10
3
(M·s)
-1
and K
c
= 9.5 x 10
4
for the general equilibrium reaction X(
g
)
Y(
g
), then the value of the rate constant for the forward reaction is
1.0 x 10
5
(M·s)
-1
.
6.5 x 10
-2
(M·s)
-1
.
8.9 x 10
4
(M·s)
-1
.
5.9 x 10
8
(M·s)
-1
.
15 M·s.
If the temperature is increased for the equilibrium reaction N
2
(
g
) + O
2
(
g
) + 180.4 kJ
2NO(
g
), which statement is
incorrect
?
The K
p
value increases.
The reaction shifts to the left.
The concentration of N
2
decreases.
The concentration of O
2
decreases.
The concentration of NO increases.
The procedure that will cause more solid to form in the equilibrium reaction AgCl(
s
) + 2NH
3
(
aq
)
Ag(NH
3
)
2
+
(
aq
) + 2Cl
-
(
aq
) is
removing Cl
-
.
adding NaCN, which reacts with Ag(NH
3
)
2
+
to form Ag(CN)
2
-
.
adding NaCl.
adding NH
3
.
adding NaNO
3
.
The reaction that will remain unchanged when the pressure is increased by decreasing the volume is
SO
2
(
g
) + Cl
2
(
g
)
SO
2
Cl
2
(
g
).
Br
2
(
g
)
2Br(
g
).
U(
s
) + 3F
2
(
g
)
UF
6
(
g
).
2HgO(
s
)
2Hg(
g
) + O
2
(
g
).
Cu
2
S(
s
) + O
2
(
g
)
2Cu(
s
) + SO
2
(
g
).
What is [CO] in the equilibrium reaction H
2
(
g
) + CO
2
(
g
)
H
2
O(
g
) + CO(
g
) if only H
2
(
g
) and CO
2
are initially present in 1.00 M concentrations? (The K
c
for the reaction is 0.62.)
[CO] = 3.8 M
[CO] = 0.28 M
[CO] = 0.79 M
[CO] = 0.38 M
[CO] = 0.44 M
What is the value of K
c
for the reaction 2A(
g
)
B(
g
) + 2C(
g
) if only A is present initially and [A] at equilibrium is 33.0% of the original concentration of A, which was 2.00 M?
11.0
1.4
0.36
0.165
2.8
What is the value of K
c
for the reaction 2SO
2
(
g
) + O
2
(
g
)
2SO
3
(
g
) if K
p
= 0.037 at 727 °C?
3.0
6.2 x 10
-4
2.2
37
4.5 x 10
-4
What is the value of K
p
for the reaction I
2
(
g
) + Cl
2
(
g
)
2ICl(
g
) at 464 °C if P
I
2
= 0.23 atm, P
Cl
2
= 0.19 atm, and P
ICl
= 5.3 atm?
6.4 x 10
2
2.4 x 10
2
4.1 x 10
-3
1.2 x 10
2
1.6 x 10
-2
Which action will alter the composition of an equilibrium mixture of CaCO
3
, CaO, and CO
2
? (The equilibrium reaction is CaCO
3
(
s
)
CaO(
s
) + CO
2
(
g
).)
removing some CaO
adding CaCO
3
adding argon
increasing the volume
adding CaCO
3
and CaO
Which concentration stress correctly matches the relationship between Q
c
and K
c
for the equilibrium reaction 2H
2
O
2
(
g
)
2H
2
O(
g
) + O
2
(
g
)?
removing H
2
O : Q
c
> K
c
removing H
2
O
2
: Q
c
< K
c
adding O
2
: Q
c
< K
c
adding H
2
O
2
: Q
c
> K
c
removing O
2
: Q
c
< K
c
Which equation is matched with the correct equilibrium expression for that equation?
H
2
(
g
) + Br
2
(
g
)
2HBr(
g
), K
c
= [H
2
][Br
2
]/2 x [HBr]
2CO(
g
) + O
2
(
g
)
2CO
2
(
g
), K
c
= [CO
2
]/[CO][O
2
2CO
2
(
g
)
2CO(
g
) + O
2
(
g
) K
c
= [CO
2
]
2
/[CO]
2
[O
2
]
O
3
(
g
) + O(
g
)
2O
2
(
g
), K
c
= 2 x [O
2
]/[O
3
][O]
N
2
(
g
) + O
2
(
g
)
2NO(
g
), K
c
= [NO]
2
/[N
2
][O
2
]
Which equilibrium expression is correct for the reaction 3Zn(
s
) + 2Al
3+
(
aq
)
3Zn
2+
(
aq
) + 2Al(
s
)?
K
c
= [Zn
2+
]
3
/ [Al
3+
]
2
K
c
= [Zn
2+
]
3
[Al]
2
/ [Zn]
3
[Al
3+
]
2
K
c
= [Zn
2+
] / [Al
3+
]
K
c
= [Al
3+
]
2
/ [Zn
2+
]
3
K
c
= [3 x Zn
2+
]
3
/ [2 x Al
3+
]
2
Which relationship in the equilibrium reaction A
B is
not
possible?
[A] = [B]
[A] > [B]
[A] + [B] = 1
[A] < [B]
[A] + [B] = 0
Which set of conditions shows that the reaction A
B is at equilibrium? (Assume that the forward and reverse reactions are first-order reactions.)
k
forward reaction
= 0.48 s
-1
, [A] = 1.8 M , k
reverse reaction
= 9.5 x 10
-4
s
-1
, [B] = 9.0 M
k
forward reaction
= 1.1 x 10
-1
s
-1
, [A] = 0.90 M , k
reverse reaction
= 3.2 x 10
-1
s
-1
, [B] = 3.0 M
k
forward reaction
= 2.4 x 10
-1
s
-1
, [A] = 0.20 M , k
reverse reaction
= 4.8 x 10
-1
s
-1
, [B] = 0.10 M
k
forward reaction
= 4.2 x 10
-2
s
-1
, [A] = 0.25 M , k
reverse reaction
= 1.4 x 10
-2
s
-1
, [B] = 0.25 M
k
forward reaction
= 2.4 x 10
-1
s
-1
, [A] = 0.20 M , k
reverse reaction
= 2.4 x 10
-1
s
-1
, [B] = 0.80 M
Which statement is correct concerning the equilibrium reaction
2N
2
(
g
) + 5O
2
(
g
) + 22 kJ
2N
2
O
5
As the temperature decreases, the reaction shifts from left to right.
As the temperature increases, the reaction shifts from left to right.
As the temperature decreases, K
c
increases.
As the temperature increases, K
c
decreases.
As the temperature increases, the reaction shifts from right to left.
Which statement is true for an equilibrium system having a K
c
= 10.0?
The equilibrium ratio of products to reactants is equal to 0.100, the inverse of 10.0.
The amount of reactants present will be very large relative to the amount of products present.
The reaction proceeds hardly at all.
The amount of reactants present will be very small relative to the amount of products present.
The reactant and product concentrations will be appreciable.
Which statement is true if K
c
= 14 for the equilibrium reaction I
2
(
g
) + Br
2
(
g
)
2IBr(
g
)?
k
f
= k
r
Rate
forward
is greater than rate
reverse
for the reaction at equilibrium.
k
f
> k
r
k
f
< k
r
If only IBr is present initially, then rate
forward
is greater than rate
reverse
.
The Submit Answers for Grading feature requires scripting to function. Your browser either does not support scripting or you have turned scripting off.
So, the Submit Answers for Grading button below will not work.
The following Submit Answers for Grading button is provided in its place and will clear your answers:
The Clear Answers and Start Over feature requires scripting to function. Your browser either does not support scripting or you have turned scripting off.
So, the Clear Answers and Start Over button below will not work.
The following Clear Answers button is provided in its place and will clear your answers:
Your browser either does not support scripting or you have turned scripting off. Because of this, the answer choices will NOT appear in a different order each time the page is loaded, though that is mentioned below. Note that you do not need this feature to use this site.
Answer choices in this exercise appear in a different order each time the page
is loaded.
Copyright © 1995 - 2010
Pearson Education
. All rights reserved. Pearson Prentice Hall is an imprint of
Pearson
.
Legal Notice
|
Privacy Policy
|
Permissions
[Return to the Top of this Page]
: [Return to the Top of this Page]
B is at equilibrium? (Assume that the forward and reverse reactions are first-order reactions.)
