Chapter 13 - Chemical Equilibrium
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Chapter 13 - Chemical Equilibrium: General Chemistry: 2022FA-CHEM-001B-202
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Chapter 13 - Chemical Equilibrium Due
Sep 25 at 11:59pm
Points
20
Questions
20
Available
Aug 29 at 12am - Dec 4 at 11:59pm
Time Limit
None
Allowed Attempts
2
Instructions
Attempt History
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20 out of 20
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1 / 1 pts
Question 1
A 35.00-L vessel at 700 K initially contains HI(
g
) at a pressure of 5.80 atm; at
equilibrium, it is found that the partial pressure of H
(
g
) is 0.56 atm. What is the
partial pressure of HI(
g
) at equilibrium?
2HI(
g
) H (
g
) + I
(
g
)
2
2
2
5.8 atm
6.36 atm
5.23 atm
0.561 atm
4.67 atm
1 / 1 pts
Question 2
The Ostwald process converts ammonia (NH
) to nitric oxide (NO) by reaction
with oxygen in the presence of a catalyst at high temperatures. In a test of the
process a reaction vessel is initially charged with 4.80 mol NH
(
g
) and 5.80 mol
O (
g
), sealed, and heated at a fixed high temperature. When equilibrium is
established the reaction mixture is analyzed and found to contain 3.80 mol
NO(
g
). What is the quantity of NH
(
g
) in the equilibrium reaction mixture?
4NH (
g
) + 5O
(g) 4NO(
g
) + 6H
O(
g
)
3
3
2
3
3
2
2
4.8 mol NH
(
g
)
3
1.05 mol NH
(
g
)
3
9/20/22, 2:20 AM
Chapter 13 - Chemical Equilibrium: General Chemistry: 2022FA-CHEM-001B-202
https://sjeccd.instructure.com/courses/32359/quizzes/198720
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1 mol NH
(
g
)
3
2 mol NH
(
g
)
3
8.6 mol NH
(
g
)
3
1 / 1 pts
Question 3
Nitrogen trifluoride decomposes to form nitrogen and fluorine gases according to
the following equation:
2NF (
g
) N (
g
) + 3F
(
g
)
When 2.54 mol of NF
is placed in a 6.00-L container and allowed to come to
equilibrium at 800 K, the mixture is found to contain 0.0434 mol of N
. What is
the value of K
at this temperature? (R = 0.0821 L ·
atm ·
mol ·
K )
3
2
2
3
2
p
-1
-1
4.43 ×
10
–7
1.54 ×
10
–5
1.91 ×
10
–3
1.59 ×
10
–5
1.78 ×
10
–3
1 / 1 pts
Question 4
For the reaction 2NO(
g
) + O
2NO (
g
) at 750°C, what is the relationship
between K
and K
?
2 2
c
p
K
= K
c
p
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Chapter 13 - Chemical Equilibrium: General Chemistry: 2022FA-CHEM-001B-202
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K
= K
= 1.0
c
p
K
= K
×
(
RT
)
c
p
–1
K
= K
×
(
RT
)
c
p
3/4
K
= K
×
(
RT
)
c
p
1
1 / 1 pts
Question 5
Carbon tetrachloride may react with oxygen to produce chlorine and carbonyl
chloride.
2CCl (
g
) + O
(
g
) 2COCl (
g
) + 2Cl
(
g
); K
= 9.9 ×
10
What is K
for the following equilibrium?
COCl (
g
) + Cl
(
g
) CCl (
g
) + 1/2O
(
g
)
4
2
2
2
c
51 c
2
2
4
2
5.0 ×
10
–53
9.9 ×
10
–51
–9.9 ×
10
51
1.0 ×
10
–52
1.0 ×
10
–26
1 / 1 pts
Question 6
Given the equilibrium constants for the following reactions:
4Cu(
s
) + O
(
g
) 2Cu O(
s
); K
2
2
1
9/20/22, 2:20 AM
Chapter 13 - Chemical Equilibrium: General Chemistry: 2022FA-CHEM-001B-202
https://sjeccd.instructure.com/courses/32359/quizzes/198720
5/13
2CuO(
s
) Cu O(
s
) + ½ O
(
g
); K
What is K
for the system
2Cu(
s
) + O
(
g
) 2CuO(
s
)
equivalent to?
2
2
2 2
(
K
)(
K
)
1
2
1/2
(
K
) /(
K
)
2
½
1
K
×
K
1
2
(
K
) /(
K
)
2
2
1
(
K
)
/(
K
)
1
1/2
2
1 / 1 pts
Question 7
Consider the following reaction:
2HF(g) H
(g) + F
(g)(
K
= 1.00 ×
10
)
Given that 1.00 mol of HF(
g
), 0.200 mol of H
(
g
), and 0.750 mol of F
(
g
) are
mixed in a 5.00-L flask, determine the reaction quotient, Q
.
2
2
c
–2
2
2
Q
= 0.150
none of these
Q
= 0.0300
Q
= 1.95
Q
= 0.0375
9/20/22, 2:20 AM
Chapter 13 - Chemical Equilibrium: General Chemistry: 2022FA-CHEM-001B-202
https://sjeccd.instructure.com/courses/32359/quizzes/198720
6/13
1 / 1 pts
Question 8
For the reaction 2H
S(
g
) 2H (
g
) + S
(
g
), K
= 9.1 ×
10
at 750 K. What
will happen when 0.10 mol of H
S, 1.0 mol of H
, and 1.5 mol of S
are added to
a 1.0-L container and the system is brought to 750 K?
2
2
2
c
2
2
2
2
More H
will be formed than S
.
2
2
The amount of H
formed will be half the amount of S
formed.
2
2
More S
will be formed than H
.
2
2
Nothing; the system is at equilibrium.
More H
S will be formed.
2
1 / 1 pts
Question 9
For the equilibrium PCl
(
g
) PCl (
g
) + Cl
(
g
), K
= 4.0 at 228°C. If pure
PCl
is placed in a 1.00-L container and allowed to come to equilibrium, and the
equilibrium concentration of PCl
(
g
) is 0.26 M
, what is the equilibrium
concentration of PCl
?
5
3
2
c
5
5
3
0.95 M
1.0 M
0.38 M
0.11 M
0.23 M
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1 / 1 pts
Question 10
For the equilibrium N
O (
g
) 2NO (
g
), at 298 K, K
= 0.15. For this
reaction system, it is found that the partial pressure of N
O
is 3.5 ×
10
atm at
equilibrium. What is the partial pressure of NO
at equilibrium? (
R
= 0.0821 L atm/(K mol))
2
4
2
p
2
4
–2
2
0.0052 atm
23 atm
0.072 atm
4.8 atm
0.0018 atm
1 / 1 pts
Question 11
The equilibrium constant for the reaction H
(
g
) + I
(
g
) 2HI(
g
) is 62.5 at
800 K. What is the equilibrium concentration of I
if at equilibrium [HI] = 0.21 M
and [H
] = 0.13 M
?
2
2
2
2
5.4 ×
10
M
–3
2.6 ×
10
M
–2
5.2 ×
10
M
–2
0.29 M
0.21 M
9/20/22, 2:20 AM
Chapter 13 - Chemical Equilibrium: General Chemistry: 2022FA-CHEM-001B-202
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8/13
1 / 1 pts
Question 12
In an experiment, 0.30 mol H
and 0.30 mol I
are mixed in a 1.00-L container,
and the reaction forms HI. If K
= 49. for this reaction, what is the equilibrium
concentration of HI?
I (
g
) + H
(
g
) 2HI(
g
)
2
2
c
2
2
0.47 M
0.040 M
0.075 M
0.53 M
0.58 M
1 / 1 pts
Question 13
Hydrogen iodide undergoes decomposition according to the equation
2HI(
g
) H (
g
) + I
(
g
)
The equilibrium constant K
at 500 K for this equilibrium is 0.060. Suppose 0.811
mol of HI is placed in a 1.50-L container at 500 K. What is the equilibrium
concentration of H
(
g
)? (
R
= 0.0821 L atm/(K mol))
2
2
p
2
0.21 M
0.039 M
0.089 M
9/20/22, 2:20 AM
Chapter 13 - Chemical Equilibrium: General Chemistry: 2022FA-CHEM-001B-202
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9/13
4.3 M
0.1 M
1 / 1 pts
Question 14
At 700 K, K
for the following equilibrium is 5.6 ×
10 .
2HgO(
s
) 2Hg(
l
) + O
(
g
)
Suppose 72.2 g of mercury(II) oxide is placed in a sealed 1.00-L vessel at 700
K. What is the partial pressure of oxygen gas at equilibrium? (
R
= 0.0821 L atm/(K mol))
p
-3
2
0.0056 atm
57 atm
19 atm
9.5 atm
0.074 atm
1 / 1 pts
Question 15
At 550 K, K
= 7.7 × 10
for the following equilibrium.
SO (
g
) + NO
(
g
) SO (
g
) + NO(
g
)
If 0.279 mol each of SO
and NO are placed in a 4.00-L container at 550 K, what
is the concentration of SO
at equilibrium? (
R
= 0.0821 L · atm/(K · mol))
p
2
2
2
3
3
3
0.067 M
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0.069 M
17 M
3 M
0.017 M
1 / 1 pts
Question 16
Which of the following equilibria would be affected by volume changes at
constant temperature? 1.
2NO(
g
) + 3F
(
g
) 2F NO(
g
)
2.
PCl (
g
) + Cl
(
g
) PCl (
g
)
3.
O (
g
) + NO(
g
) NO (
g
) + O
(
g
)
2
3
3
2
5
3
2
2
2 only
1 only
1 and 2
1, 2, and 3
3 only
1 / 1 pts
Question 17
Ammonia is prepared industrially by the reaction
N (
g
) + 3H
(
g
) 2NH (
g
)
2
2
3
9/20/22, 2:20 AM
Chapter 13 - Chemical Equilibrium: General Chemistry: 2022FA-CHEM-001B-202
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11/13
For the reaction, Δ
H
° = –92.2 kJ and K
(at 25°C) = 4.0 × 10
. When the
temperature of the reaction is increased to 500°C, which of the following
statements is true?
8
At equilibrium, more NH
is present at 500°C than at 25°C.
3
None of the above statements is true.
Product formation (at equilibrium) is less favored as the temperature is
raised.
K
for the reaction will be larger at 500°C than at 25°C.
The reaction of N
with H
to form ammonia is endothermic.
2
2
1 / 1 pts
Question 18
One method for the decomposition of carbon dioxide proceeds as follows:
2CO (
g
) 2CO(
g
) + O
(
g
); Δ
H
= 559 kJ
Which of the following changes will cause an increase in the equilibrium
concentration of CO?
2
2
increasing the pressure of the system at constant temperature
adding a catalyst
removing CO
from the system
2
adding more O
to the system
2
increasing the temperature of the system
9/20/22, 2:20 AM
Chapter 13 - Chemical Equilibrium: General Chemistry: 2022FA-CHEM-001B-202
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1 / 1 pts
Question 19
For the following reaction system at equilibrium, which one of the changes below
would cause the equilibrium to shift to the right?
Br (
g
) + 2NO(
g
) 2NOBr(
g
); Δ
H
° = –30 kJ
2
Add some NOBr.
Decrease the temperature.
Increase the volume of the reaction vessel.
Remove some NO.
Remove some Br
.
2
1 / 1 pts
Question 20
Consider the following system at equilibrium: N
(
g
) + 3H
(
g
) 2NH (
g
);
Δ
H
° = -92.94 kJ Which of the following changes will shift the equilibrium to the
right?
I.increasing the temperature
II.decreasing the temperature
III.increasing the volume
IV.decreasing the volume
V.removing some NH
VI.adding some NH
VII.
removing some N
2
2
3
3
3
2
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VIII. adding some N
2
I, IV, VI, VII
II, III, V, VIII
I, III, V, VII
I, VI, VIII
II, IV, V, VIII
Quiz Score: 20
out of 20
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The hydrogen gas formed in a chemical reaction is collected over water at 30 °C at a total pressure of 732 mm Hg . The vapor pressure
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[l]o (M)
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0.0100
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2.00
Experiment #
Rate (M/s)
1
2.63 x10-6
5.58
0.0200
1.70
5.18 x 106
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8.01 x 10-6
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4
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Value of n (2 significant figures):
verage value of k (3 significant figures):
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PERTINENT CALCULATIONS
Remember:
rate = k[C25H30CIN3]"[OH_]" where n =0 since excess OH was used.
n3=
1. Refer to your graphs and complete table below
Linear correlation (r- value)
Graph
Kinetic Run I
Kinetic Run II Average r- value
absorbance vs time
0.9972
0.9955
0.9964
In (absorbance) vs time
0.9978
0.9994
0.9986
2/(absorbance) vs time
0.9805
0.9879
0.9952
2. Based on the average linear correlation (r2 -value) the reaction order, m, with respect to crystal
violet, CV, is
Explain.
3. Write the rate law.
4.
The slope, and therefore pseudo" rate constant, kr', is
at T1.
CC, and ko' is
at T2
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A thru D has already been answered. Please show parts E and F
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2I– (aq) + H2O2 (aq) + 2H3O + (aq) → I2 (aq) + 4H2O (l) (slow)
C6H8O6 (aq) + 2H2O (l) + I2 (aq) → C6H6O6 (aq) + 2H3O + (aq) + 2I– (aq) (very fast)
I2 (aq) + I– (aq) ⇌ I3- (aq)
I3- (aq) + starch → blue I3- · starch complex (aq) (fast)
A 0.100 L solution is prepared with initial concentrations of 4.0 × 10−3 M iodine I2 , 8.0×10−3 M iodide I– , and 5.0×10−3 M ascorbic acid C6H8O6 . After the second reaction goes to completion, what will the molar concentrations of iodide and ascorbic acid in the solution be?
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2I– (aq) + H2O2 (aq) + 2H3O + (aq) → I2 (aq) + 4H2O (l) (slow)
C6H8O6 (aq) + 2H2O (l) + I2 (aq) → C6H6O6 (aq) + 2H3O + (aq) + 2I– (aq) (very fast)
I2 (aq) + I– (aq) ⇌ I – 3 (aq)
I3- (aq) + starch → blue I3- · starch complex (aq) (fast)
A different 0.100 L reaction mixture is prepared with initial concentrations of 1.0×10−2 M iodide I– , 2.0 × 10−3 M ascorbic acid C6H8O6 , and 0.135 M hydrogen peroxide H2O2 . If the first two reactions above procede at the same rate (they’re limited by the first one!), which of these reactants will be completely consumed first?
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Reaction kinetics lab
Can anyone help me to answer the question please?
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A 100%
7:07 PM Wed Feb 5
3
...
Unanswered •1 attempt left
Rate law of a reaction is experimentally determined as
Rate = k [A]^2 [B]
The unit of k is
1/(M^2-sec)
1/(M-sec)
sec/M
M/sec
M^2/sec
Submit
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