1. For the reaction 2A + B + C → products, the law rate takes the form of: r=k [A]"[B]^[C]°. Why aren't the coefficients in the balanced equation always the exponents in the rate law?
1. For the reaction 2A + B + C → products, the law rate takes the form of: r=k [A]"[B]^[C]°. Why aren't the coefficients in the balanced equation always the exponents in the rate law?
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![Rate Law Problems
1. For the reaction 2A +B +C→ products, the law rate takes the form of:
r =k [A]M[B]^[C]°. Why aren't the coefficients in the balanced equation always the
exponents in the rate law?
2. If 2A +B → C+D+ energy represents a one step reaction.
a) Write the rate law.
b) How is the initial rate of the reaction affected by the following changes:
(i)
Tripling the concentration of A
(ii) Decreasing the size of the container by ½.
3. Consider the net reaction 3A + 4B → products, the following data were obtained:
Initial [A]
Initial [B]
Initial Rate
10 M/min
40 M/min
10 M/min
90 M/min
Experiment
1
2.0 M
4.0 M
2.0 M
6.0 M
4.0 M
2
3
2.0 M
10.0 M
4
4.0 M
4. a) What is the rate law for the reaction 2A+2B → C+D if the following is the
reaction mechanism?
2B →E
A+E>F+C
A+F>D
Step #1 (slow)
Step #2 (fast)
Step #3 (fast)
b) Ifk=0.012 liters/mole-min., what is the rate when [A] = 2.0 M and [B] = 4.0
M?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa0ce2a49-b6bf-4429-b2ce-d0e29fd78daf%2F697b4676-33a8-4eb7-a6a8-d838a7db2f10%2Fwko8o4id_processed.png&w=3840&q=75)
Transcribed Image Text:Rate Law Problems
1. For the reaction 2A +B +C→ products, the law rate takes the form of:
r =k [A]M[B]^[C]°. Why aren't the coefficients in the balanced equation always the
exponents in the rate law?
2. If 2A +B → C+D+ energy represents a one step reaction.
a) Write the rate law.
b) How is the initial rate of the reaction affected by the following changes:
(i)
Tripling the concentration of A
(ii) Decreasing the size of the container by ½.
3. Consider the net reaction 3A + 4B → products, the following data were obtained:
Initial [A]
Initial [B]
Initial Rate
10 M/min
40 M/min
10 M/min
90 M/min
Experiment
1
2.0 M
4.0 M
2.0 M
6.0 M
4.0 M
2
3
2.0 M
10.0 M
4
4.0 M
4. a) What is the rate law for the reaction 2A+2B → C+D if the following is the
reaction mechanism?
2B →E
A+E>F+C
A+F>D
Step #1 (slow)
Step #2 (fast)
Step #3 (fast)
b) Ifk=0.012 liters/mole-min., what is the rate when [A] = 2.0 M and [B] = 4.0
M?
![More Rate Law Problems
1.
a) Write the rate law for the one step reaction 2NO → N;Oz9).
b) If the rate of the disappearance of NO is 0.5 M-min" when the
concentration of NO is 2.02 M, find the value of k.
c) What is the rate of disappearance of NO if the concentration of NO is
1.0 x 10° M?
d) How does the rate change when (NO) is (a) doubled and (b) cut to 1/3?
2. The net reaction A+B+2C → D+E @ 400°C follows the rate law, r=k[A]°[C]
a) Complete the blanks in the following table:
Experiment
[A]
[B]
mol/L
|C)
k
rate
mol/L
mol/L
mol/L'min
2.0
4.0
2.0
1.0
2
2.0
1.0
b) How may the value of the specific rate constant be increased for the above
reaction?
3. If buming of CO [2CO + O2→ 200,], proceeds by the steps:
02 + 20
2C0 + 20 → 2002
If the activation energy is much greater for (1) than (2), what is the rate law?
(1)
(2)
4.
a) What is the rate law for 2A + 3B → 2C + D if the following data is
obtained:
Experiment [A]
mol/L
[B]
mol/L
rate
mol/L's
0.11 x 10
1.0 x 10
1.0 x 10
1
0.5
1.5
1.5
2.0
4.0
2.0
2
3
b) Find the value of the specific rate constant.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa0ce2a49-b6bf-4429-b2ce-d0e29fd78daf%2F697b4676-33a8-4eb7-a6a8-d838a7db2f10%2Fcfhgrb8_processed.png&w=3840&q=75)
Transcribed Image Text:More Rate Law Problems
1.
a) Write the rate law for the one step reaction 2NO → N;Oz9).
b) If the rate of the disappearance of NO is 0.5 M-min" when the
concentration of NO is 2.02 M, find the value of k.
c) What is the rate of disappearance of NO if the concentration of NO is
1.0 x 10° M?
d) How does the rate change when (NO) is (a) doubled and (b) cut to 1/3?
2. The net reaction A+B+2C → D+E @ 400°C follows the rate law, r=k[A]°[C]
a) Complete the blanks in the following table:
Experiment
[A]
[B]
mol/L
|C)
k
rate
mol/L
mol/L
mol/L'min
2.0
4.0
2.0
1.0
2
2.0
1.0
b) How may the value of the specific rate constant be increased for the above
reaction?
3. If buming of CO [2CO + O2→ 200,], proceeds by the steps:
02 + 20
2C0 + 20 → 2002
If the activation energy is much greater for (1) than (2), what is the rate law?
(1)
(2)
4.
a) What is the rate law for 2A + 3B → 2C + D if the following data is
obtained:
Experiment [A]
mol/L
[B]
mol/L
rate
mol/L's
0.11 x 10
1.0 x 10
1.0 x 10
1
0.5
1.5
1.5
2.0
4.0
2.0
2
3
b) Find the value of the specific rate constant.
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