The proposed 3-step mechanism for a reaction is - A(g) fast, reaches equilibrium (For Step 1, k1 = forward rate constant & k.1 = reverse rate constant.) B(g) slow (k2 = rate constant) Step 1) X(g) + Y(g) %3D Step 2) A(g) + Z(g) -> %3D Step 3) B(g) P(g) fast (k3 = rate constant) a) What is the overall reaction? b) What is the rate law supported by this mechanism? Explain your answer. c) The following is experimental data found for this reaction: Initial [X] Initial [Y] Initial [Z] Initial Rate (M) (M) (M) (M/day) Exp 1 0.150 0.150 0.150 0.569 Exp 2 0.250 0.150 0.150 0.948 Exp 3 0.250 0.300 0.150 3.793 Exp 4 0.300 0.350 0.200 6.196 i) What is the experimentally determined rate law? ii) Determine the rate constant and include units. d) Does your experimentally determined rate law support the proposed mechanism? Explain your answer. e) AH° = +347 kJ/mol for the overall reaction. Draw a reasonable reaction profile for the proposed mechanism. Label your profile with the proper reactants, products, and intermediates. Indicate where the activated complexes would be. You can write the activated complexes as 'AC'. Be sure to label your axis.
The proposed 3-step mechanism for a reaction is - A(g) fast, reaches equilibrium (For Step 1, k1 = forward rate constant & k.1 = reverse rate constant.) B(g) slow (k2 = rate constant) Step 1) X(g) + Y(g) %3D Step 2) A(g) + Z(g) -> %3D Step 3) B(g) P(g) fast (k3 = rate constant) a) What is the overall reaction? b) What is the rate law supported by this mechanism? Explain your answer. c) The following is experimental data found for this reaction: Initial [X] Initial [Y] Initial [Z] Initial Rate (M) (M) (M) (M/day) Exp 1 0.150 0.150 0.150 0.569 Exp 2 0.250 0.150 0.150 0.948 Exp 3 0.250 0.300 0.150 3.793 Exp 4 0.300 0.350 0.200 6.196 i) What is the experimentally determined rate law? ii) Determine the rate constant and include units. d) Does your experimentally determined rate law support the proposed mechanism? Explain your answer. e) AH° = +347 kJ/mol for the overall reaction. Draw a reasonable reaction profile for the proposed mechanism. Label your profile with the proper reactants, products, and intermediates. Indicate where the activated complexes would be. You can write the activated complexes as 'AC'. Be sure to label your axis.
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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![The proposed 3-step mechanism for a reaction is
Step 1) X(g) + Y(g)
A(g) fast, reaches equilibrium
(For Step 1, k1 = forward rate constant & k.1
= reverse rate constant.)
%3D
Step 2) A(g) + Z(g)
Step 3) B(g)
B(g) slow (k2 = rate constant)
P(g) fast (k3 = rate constant)
>
a) What is the overall reaction?
b) What is the rate law supported by this mechanism? Explain your answer.
c) The following is experimental data found for this reaction:
Initial [X] Initial [Y] Initial [Z]
Initial Rate
(M)
(M)
(M)
(M/day)
Exp 1
0.150
0.150
0.150
0.569
Exp 2
0.250
0.150
0.150
0.948
Exp 3
0.250
0.300
0.150
3.793
Exp 4
0.300
0.350
0.200
6.196
i) What is the experimentally determined rate law?
ii) Determine the rate constant and include units.
d) Does your experimentally determined rate law support the proposed mechanism? Explain your
answer.
e) AH° = +347 kJ/mol for the overall reaction. Draw a reasonable reaction profile for the proposed
mechanism. Label your profile with the proper reactants, products, and intermediates. Indicate
where the activated complexes would be. You can write the activated complexes as 'AC. Be sure
to label your axis.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9421a115-c6e2-48c9-bd20-aae23743c2e8%2F7ebd1b36-6dbf-44c3-8721-051746bc172b%2F4zl7q4g_processed.png&w=3840&q=75)
Transcribed Image Text:The proposed 3-step mechanism for a reaction is
Step 1) X(g) + Y(g)
A(g) fast, reaches equilibrium
(For Step 1, k1 = forward rate constant & k.1
= reverse rate constant.)
%3D
Step 2) A(g) + Z(g)
Step 3) B(g)
B(g) slow (k2 = rate constant)
P(g) fast (k3 = rate constant)
>
a) What is the overall reaction?
b) What is the rate law supported by this mechanism? Explain your answer.
c) The following is experimental data found for this reaction:
Initial [X] Initial [Y] Initial [Z]
Initial Rate
(M)
(M)
(M)
(M/day)
Exp 1
0.150
0.150
0.150
0.569
Exp 2
0.250
0.150
0.150
0.948
Exp 3
0.250
0.300
0.150
3.793
Exp 4
0.300
0.350
0.200
6.196
i) What is the experimentally determined rate law?
ii) Determine the rate constant and include units.
d) Does your experimentally determined rate law support the proposed mechanism? Explain your
answer.
e) AH° = +347 kJ/mol for the overall reaction. Draw a reasonable reaction profile for the proposed
mechanism. Label your profile with the proper reactants, products, and intermediates. Indicate
where the activated complexes would be. You can write the activated complexes as 'AC. Be sure
to label your axis.
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