The rate for the overall reaction NO2 (g) + CO (g) ® NO (g) + CO2 (g) is Rate = k[NO2]2. Consider this mechanism: 2 NO2 (g) ® N2 (g) + 2 O2 (g) [slow] 2 CO (g) + O2 (g) ® 2 CO2 (g) [fast] N2 (g) + O2 (g) ®2 NO (g) [fast] Is this reaction mechanism consistent with the rate law? Why or Why not? 2. Write the rate laws for the intermediate steps. 3. List the reaction intermediates present in this mechanism. 4. Draw a reaction energy diagram for this mechanism, given that the overall reaction’s ΔH°rxn = -226 kJ/mol.
The rate for the overall reaction NO2 (g) + CO (g) ® NO (g) + CO2 (g) is Rate = k[NO2]2. Consider this mechanism: 2 NO2 (g) ® N2 (g) + 2 O2 (g) [slow] 2 CO (g) + O2 (g) ® 2 CO2 (g) [fast] N2 (g) + O2 (g) ®2 NO (g) [fast] Is this reaction mechanism consistent with the rate law? Why or Why not? 2. Write the rate laws for the intermediate steps. 3. List the reaction intermediates present in this mechanism. 4. Draw a reaction energy diagram for this mechanism, given that the overall reaction’s ΔH°rxn = -226 kJ/mol.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter11: Chemical Kinetics: Rates Of Reactions
Section11.7: Reaction Mechanisms
Problem 11.12E
Related questions
Question
The rate for the overall reaction
NO2 (g) + CO (g) ® NO (g) + CO2 (g)
is Rate = k[NO2]2.
- Consider this mechanism:
- 2 NO2 (g) ® N2 (g) + 2 O2 (g) [slow]
- 2 CO (g) + O2 (g) ® 2 CO2 (g) [fast]
- N2 (g) + O2 (g) ®2 NO (g) [fast]
Is this reaction mechanism consistent with the rate law? Why or Why not?
2. Write the rate laws for the intermediate steps.
3. List the reaction intermediates present in this mechanism.
4. Draw a reaction energy diagram for this mechanism, given that the overall reaction’s ΔH°rxn = -226 kJ/mol.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 3 steps with 4 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781133949640
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781133949640
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning