4. The reaction 2NO (g) + 2H2 (g) N2 (g) + 2H;O (g) is found experimentally to be second order in NO (g) and first-order in H2 (g). a. Write the rate law for the reaction. b. What is the overall order of the reaction? c. What are the units for the rate constant k?
4. The reaction 2NO (g) + 2H2 (g) N2 (g) + 2H;O (g) is found experimentally to be second order in NO (g) and first-order in H2 (g). a. Write the rate law for the reaction. b. What is the overall order of the reaction? c. What are the units for the rate constant k?
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions
Section14.7: Reaction Mechanisms
Problem 14.14CYU: One possible mechanism for the decomposition of nitryl chloride, NO2CI, is What is the overall...
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![4. The reaction 2NO (g) + 2H2 (g)
- N2 (g) + 2H2O (g) is found experimentally to be second
order in NO (g) and first-order in H2 (g).
a. Write the rate law for the reaction.
b. What is the overall order of the reaction?
c. What are the units for the rate constant k?
d. If [NO] is doubled (while keeping [H2] constant), by what factor will the reaction rate
increase?
e. If [H2] is doubled (while keeping [NO] constant), by what factor will the reaction rate
increase?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6b574d51-0fdb-495e-9b46-97198cf41098%2F99a3e657-792f-4b29-a18c-b7be4c2b2c8f%2Fsjngc3k_processed.jpeg&w=3840&q=75)
Transcribed Image Text:4. The reaction 2NO (g) + 2H2 (g)
- N2 (g) + 2H2O (g) is found experimentally to be second
order in NO (g) and first-order in H2 (g).
a. Write the rate law for the reaction.
b. What is the overall order of the reaction?
c. What are the units for the rate constant k?
d. If [NO] is doubled (while keeping [H2] constant), by what factor will the reaction rate
increase?
e. If [H2] is doubled (while keeping [NO] constant), by what factor will the reaction rate
increase?
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