A study of the gas-phase oxidation of nitrogen monoxide at 25°C gave the following results: 2NO (g) + 2H2(g) → N2(g) + 2H20(g) [NO] [H:] Rate (M/s) Exp. 1 4.5 x 102 2.2 x 102 0.1475 Exp. 2 4.5 x 102 6.6 x 102 0.4425 Exp. 3 1.35 x 10 6.6 x 102 3.9825 a) Determine the rate law for this reaction (Show work). b) Determine the rate constant for this reaction (include units).
A study of the gas-phase oxidation of nitrogen monoxide at 25°C gave the following results: 2NO (g) + 2H2(g) → N2(g) + 2H20(g) [NO] [H:] Rate (M/s) Exp. 1 4.5 x 102 2.2 x 102 0.1475 Exp. 2 4.5 x 102 6.6 x 102 0.4425 Exp. 3 1.35 x 10 6.6 x 102 3.9825 a) Determine the rate law for this reaction (Show work). b) Determine the rate constant for this reaction (include units).
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
Chapter12: Chemical Kinetics
Section: Chapter Questions
Problem 120CP: Consider the following hypothetical data collected in two studies of the reaction 2A+2BC+2D Time(s)...
Related questions
Question
![A study of the gas-phase oxidation of nitrogen monoxide at 25°C gave the following results:
2NO (g) + 2H2(g) → N2(g) + 2H20(g)
[NO]
[H:]
Rate (M/s)
Exp. 1
4.5 x 102
2.2 x 102
0.1475
Exp. 2
4.5 x 102
6.6 x 102
0.4425
Exp. 3
1.35 x 101
6.6 x 102
3.9825
a) Determine the rate law for this reaction (Show work).
b) Determine the rate constant for this reaction (include units).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2bf10666-6497-439e-b69b-316cab94ca4b%2Fe10c3a99-9a9d-4895-a501-d0abb12b5788%2Fnkt0qsh_processed.jpeg&w=3840&q=75)
Transcribed Image Text:A study of the gas-phase oxidation of nitrogen monoxide at 25°C gave the following results:
2NO (g) + 2H2(g) → N2(g) + 2H20(g)
[NO]
[H:]
Rate (M/s)
Exp. 1
4.5 x 102
2.2 x 102
0.1475
Exp. 2
4.5 x 102
6.6 x 102
0.4425
Exp. 3
1.35 x 101
6.6 x 102
3.9825
a) Determine the rate law for this reaction (Show work).
b) Determine the rate constant for this reaction (include units).
Expert Solution
Step 1
To determine rate law, first calculate order of NO and H2 by using trial values given. Using that value find out rate constant for given data.
Trending now
This is a popular solution!
Step by step
Solved in 6 steps
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
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:
9781337398909
Author:
Lawrence S. Brown, Tom Holme
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:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning