The reaction of nitric oxide with hydrogen at 1280°C is: 2 NO(g) + 2 H2(g) → N2(g) + 2 H₂O(g) From the following data determine the rate law and rate constant: Experiment 1 2 3 [NO] 5.0 x 10-3 10.0 × 10-3 10.0 x 10-3 [H₂] 2.0 × 10-3 2.0 × 10-3 4.0 × 10-3 Initial Rate (M/s) 1.3 x 10-5 5.0 x 10-5 10.0 × 10-5
The reaction of nitric oxide with hydrogen at 1280°C is: 2 NO(g) + 2 H2(g) → N2(g) + 2 H₂O(g) From the following data determine the rate law and rate constant: Experiment 1 2 3 [NO] 5.0 x 10-3 10.0 × 10-3 10.0 x 10-3 [H₂] 2.0 × 10-3 2.0 × 10-3 4.0 × 10-3 Initial Rate (M/s) 1.3 x 10-5 5.0 x 10-5 10.0 × 10-5
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 41E: The rate of the reaction NO2(g)+CO(g)NO(g)+CO2(g) depends only on the concentration of nitrogen...
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Question
What order would you predict for [H2]?
A. Zero
b. First
c. Second
d. Cannot be predicted from the information given
![The reaction of nitric oxide with hydrogen at
1280°C is: 2 NO(g) + 2 H₂(g) → N2(g) + 2 H₂O(g)
From the following data determine the rate law
and rate constant:
Experiment
1
2
3
[NO]
5.0 x 10-3
10.0 x 10-3
10.0 x 10-3
[H₂]
2.0 × 10-³
2.0 x 10-³
4.0 × 10-³
Initial Rate (M/s)
1.3 x 10-5
5.0 x 10-5
10.0 x 10-5](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1d538ef5-6095-46a7-a26b-352fc3cbaffd%2Fba11c440-3045-4e48-99e8-7dd8ca61dda2%2Fkpb84a9_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The reaction of nitric oxide with hydrogen at
1280°C is: 2 NO(g) + 2 H₂(g) → N2(g) + 2 H₂O(g)
From the following data determine the rate law
and rate constant:
Experiment
1
2
3
[NO]
5.0 x 10-3
10.0 x 10-3
10.0 x 10-3
[H₂]
2.0 × 10-³
2.0 x 10-³
4.0 × 10-³
Initial Rate (M/s)
1.3 x 10-5
5.0 x 10-5
10.0 x 10-5
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