Use the following chart to determine the rate law of the equation A + B → P Experiment # [A] (M) [B] (M) Rate (M/s) 1 0.088 0.013 2.52 x 10-3 2 0.088 0.026 5.06 x 10-3 3 0.044 0.026 2.52 x 10-3 k[A][B] k[P] k[A]2[B] k[A]2[B]2 k[A]2 2. The magnitude of the rate constant in question 1 is ________. a).001 b).025 c) 2.21 d) 2.50 e) 28.2
Use the following chart to determine the rate law of the equation A + B → P Experiment # [A] (M) [B] (M) Rate (M/s) 1 0.088 0.013 2.52 x 10-3 2 0.088 0.026 5.06 x 10-3 3 0.044 0.026 2.52 x 10-3 k[A][B] k[P] k[A]2[B] k[A]2[B]2 k[A]2 2. The magnitude of the rate constant in question 1 is ________. a).001 b).025 c) 2.21 d) 2.50 e) 28.2
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter11: Chemical Kinetics
Section: Chapter Questions
Problem 11.102PAE: 11.102 Suppose that you are studying a reaction and need to determine its rate law. Explain what you...
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Question
1. Use the following chart to determine the rate law of the equation A + B → P
Experiment # |
[A] (M) |
[B] (M) |
Rate (M/s) |
1 |
0.088 |
0.013 |
2.52 x 10-3 |
2 |
0.088 |
0.026 |
5.06 x 10-3 |
3 |
0.044 |
0.026 |
2.52 x 10-3 |
- k[A][B]
- k[P]
- k[A]2[B]
- k[A]2[B]2
- k[A]2
2. The magnitude of the rate constant in question 1 is ________.
a).001
b).025
c) 2.21
d) 2.50
e) 28.2
Number 1 info needed for numberr 2
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