For the reaction: 4P + 3Q → 2R the following data were obtained at constant temperature Initial [Q] (mol/L) 0.100 Initial [P] (mol/L) 0.100 Experiment Initial Rate (mol/L.min) 5.00 1 45.0 0.300 0.100 10.0 0.100 0.200 4 90.0 0.300 0.200 a. What is the order of the reaction with respect to each reactant? b. Write the rat law of the reaction. c. Calculate k( using the data from Experiment 1)
For the reaction: 4P + 3Q → 2R the following data were obtained at constant temperature Initial [Q] (mol/L) 0.100 Initial [P] (mol/L) 0.100 Experiment Initial Rate (mol/L.min) 5.00 1 45.0 0.300 0.100 10.0 0.100 0.200 4 90.0 0.300 0.200 a. What is the order of the reaction with respect to each reactant? b. Write the rat law of the reaction. c. Calculate k( using the data from Experiment 1)
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 11.35PAE: 11.35 For the reaction 2 NO(g) + 2 H?(g) — N,(g) + 2 H,O(g) at 1100°C, the following data have been...
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![For the reaction: 4P + 3Q → 2R
|
the following data were obtained at constant temperature
Initial [Q]
(mol/L)
0.100
Initial [P]
(mol/L)
0.100
Experiment
Initial Rate
(mol/L.min)
5.00
1
45.0
0.300
0.100
10.0
0.100
0.200
4
90.0
0.300
0.200
a. What is the order of the reaction with respect to each reactant?
b. Write the rat law of the reaction.
c. Calculate k( using the data from Experiment 1)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F896fb524-faf8-45ec-8446-caa6404eff3d%2F9de9b1ad-fef2-4e7f-a2ca-b2ab517fd457%2F8dmu2mij_processed.jpeg&w=3840&q=75)
Transcribed Image Text:For the reaction: 4P + 3Q → 2R
|
the following data were obtained at constant temperature
Initial [Q]
(mol/L)
0.100
Initial [P]
(mol/L)
0.100
Experiment
Initial Rate
(mol/L.min)
5.00
1
45.0
0.300
0.100
10.0
0.100
0.200
4
90.0
0.300
0.200
a. What is the order of the reaction with respect to each reactant?
b. Write the rat law of the reaction.
c. Calculate k( using the data from Experiment 1)
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