2NO+ O2 → 2NO2 Experiment [NO], M [0₂], M 0.00302 0.00287 0.00604 0.00287 0.00574 0.00574 1 2 3 4 Rate = 0.00302 0.00604 k= Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Initial Rate, M. s-¹ 0.000231 0.000923 0.000462 M-2.s-1 0.00185
2NO+ O2 → 2NO2 Experiment [NO], M [0₂], M 0.00302 0.00287 0.00604 0.00287 0.00574 0.00574 1 2 3 4 Rate = 0.00302 0.00604 k= Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Initial Rate, M. s-¹ 0.000231 0.000923 0.000462 M-2.s-1 0.00185
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 11.36PAE: The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in...
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![The following initial rate data are for the oxidation of nitrogen monoxide by oxygen at 25 °C:
2NO+ O2 → 2NO2
-1
Experiment [NO]o, M [O2]o, M Initial Rate, M-s-¹
S
0.00302
0.00287 0.000231
0.00604
0.00287
0.000923
0.00302
0.00574
0.000462
0.00604
0.00574
1
2
3
4
Complete the rate law for this reaction in the box below.
Use the form k[A] [B]", where '1' is understood for m or n and concentrations taken to the zero power
do not appear. Don't enter 1 for m or n.
Rate =
k=
0.00185
M-2.s-1
S](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F79598ce0-8110-4c0e-a509-3cd8fbd6fa16%2Fc3761a2e-ea83-4524-88c4-555237a9d977%2Fg029ra_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The following initial rate data are for the oxidation of nitrogen monoxide by oxygen at 25 °C:
2NO+ O2 → 2NO2
-1
Experiment [NO]o, M [O2]o, M Initial Rate, M-s-¹
S
0.00302
0.00287 0.000231
0.00604
0.00287
0.000923
0.00302
0.00574
0.000462
0.00604
0.00574
1
2
3
4
Complete the rate law for this reaction in the box below.
Use the form k[A] [B]", where '1' is understood for m or n and concentrations taken to the zero power
do not appear. Don't enter 1 for m or n.
Rate =
k=
0.00185
M-2.s-1
S
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