The following initial rate data are for the oxidation of nitrogen monoxide by oxygen at 25 °C: 2NO+O2 → 2NO2 Experiment [NO]o, M [0₂]0, M Initial Rate, M. s-¹ 0.00338 0.00224 0.000226 0.00676 0.00224 0.000903 0.00338 0.00448 0.000451 0.00676 0.00448 0.00181 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 = 1 2 3 4 k - M-2 . s-1
The following initial rate data are for the oxidation of nitrogen monoxide by oxygen at 25 °C: 2NO+O2 → 2NO2 Experiment [NO]o, M [0₂]0, M Initial Rate, M. s-¹ 0.00338 0.00224 0.000226 0.00676 0.00224 0.000903 0.00338 0.00448 0.000451 0.00676 0.00448 0.00181 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 = 1 2 3 4 k - M-2 . s-1
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter11: Chemical Kinetics: Rates Of Reactions
Section: Chapter Questions
Problem 109QRT
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![The following initial rate data are for the oxidation of nitrogen monoxide by oxygen at 25 °C:
2NO+ O₂ → 2NO2
Experiment [NO], M [0₂]o, M
0.00338
0.00224
0.00676
0.00224
0.00338
0.00448
0.00676
0.00448
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 =
1
2
B
4
P
1
Initial Rate, M-s¯¹
S
0.000226
0.000903
0.000451
0.00181
M-2.s-¹
S](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2a948ce4-bfec-4c4b-a693-d4721e6497c9%2F062f1986-7200-48d6-8569-e35e48861832%2F6so9y8e_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
Experiment [NO], M [0₂]o, M
0.00338
0.00224
0.00676
0.00224
0.00338
0.00448
0.00676
0.00448
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 =
1
2
B
4
P
1
Initial Rate, M-s¯¹
S
0.000226
0.000903
0.000451
0.00181
M-2.s-¹
S
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