The following initial rate data are for the oxidation of nitrogen monoxide by oxygen at 25 °C: 2 NO + 0,2 NO, NO], M 3 יו 7 | 1.54x10-2 7.70x10-3 1.54x10-2 [0:],, M 1.01×10-3 1.01×10-3 2.02x10-3 2.02x10-3 Experiment |Initial Rate, M s- 5.07x104 2.03x10-3 1.01×10-3 4.06x10-3 1 2 3 Complete the rate law for this reaction in the box below. Use the form k[A]®[B]" , where 'l' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter1 for m or n. Rate = From these data, the rate constant is
The following initial rate data are for the oxidation of nitrogen monoxide by oxygen at 25 °C: 2 NO + 0,2 NO, NO], M 3 יו 7 | 1.54x10-2 7.70x10-3 1.54x10-2 [0:],, M 1.01×10-3 1.01×10-3 2.02x10-3 2.02x10-3 Experiment |Initial Rate, M s- 5.07x104 2.03x10-3 1.01×10-3 4.06x10-3 1 2 3 Complete the rate law for this reaction in the box below. Use the form k[A]®[B]" , where 'l' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter1 for m or n. Rate = From these data, the rate constant is
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:
2 NO + 0,2 NO,
Experiment
NO]o, M
7.70x10-3
1.54x10-2
7.70x10-3
1.54x10-2
[0:], M
Initial Rate, Ms-1
5.07x10-4
2.03x10-3
1.01x10-3
4.06x10-3
1
1.01×10-3
1.01x10-3
2.02x10-3
2.02x10-3
2
13
14
Complete the rate law for this reaction in the box below.
Use the form k[A]m[B]" , where 'l' 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 =
From these data, the rate constant is](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fca28178a-3d47-4681-8e63-a516498b8666%2Fb3c923a1-6432-41ca-8430-71b985c088e3%2Ff98b1ha_processed.png&w=3840&q=75)
Transcribed Image Text:The following initial rate data are for the oxidation of nitrogen monoxide by oxygen at 25 °C:
2 NO + 0,2 NO,
Experiment
NO]o, M
7.70x10-3
1.54x10-2
7.70x10-3
1.54x10-2
[0:], M
Initial Rate, Ms-1
5.07x10-4
2.03x10-3
1.01x10-3
4.06x10-3
1
1.01×10-3
1.01x10-3
2.02x10-3
2.02x10-3
2
13
14
Complete the rate law for this reaction in the box below.
Use the form k[A]m[B]" , where 'l' 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 =
From these data, the rate constant is
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