1.The oxidation of nitrogen monoxide by oxygen at 25 oC 2 NO + O22 NO2 is second order in NO and first order in O2. Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n... , where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate of the reaction was determined to be 6.44×10-5 Ms-1 when [NO] = 1.41×10-3 M and [O2] = 2.97×10-3 M. From this experiment, the rate constant is ________ M-2s-1.
1.The oxidation of nitrogen monoxide by oxygen at 25 oC 2 NO + O22 NO2 is second order in NO and first order in O2. Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n... , where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate of the reaction was determined to be 6.44×10-5 Ms-1 when [NO] = 1.41×10-3 M and [O2] = 2.97×10-3 M. From this experiment, the rate constant is ________ M-2s-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 11.50PAE
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1.The oxidation of nitrogen monoxide by oxygen at 25 oC
2 NO + O22 NO2
is second order in NO and first order in O2.
Complete the rate law for this reaction in the box below.
Use the form k[A]m[B]n... , where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear.
Rate = |
In an experiment to determine the rate law, the
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