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ded for this question. The following initial rate data are for the reaction of nitrogen monoxide with ozone at 25 °C: NOO3 NO2+ O2 Experiment [NO], M [03]0, M Initial Rate, M.S-1 1 0.164 0.0409 0.636 2 0.164 0.0818 1.27 3 0.329 0.0409 1.28 4 0.329 0.0818 2.55 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 = M-1 8-1

ded for this question. The following initial rate data are for the reaction of nitrogen monoxide with ozone at 25 °C: NOO3 NO2+ O2 Experiment [NO], M [03]0, M Initial Rate, M.S-1 1 0.164 0.0409 0.636 2 0.164 0.0818 1.27 3 0.329 0.0409 1.28 4 0.329 0.0818 2.55 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 = M-1 8-1

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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ded for this question. The following initial rate data are for the reaction of nitrogen monoxide with ozone at 25 °C: NOO3 NO2+ O2 Experiment [NO], M [03]0, M Initial Rate, M.S-1 1 0.164 0.0409 0.636 2 0.164 0.0818 1.27 3 0.329 0.0409 1.28 4 0.329 0.0818 2.55 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 = M-1 8-1
Transcribed Image Text:ded for this question. The following initial rate data are for the reaction of nitrogen monoxide with ozone at 25 °C: NOO3 NO2+ O2 Experiment [NO], M [03]0, M Initial Rate, M.S-1 1 0.164 0.0409 0.636 2 0.164 0.0818 1.27 3 0.329 0.0409 1.28 4 0.329 0.0818 2.55 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 = M-1 8-1
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