4. Suppose the formation of iodine proceeds by the following mechanism: Step 1 2 Elementary Reaction Rate Constant H2 (g) + ICI (g) → HI (g) + HCI (g) �1 HI (g) + ICI (g) 12 (g) + HCI (g) ◆2 a. Write the balanced chemical equation for the overall chemical reaction. slow fast b. Write the experimentally- observable rate law for the overall chemical reaction. 5. A certain reaction has the following general form: aA - bB At a particular temperature and [A], -1.60 x 10 M, concentration versus time were collected for this reaction, and a plot of 1/[A] versus time resulted in a straight line with a slope value of 3.40 x 10² L mol² s². What is the final concentration after 317.00 seconds?

4. Suppose the formation of iodine proceeds by the following mechanism: Step 1 2 Elementary Reaction Rate Constant H2 (g) + ICI (g) → HI (g) + HCI (g) �1 HI (g) + ICI (g) 12 (g) + HCI (g) ◆2 a. Write the balanced chemical equation for the overall chemical reaction. slow fast b. Write the experimentally- observable rate law for the overall chemical reaction. 5. A certain reaction has the following general form: aA - bB At a particular temperature and [A], -1.60 x 10 M, concentration versus time were collected for this reaction, and a plot of 1/[A] versus time resulted in a straight line with a slope value of 3.40 x 10² L mol² s². What is the final concentration after 317.00 seconds?

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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