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The following initial rate data are for the gas phase reaction of hydrogen with iodine: H2 + I2 → 2 HI Initial Rate, Experiment [H2]o, M [12lo, M Ms-1 1 2.70x10-2 2.54x10-2 1.33x10-21 2 2.70x10-2 5.09x10-2 2.67x10-21 3 5.40x10-2 2.54x10-2 2.66x10-21 5.40x10-2 5.09x10-2 5.33x10-21 Complete the rate law for this reaction in the box below. Use the form k[A]m[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 = From these data the rate constant is M-1s-1

The following initial rate data are for the gas phase reaction of hydrogen with iodine: H2 + I2 → 2 HI Initial Rate, Experiment [H2]o, M [12lo, M Ms-1 1 2.70x10-2 2.54x10-2 1.33x10-21 2 2.70x10-2 5.09x10-2 2.67x10-21 3 5.40x10-2 2.54x10-2 2.66x10-21 5.40x10-2 5.09x10-2 5.33x10-21 Complete the rate law for this reaction in the box below. Use the form k[A]m[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 = From these data the rate constant is M-1s-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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The following initial rate data are for the gas phase reaction of hydrogen with iodine: H2 + I2 - 2 HI Initial Rate, Experiment [H2]o, M [12]o, M Ms-1 1 2.70x10-2 2.54x10-2 1.33x10-21 2 2.70x10-2 5.09x10-2 2.67x10-21 5.40x10-2 2.54x10-2 2.66x10-21 5.40x10-2 5.09x10-2 5.33x10-21 Complete the rate law for this reaction in the box below. Use the form k[A]m[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 = From these data, the rate constant is M-1s-1.
Transcribed Image Text:The following initial rate data are for the gas phase reaction of hydrogen with iodine: H2 + I2 - 2 HI Initial Rate, Experiment [H2]o, M [12]o, M Ms-1 1 2.70x10-2 2.54x10-2 1.33x10-21 2 2.70x10-2 5.09x10-2 2.67x10-21 5.40x10-2 2.54x10-2 2.66x10-21 5.40x10-2 5.09x10-2 5.33x10-21 Complete the rate law for this reaction in the box below. Use the form k[A]m[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 = From these data, the rate constant is M-1s-1.
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