Now that the order for both reactants is known, the rate constant, k, can be determined. Each of the four trials can be used to calculate k and then the four results can be averaged. We will use Trial 4 to determine the rate constant in this example. What is the value of the rate constant? [A], mol/L [B], mol/L rate, mol/(L-min) Trial 1 0.424 0.801 0.126 Trial 2 0.848 0.801 0.253 Trial 3 0.424 1.60 0.506 Trial 4 0.249 0.244 0.00689 Rate = k[A]'[B]2

Now that the order for both reactants is known, the rate constant, k, can be determined. Each of the four trials can be used to calculate k and then the four results can be averaged. We will use Trial 4 to determine the rate constant in this example. What is the value of the rate constant? [A], mol/L [B], mol/L rate, mol/(L-min) Trial 1 0.424 0.801 0.126 Trial 2 0.848 0.801 0.253 Trial 3 0.424 1.60 0.506 Trial 4 0.249 0.244 0.00689 Rate = k[A]'[B]2

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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