(a) Determine whether this hydrogen peroxide reaction is first-order or second-order by first calculating the necessary concentration variable for each point (below). In [H₂O₂] 1/[H₂O₂] L/mol Time (min) [H₂O₂] mol/L 0.0200 0.0160 0.0131 0.0106 0.0086 0.0069 0.0056 0.0037 0.0024 0 200 400 600 800 1000 1200 1600 2000 (b) Plot In [H₂O2] vs. time. Attach the graph. (c) Plot 1/[H₂O₂] vs. time. Attach the graph. (d) Write the rate law for this reaction. Explain how you know the order (exponent) for [H₂O₂] in this reaction.
(a) Determine whether this hydrogen peroxide reaction is first-order or second-order by first calculating the necessary concentration variable for each point (below). In [H₂O₂] 1/[H₂O₂] L/mol Time (min) [H₂O₂] mol/L 0.0200 0.0160 0.0131 0.0106 0.0086 0.0069 0.0056 0.0037 0.0024 0 200 400 600 800 1000 1200 1600 2000 (b) Plot In [H₂O2] vs. time. Attach the graph. (c) Plot 1/[H₂O₂] vs. time. Attach the graph. (d) Write the rate law for this reaction. Explain how you know the order (exponent) for [H₂O₂] in this reaction.
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
Chapter12: Chemical Kinetics
Section: Chapter Questions
Problem 110CP: Consider a reaction of the type aA products, in which the rate law is found to he rate = k[A]3...
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