6. Reconsider the plot shown in Prelab Question 1. This plot shows a first order decay with an initial concentration of 0.010 M. Reaction Rate 0.0100 0.000 0.0060 0.0040 0.020 -0.000 10 20 50 Time (s) a. Estimate the rate constant. b. Use your rate constant and equation 6 to estimate the half-life from the rate constant. c. Estimated the half-life directly from the plot. Are your two estimates of the half-life consistent? Explain why or why not. Concentration (M)

6. Reconsider the plot shown in Prelab Question 1. This plot shows a first order decay with an initial concentration of 0.010 M. Reaction Rate 0.0100 0.000 0.0060 0.0040 0.020 -0.000 10 20 50 Time (s) a. Estimate the rate constant. b. Use your rate constant and equation 6 to estimate the half-life from the rate constant. c. Estimated the half-life directly from the plot. Are your two estimates of the half-life consistent? Explain why or why not. Concentration (M)

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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Consider a reaction of the type aA products, in which the rate law is found to he rate = k[A]3 (termolecular reactions are improbable but possible). If the first half-tife of the reaction is found to he 40. s, what is the time for the second half-life? Hint: Using your calculus knowledge, derive the integrated rate law from the differential rate law for a tennolecular reaction: Rate=d[A]dt=k[A]3
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What is the rate equation for the elementary termolecular reaction A+2B products? For 3A products?
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Consider the following hypothetical data collected in two studies of the reaction 2A+2BC+2D Time(s) Experiment 1 [A] (mol/L) Experiment 2 [A] (mol/L) 0 1.0 102 1.0 102 10. 8.4 103 5.0 103 20. 7.1 103 2.5 103 30. ? 1.3 103 40. 5.0 103 6.3 104 In Experiment 1, [B]0 = 10.0 M. In Experiment 2, [B]0 = 20.0 M. Rate=[A]t a. Use the concentration versus time data to determine the rate law for the reaction. b. Solve for the value of the rate constant (k) for the reaction. Include units. c. Calculate the concentration of A in Experiment 1 at t =30.s
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