3 Kinetic Study: The lodine Clock Reaction Prelaboratory Questions Name Laboratory Section 1. Consider the following reaction: 2 N,O5 (g) 4 NO2 (g) + O2 (g) -> The initial concentration of N,O5 was 0.84 mol/L, and 35 minutes after initiating the reaction, all of the N,Os has been consumed. a) Calculate the average rate of the reaction over this 35-minute time interval. b) Is it correct to assume that the rate law is Rate = k[N,O5]² based on the balanced chemical equation? Briefly explain your answer. c) Suppose the reaction rate is determined by simultaneously measuring the rate of decrease of N,Os concentration (-ALN,O5]/At) and the rate of increase of NO, concentration (A[NO,]/At). Which rate will be higher and by what factor? (continued on next page) 137

3 Kinetic Study: The lodine Clock Reaction Prelaboratory Questions Name Laboratory Section 1. Consider the following reaction: 2 N,O5 (g) 4 NO2 (g) + O2 (g) -> The initial concentration of N,O5 was 0.84 mol/L, and 35 minutes after initiating the reaction, all of the N,Os has been consumed. a) Calculate the average rate of the reaction over this 35-minute time interval. b) Is it correct to assume that the rate law is Rate = k[N,O5]² based on the balanced chemical equation? Briefly explain your answer. c) Suppose the reaction rate is determined by simultaneously measuring the rate of decrease of N,Os concentration (-ALN,O5]/At) and the rate of increase of NO, concentration (A[NO,]/At). Which rate will be higher and by what factor? (continued on next page) 137

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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