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Prelaboratory Questions Name Laboratory Section 8. 1. Consider the following reaction: 2 N2O5 (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,O5 has been consumed. a) Calculate the average rate of the reaction over this 35-minute time interval. k[N2O5]? based on the balanced b) Is it correct to assume that the rate law is Rate chemical equation? Briefly explain your answer. %3D c) Suppose the reaction rate is determined by simultaneously measuring the rate of decrease of NoOs concentration (-A[N2O5]/At) and the rate of increase of NO, concentration (A[NO,J/At). Which rate will be higher and by what factor? (continued on next page) 137

Prelaboratory Questions Name Laboratory Section 8. 1. Consider the following reaction: 2 N2O5 (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,O5 has been consumed. a) Calculate the average rate of the reaction over this 35-minute time interval. k[N2O5]? based on the balanced b) Is it correct to assume that the rate law is Rate chemical equation? Briefly explain your answer. %3D c) Suppose the reaction rate is determined by simultaneously measuring the rate of decrease of NoOs concentration (-A[N2O5]/At) and the rate of increase of NO, concentration (A[NO,J/At). Which rate will be higher and by what factor? (continued on next page) 137

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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Prelaboratory Questions Name Laboratory Section 8. 1. Consider the following reaction: 2 N2O5 (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,O5 has been consumed. a) Calculate the average rate of the reaction over this 35-minute time interval. k[N2O5]? based on the balanced b) Is it correct to assume that the rate law is Rate chemical equation? Briefly explain your answer. %3D c) Suppose the reaction rate is determined by simultaneously measuring the rate of decrease of NoOs concentration (-A[N2O5]/At) and the rate of increase of NO, concentration (A[NO,J/At). Which rate will be higher and by what factor? (continued on next page) 137
Transcribed Image Text:Prelaboratory Questions Name Laboratory Section 8. 1. Consider the following reaction: 2 N2O5 (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,O5 has been consumed. a) Calculate the average rate of the reaction over this 35-minute time interval. k[N2O5]? based on the balanced b) Is it correct to assume that the rate law is Rate chemical equation? Briefly explain your answer. %3D c) Suppose the reaction rate is determined by simultaneously measuring the rate of decrease of NoOs concentration (-A[N2O5]/At) and the rate of increase of NO, concentration (A[NO,J/At). Which rate will be higher and by what factor? (continued on next page) 137
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