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

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Chapter13: Rates Of Reaction
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Problem 13.123QP: The reaction of thioacelamidc with water is shown by the equation below:...
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1c

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
Transcribed Image Text: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
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