b)The results obtained from the decomposition of N;O; at two different temperatureswere recorded as follows:Temperature ("C) Rate constant, k (s)1.74 x 10 *25356.61 x 10 3i What is the order of the reaction?i Determine the value of E, for the reaction.i What would happen to the reaction rate if a catalyst was added?Explain how the catalyst works.

Given that Temperature (oC) Rate constant, k(s-1) 25 1.74x10-5 35 6.61x10-5

b) The results obtained from the decomposition of N;Os at two different temperatures were recorded as follows: Temperature (C) Rate constant, k (s) 25 1.74x 10 35 6.61 x 10 i What is the order of the reaction? i Determine the value of E, for the reaction i What would happen to the reaction rate if a catalyst was added? Explain how the catalyst works.

b) The results obtained from the decomposition of N;Os at two different temperatures were recorded as follows: Temperature (C) Rate constant, k (s) 25 1.74x 10 35 6.61 x 10 i What is the order of the reaction? i Determine the value of E, for the reaction i What would happen to the reaction rate if a catalyst was added? Explain how the catalyst works.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter11: Rate Of Reaction

Section: Chapter Questions

Problem 28QAP: Diethylhydrazine reacts with iodine according to the following equation: Â...

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The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in automobile engines. Suppose that a series of experiments measured the rate of this reaction at 500 K and produced the following data; [NO] (mol L ’) [OJ (mol L 1) Rate = -A[NO]/Af (mol L_1 s-1) 0.002 0.005 8.0 X 10"'7 0.002 0.010 1.6 X 10-'6 0.006 0.005 2.4 X IO-'6 Derive a rate law for the reaction and determine the value of the rate constant.
Diethylhydrazine reacts with iodine according to the following equation: Â (C2H5)2(NH)2(l)+I2(aq)(C2H5)2N2+2HI(aq)The rate of the reaction is followed by monitoring the disappearance of the purple color due to iodine. The following data are obtained at a certain temperature. (a) What is the order of the reaction with respect to diethylhydrazine, iodine, and overall? (b) Write the rate expression of the reaction. (c) Calculate k for the reaction. (d) What must [(C2H5)2] be so that the rate of the reaction is 5.00104mol/Lh when [ I2 ]=0.500M?
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11.44 A possible reaction for the degradation of the pesticide DDT to a less harmful compound was simulated in the laboratory. The reaction was found to be first order, with k = 4.0 X 10_H s"' at 25°C. What is the half-life for the degradation of DDT in this experiment, in years?
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The following rate constants were obtained in an experiment in which the decomposition of gaseous N2O; was studied as a function of temperature. The products were NO, and NO,. Temperature (K) 3.5 x 10_i 298 2.2 x 10"4 308 6.8 X IO-4 318 3.1 x 10 1 328 Determine Etfor this reaction in kj/mol.
Explain what is meant by the average rate of a reaction.
Based on the diagrams in Exercise 12.83, which of the reactions has the fastest rate? Which has the slowest rate?
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Azomethane decomposes into nitrogen and ethane at high temperatures according to the following equation: (CH3)2N2(g)N2(g)+C2H6(g)The rate of the reaction is followed by monitoring the disappearance of the purple color due to iodine. The following data are obtained at a certain temperature. (a) By plotting the data, show that the reaction is first-order. (b) From the graph, determine k. (c) Using k, find the time (in hours) that it takes to decrease the concentration to 0.100 M. (d) Calculate the rate of the reaction when [ (CH3)2N2 ]=0.415M.