29. An integrative rate law experiment shows that the plot of In [NO2] vs. time is a straight line (in Fig. 2) for the reaction:6NO2 (g) → 3 O2 (g) + 6NO (g)0.8Time (min)crall retion[NO2] (M)2.00000.0000the given halftionNose0.65.00001.587410.0001.25990.415.0001.0000In [NO,]20.0000.793700.2Part 1. The reaction isorder.a) zero-th b) first c) secondd) third e) none of the above-0.20.5.101520Part 2.The rate constant with correct units of the above reaction istime (min)Fig. 2a) 0.0667 M-' minb) 0.0462 min-!c) 0.0826 M min!d) 1.960 mine) none of the above

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29. An integrative rate law experiment shows that the plot of In [NO2] vs. time is a straight line (in Fig. 2) for the reaction: 6NO2 (g) → 3 O2 (g) + 6NO (g) 08 Time (min) [NO:] (M) 2.0000 0.0000 with the ivenlf 0.6 5.0000 10.000 15.000 1.5874 1.2599 0.4 1.0000 In [NO,] 20.000 0.79370 0.2 Part 1. The reaction is order. a) zero-th b) first c) second d) third e) none of the above -0.2 10 15 20 Part 2.The rate constant with correct units of the above reaction is time (min) Fig. 2 a) 0.0667 M' min! b) 0.0462 min c) 0.0826 M min d) 1.960 min e) none of the above

29. An integrative rate law experiment shows that the plot of In [NO2] vs. time is a straight line (in Fig. 2) for the reaction: 6NO2 (g) → 3 O2 (g) + 6NO (g) 08 Time (min) [NO:] (M) 2.0000 0.0000 with the ivenlf 0.6 5.0000 10.000 15.000 1.5874 1.2599 0.4 1.0000 In [NO,] 20.000 0.79370 0.2 Part 1. The reaction is order. a) zero-th b) first c) second d) third e) none of the above -0.2 10 15 20 Part 2.The rate constant with correct units of the above reaction is time (min) Fig. 2 a) 0.0667 M' min! b) 0.0462 min c) 0.0826 M min d) 1.960 min e) none of the above

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.28PAE

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Similar questions

11.35 For the reaction 2 NO(g) + 2 H?(g) — N,(g) + 2 H,O(g) at 1100°C, the following data have been obtained: [NOJ [HJ Rate = A(N2]/At (mol L~1) (mol L_1) (mol L-1 s_1) 5.0 X 10’1 0.32 0.012 1.0 X 10~’ 0.32 0.048 1.0 X 10"2 0.64 0.096 Derive a rate law for the reaction and determine the value of the rate constant.
Nitrogen monoxide reacts with chlorine to form nitrosyl chloride. NO(g)+12Cl2(g)NOCl(g) The figure shows the increase in nitrosyl chloride concentration under appropriate experimental conditions. The concentration of nitrosyl chloride actually starts at zero, although this fact may be difficult to see in the figure. (a) Write an expression for the rate of reaction in terms of a changing concentration. (b) Calculate the average rate of reaction between 40 and 120 seconds. (c) Calculate the instantaneous rate of reaction after 80 seconds. (d) Calculate the instantaneous rate of consumption of chlorine 60 seconds after the start of the reaction.
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
Nitrogen monoxide reacts with chlorine according to the equation: 2NOCI(g)2NOCI(g) The following initial rates of reaction have been observed for certain reactant concentrations: [NO] (moI/L1) [CI2] (mol/L) Rate (moI/L/h) 0.50 0.50 1.14 1.00 0.50 4.56 1.00 1.00 9.12 What is the rate equation that describes the rate’s dependence on the concentrations of NO and CI2? What is the rate constant? What are the orders with respect to each reactant?
Experimental data are listed here for the reaction B: Time (s) IB] (mol/L) 0.00 0.000 10.0 0.326 20.0 0.572 30.0 0.750 40.0 0.890 Prepare a graph from these data, connect the points with a smooth line, and calculate the rate of change of [B] for each 10-s interval from 0.0 to 40.0 s. Does the rate of change decrease from one time interval to the next? Suggest a reason for this result. How is the rate of change of [AJ related to the rate of change of [B] in each time interval? Calculate the rate of change of [AJ for the time interval from 10.0 to 20.0 s. What is the instantaneous rate, A[B]/Ar, when [BI = 0.750 mol/L?
6. Phenyl acetate, an ester, reacts with water according to the equation The data in the table were collected for this reaction at 5°C. Time (s) [Phenyl acetate] (mol/L) 0 0.55 15.0 0.42 30.0 0.31 45.0 0.23 60.0 0.17 75.0 0.12 90.0 0.085 Plot the phenyl acetate concentration versus time, and describe the shape of the curve observed. Calculate the rate of change of the phenyl acetate concentration during the period 15.0 seconds to 30.0 seconds and also during the period 75.0 seconds to 90.0 seconds. Why is one value smaller than the other? What is the rate of change of the phenyl acetate concentration during the time period 60.0 seconds to 75.0 seconds? What is the instantaneous rate at 15.0 seconds?
Based on the diagrams in Exercise 12.83, which of the reactions has the fastest rate? Which has the slowest rate?
The decomposition of sulfuryl chloride, SO2Cl2, to sulfur dioxide and chlorine gases is a first-order reaction. SO2Cl2(g)SO2(g)+Cl2(g)At a certain temperature, the half-life of SO2Cl2 is 7.5102 min. Consider a sealed flask with 122.0 g of SO2Cl2. (a) How long will it take to reduce the amount of SO2Cl2 in the sealed flask to 45.0 g? (b) If the decomposition is stopped after 29.0 h, what volume of Cl2 at 27C and 1.00 atm is produced?
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?
Each of the statements given below is false. Explain why. a. The activation energy of a reaction depends on the overall energy change (E) for the reaction. b. The rate law for a reaction can be deduced from examination of the overall balanced equation for the reaction. c. Most reactions occur by one-step mechanisms.
Consider a hypothetical reaction between A and B: A + B products Use the following initial rate data to calculate the rate constant for this reaction. [A] (mol/L) [B] (mol/L) Initial Rate (mol/L s) 0.20 1.0 3.0 0.50 1.0 11.8 2.0 2.0 189.5
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.