Question 9Take QuizButadiene (C4H6) is consumed in a reaction by a 2nd order process. The initialconcentration of C4H6 is 68.58 M. After 2.07 seconds, the concentration of C4H6 is0.216 M. What is the rate constant for this reaction. Enter your answer as a number with3 sig figs. Assume that the units are M-¹s ¹.Question 10A second order reaction with the equation A--> B has a half life of 59.26 seconds with aninitial concentration of {A} = 0.432 M. If you started with an initial concentration of {A} =0.792 M, how many seconds would it take for the concentration to get to 0.271 M?Exit

Question 9 Take Quiz Butadiene (C4H6) is consumed in a reaction by a 2nd order process. The initial concentration of C4H6 is 68.58 M. After 2.07 seconds, the concentration of C4H6 is 0.216 M. What is the rate constant for this reaction. Enter your answer as a number with 3 sig figs. Assume that the units are M-¹5-¹. Question 10 A second order reaction with the equation A--> B has a half life of 59.26 seconds with an initial concentration of {A} = 0.432 M. If you started with an initial concentration of {A} = 0.792 M, how many seconds would it take for the concentration to get to 0.271 M? Exit

Question 9 Take Quiz Butadiene (C4H6) is consumed in a reaction by a 2nd order process. The initial concentration of C4H6 is 68.58 M. After 2.07 seconds, the concentration of C4H6 is 0.216 M. What is the rate constant for this reaction. Enter your answer as a number with 3 sig figs. Assume that the units are M-¹5-¹. Question 10 A second order reaction with the equation A--> B has a half life of 59.26 seconds with an initial concentration of {A} = 0.432 M. If you started with an initial concentration of {A} = 0.792 M, how many seconds would it take for the concentration to get to 0.271 M? Exit

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 11.40PAE: In Exercise 11.39, if the initial concentration of N2Oj is 0.100 .\1. how long will it take for the...

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Experimental data are listed here for the reaction A 2 B. (a) Prepare a graph from these data; connect the points with a smooth line; and calculate the rate of change of [B] for each 10-second interval from 0.0 to 40.0 seconds. Does the rate of change decrease from one time interval to the next? Suggest a reason for this result. (b) How is the rate of change of [A] related to the rate of change of [B] in each time interval? Calculate the rate of change of [A] for the time interval from 10.0 to 20.0 seconds.
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?
Ammonium cyanate, NH4NCO, rearranges in water to give urea, (NH2)2CO. NH4NCO(aq) (NH2)2CO(aq) Using the data in the table: (a) Decide whether the reaction is first-order or second-order. (b) Calculate k for this reaction. (c) Calculate the half-life of ammonium cyanate under these conditions. (d) Calculate the concentration of NH4NCO after 12.0 hours.
Use the data provided in a graphical method to determine the order and rate constant of the following reaction: 2PQ+W Time (s) 9.0 13.0 18.0 22.0 25.0 [P] (M) 1.077103 1.068103 1.055103 1.046103 1.039103
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When heated, tetrafluoroethylene dimerizes to form octafluorocyclobutane. C2F4(g) C4F8(g) To determine the rate of this reaction at 488 K, the data in the table were collected. Analysis was done graphically, as shown below: (a) What is the rate law for this reaction? (b) What is the value of the rate constant? (c) What is the concentration of C2F4 after 600 s? (d) How long will it take until the reaction is 90% complete?
In Exercise 11.39, if the initial concentration of N2Oj is 0.100 .\1. how long will it take for the concentration to drop to 0.0100 times its original value? The decomposition of N2O5 in solution in carbon tetrachloride is a first-order reaction: 2N2O5—»4NO2 + O2 The rate constant at a given temperature is found to be 5.25 X 10-4 s-’. If the initial concentration of N2O5 is 0.200 M, what is its concentration after exactly 10 minutes have passed?
A certain reaction has the form aAProducts At a particular temperature, concentration versus time data were collected. A plot of 1/ [A] versus Lime (in seconds) gave a straight line with a slope of 6.90 102. What is the differential rate law for this reaction? What is the integrated rate law for this reaction? What is the value of the rate constant for this reaction? If [A]0 for this reaction is 0.100 M, what is the first half-life (in seconds)? If the original concentration (at t = 0) is 0.100 M, what is the second half-life (in seconds)?
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From the given data, use a graphical method to determine the order and rate constant of the following reaction: 2XY+Z Time (s) 5.0 10.0 15.0 20.0 25.0 30.0 35.0 40.0 [X](M) 0.0990 0.0497 0.0332 0.0249 0.0200 0.0166 0.0143 0.0125
The rate of the reaction NO2(g)+CO(g)NO(g)+CO2(g) depends only on the concentration of nitrogen dioxide below 225C. At a temperature below 225C, the following data were collected: Time(s) [NO2](mol/L) 0 0.500 1.20 103 0.444 3.00 103 0.381 4.50 103 0.340 9.00 103 0.250 1.80 104 0.174 Determine the rate law, the integrated rate law, and the value of the rate constant. Calculate [NO2] at 2.70 104 s after the start of the reaction.
Say you run the following elementary, termolecular reaction: 2A+BD Using the starting concentrations [A] = 2.0 M and [B] = 2.0 M, you measure the rate to be 16 M2 S1 .What is the value of the rate constant?