Consider the following reaction: C6H11F + KBr →C6H11B1 + KFThe following concentration vs. time data were collected.[CH11E].time. min0.400 M0.380 M3.000.350 M7.700.320 M12.870.300 M16.320.270 M22.640.250 M27.24A. Graph the data to determine the order.B. What is the order with respect to [C6H11F]?C. Calculate the rate constant, k.D. Write the rate law (equation).E. Calculate the half-life.F. How many minutes will it take to reach a concentration of 0.280 M?Upload the graphs with correlation coefficients and trendline equations and calculations.

In order to determine the order of a reaction graphically, we have to plot 3 different graphs which…

Consider the following reaction: C,H11F + KBr → C6H11B1 + KF The following concentration vs. time data were collected. time. min 0.400 M 0.380 M 3.00 0.350 M 7.70 0.320 M 12.87 0.300 M 16.32 0.270 M 22.64 0.250 M 27.24 A. Graph the data to determine the order. B. What is the order with respect to [C,H11F]? C. Calculate the rate constant, k. D. Write the rate law (equation). E. Calculate the half-life. F. How many minutes will it take to reach a concentration of 0.280 M? Upload the graphs with correlation coefficients and trendline equations and calculatic

Consider the following reaction: C,H11F + KBr → C6H11B1 + KF The following concentration vs. time data were collected. time. min 0.400 M 0.380 M 3.00 0.350 M 7.70 0.320 M 12.87 0.300 M 16.32 0.270 M 22.64 0.250 M 27.24 A. Graph the data to determine the order. B. What is the order with respect to [C,H11F]? C. Calculate the rate constant, k. D. Write the rate law (equation). E. Calculate the half-life. F. How many minutes will it take to reach a concentration of 0.280 M? Upload the graphs with correlation coefficients and trendline equations and calculatic

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 33E: The reaction I(aq)+OCl(aq)IO(aq)+Cl(aq) was studied, and the following data were obtained:...

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The thermal decomposition of diacetylene, C4H2, was studied at 950 C. Use the following data (K. C. Hou and H. B. Palmer, Journal of Physical Chemistry. Vol. 60, p. 858, 1965) to determine the order 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
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 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.
Sulfuryl chloride (SO2Cl2) decomposes to sulfur dioxide (SO2) and chlorine (Cl2) by reaction in the gas phase. The following pressure data were obtained when a sample containing 5.00 102 mol sulfuryl chloride was heated to 600. K in a 5.00 101-L container. Time (hours): 0.00 1.00 2.00 4.00 8.00 16.00 PSO2Cl2(atm): 4.93 4.26 3.52 2.53 1.30 0.34 Defining the rate as [SO2Cl2]t, a. determine the value of the rate constant for the decomposition of sulfuryl chloride at 600. K. b. what is the half-life of the reaction? c. what fraction of the sulfuryl chloride remains after 20.0 h?
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?
Compare the functions of homogeneous and heterogeneous catalysts.
A study of the rate of the reaction represented as 2AB gave the following data: Time (s) 0.0 5.0 10.0 15.0 20.0 25.0 35.0 [A](M) 1.00 0.775 0.625 0.465 0.350 0.205 0.230 (a) Determine the average rate of disappearance of A between 0.0 s and 10.0 s, and between 10.0 s and 20.0 s. (b) Estimate the instantaneous rate of disappearance of A at 15.0 s from a graph of time versus [A]. What are theunits of this rate? (c) Use the rates found in parts (a) and (b) to determine the average rate of formation of B between 0.00 s and 10.0 s, and the instantaneous rate of formation of B at 15.0 s.
The reaction I(aq)+OCl(aq)IO(aq)+Cl(aq) was studied, and the following data were obtained: [I]0(mol/L) [OCl]0(mol/L) Initial Rate (mol/L s) 0.12 0.18 7.91 102 0.060 0.18 3.95 102 0.030 0.090 9.88 103 0.24 0.090 7.91 102 a. What is the rate law? b. Calculate the value of the rate constant. c. Calculate the initial rate for an experiment where both Iand OCl are initially present at 0.15 mol/L.
Phenyl acetate, an ester, reacts with water according to the equation The data in the table were collected for this reaction at 5 C. (a) Plot the phenyl acetate concentration versus time, and describe the shape of the curve observed. (b) 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?
The following data were collected in two studies of the reaction 2A+BC+D Time (s) Experiment 1 [A] (mol/L) 102 Experiment 2 [A] (mol/L) 102 0 10.0 10.0 20. 6.67 5.00 40. 5.00 3.33 60. 4.00 2.50 80. 3.33 2.00 100. 2.86 1.67 120. 2.50 1.43 In Experiment 1, [B]0 = 5.0 M. In Experiment 2, [B]0 = 10.0 M. Rate=[A]t a. Why is [B] much greater than [A]? b. Give the rate law and value for k for this reaction.
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