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

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Consider the following reaction: 2H₂O₂(aq)→ 2H₂O(1) + O₂(g) Concentration (M) 1.2 1.0 0.8- 0.6- 0.4- 0.2- 0 0 10 Show Transcribed Text 20 [H₂O₂] 30 c 40 50 Time (s) 60 70 80 The graph shows the concentration of H₂O₂ as a function of time. Use the graph to calculate the following. a.) Calculate the average rate of the reaction between 10 and 20 s. b.) Calculate the instantaneous rate of the reaction at 30 s. c.) Calculate the instantaneous rate of formation of O₂ at 50 s. d.) If the initial volume of the H₂O₂ solution is 1.5 L, what total amount of O₂ (in moles) is formed in the first 50 s of reaction?
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