4 SIMULATION Determining the Rate Law I[A] vs TimeIn[A] vs Time1/[A] vs TimeO Least SquaresPlotTime, sThe reactionA - Cwas performed and the concentration vs. time data below collected.time, s1234578[A], mol/L 0.7481 0.1625 0.09116 0.06334 0.048540.039340.03307 0.02853 0.02508Complete the rate law for the reaction by filling in the values for the rate constant and reaction order.Rate = k[A]Xrate constant (without units) =reaction order =[v]uI

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The reaction A - C was performed and the concentration vs. time data below collected. time, s 1 2 3 5 6 7 [A], mol/L 0.7481 0.1625 0.09116 0.06334 0.04854 0.03934 0.03307 0.02853 0.02508 Complete the rate law for the reaction by filling in the values for the rate constant and reaction order. Rate = k[A]* rate constant (without units) = reaction order =

The reaction A - C was performed and the concentration vs. time data below collected. time, s 1 2 3 5 6 7 [A], mol/L 0.7481 0.1625 0.09116 0.06334 0.04854 0.03934 0.03307 0.02853 0.02508 Complete the rate law for the reaction by filling in the values for the rate constant and reaction order. Rate = k[A]* rate constant (without units) = reaction order =

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 110CP: Consider the following hypothetical data collected in two studies of the reaction 2A+2BC+2D Time(s)...

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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
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?
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What is the difference between average rate, initial rate, and instantaneous rate?
For a certain reaction, Ea is 135 kJ and H=45 kJ. In the presence of a catalyst, the activation energy is 39% of that for the uncatalyzed reaction. Draw a diagram similar to Figure 11.14 but instead of showing two activated complexes (two humps) show only one activated complex (i.e., only one hump) for the reaction. What is the activation energy of the uncatalyzed reverse reaction?
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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?
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