3. Consider the elementary or single step reaction, A → B, which we will depict using the following symbols: A The concentration of A and B were monitored as a function of time, t, as seen in the diagram below: t = 2.5 min t = 0.00 min What is the value of the rate constant, k? a. 1.7 min! b. 0.28 s с. 3.6 min-! d. 0.0046 s Cannot tell from the information given e.

3. Consider the elementary or single step reaction, A → B, which we will depict using the following symbols: A The concentration of A and B were monitored as a function of time, t, as seen in the diagram below: t = 2.5 min t = 0.00 min What is the value of the rate constant, k? a. 1.7 min! b. 0.28 s с. 3.6 min-! d. 0.0046 s Cannot tell from the information given e.

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 11.48PAE: 11.48 The following data were collected for the decomposition of NT),-: Time, f (min) [N2Os] (mol...

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11.48 The following data were collected for the decomposition of NT),-: Time, f (min) [N2Os] (mol L-1) 0 0.200 5 0.171 10 0.146 15 0.125 20 0.106 25 0.0909 30 0.0777 35 0.0664 40 0.0570 Use appropriate graphs to determine the rate constant for this reaction. Find the half-life of the reaction.
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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