The reaction A - C was performed and the concentration vs. time data below collected. time, s 1 2 4 5 6 7 8 [A], mol/L 0.9540 0.5864 0.3605 0.2216 0.1362 0.08371 0.05145 0.03163 0.01944 Comp te the rate law for the reaction by ng 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 4 5 6 7 8 [A], mol/L 0.9540 0.5864 0.3605 0.2216 0.1362 0.08371 0.05145 0.03163 0.01944 Comp te the rate law for the reaction by ng in the values for the rate constant and reaction order. Rate = k[A]* rate constant (without units) = reaction order =

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter18: Chemical Kinetics

Section: Chapter Questions

Problem 53AP

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The color change accompanying the reaction of phenolphthalein with strong base is illustrated below. The change in concentration of the dye can be followed by spectrophotometry (Section 4.9), and some data collected by that approach are given below. The initial concentrations were [phenolphthalein] = 0.0050 mol/L and [OH] = 0.61 mol/L. (Data are taken from review materials for kinetics at chemed.chem.purdue.edu.) (For more details on this reaction see L Nicholson, Journal of Chemical Education, Vol. 66, p. 725, 1989.) (a) Plot the data above as [phenolphthalein] versus time, and determine the average rate from t = 0 to t = 15 seconds and from t = 100 seconds to t = 125 seconds. Does the rate change? If so, why? (b) Use a graphical method to determine the order of the reaction with respect to phenolphthalein. Write the rate law, and determine the rate constant. (c) What is the half-life for the reaction?
Instantaneous rates for the reaction of hydroxide ion with Cv+ can be determined from the slope of the curve in Figure 11.3 at various concentrations. They are (1) At 4.0 105 mol/L, rate = 12.3 107 mol L1 s1 (2) At 3.0 105 mol/L, rate = 9.25 107 mol L1 s1 (3) At 2.0 105 mol/L, rate = 6.16 107 mol L1 s1 (4) At 1.5 105 mol/L, rate = 4.60 107 mol L1 s1 (5) At 1.0 105 mol/L, rate = 3.09 107 mol L1 s1 (a) What is the relationship between the rates in (1) and (3)? Between (2) and (4)? Between (3) and (5)? (b) What is the relationship between the concentrations in each of these cases? (c) Is the rate of the reaction proportional to the concentration of Cv+? Explain your answer.
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A first order reaction takes 69.3 min for 50% completion. Set up on equationfor determining the time needed for 80% completion.