The second-order rate constants for the reaction of oxygen atoms with aromatic hydrocarbons have been measured (R. Atkinson and J.N. Pitts, J. Phys. Chem. 79, 293 (1973)). Rate constants for the reaction of benzene with oxygen atoms at three temperatures are given below: T/K k/(L³ mol-¹) 300.3 1.44 x 107 341.2 3.03 x 107 392.2 6.9 x 107 Determine the activation energy and pre-exponential factor for the reaction from these data.

The second-order rate constants for the reaction of oxygen atoms with aromatic hydrocarbons have been measured (R. Atkinson and J.N. Pitts, J. Phys. Chem. 79, 293 (1973)). Rate constants for the reaction of benzene with oxygen atoms at three temperatures are given below: T/K k/(L³ mol-¹) 300.3 1.44 x 107 341.2 3.03 x 107 392.2 6.9 x 107 Determine the activation energy and pre-exponential factor for the reaction from these data.

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 11.24PAE: Second-order rate constants used in modeling atmospheric chemistry are commonly reported in units of...

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List at least four experimentally determined parameters that you, an experimenter, can define when exploring the hydrolysis of ethyl benzoate by aqueous sodium hydroxide.
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For the past 10 years, the unsaturated hydrocarbon 1, 3-butadiene (CH2 = CH - CH = CH2) has ranked 38th among the top 50 industrial Chemicals. It is used primarily for the manufacture of synthetic rubber. An isomer exists also as cyclobutene: The isomerization of cyclobutene to butadiene is first-order and the rate constant has been measured as 2.0104s1 at 150 C in a 0.53-L ?ask. Determine the partial pressure of cyclobutene and its concentration after 30.0 minutes if an isomerization reaction is carried out at 150 C with an initial pressure of 55 torr.
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Label the elementary processes for the reaction between H2 and O2 see section 20.7 as initiation, propagation, branching, or termination reactions.
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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?
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Second-order rate constants used in modeling atmospheric chemistry are commonly reported in units of cm3 molecule-1s-1. Convert the following rate constants to L mol-1s-1: 3.51014 cm3 molecule-1 s-1 7.11018 cm3 molecule-1 s-1 6.11030 cm3 molecule-1s-1