The reaction rate for the decomposition of N,O5 to form NO2 and O2 was studied as a function of temperature. The first order reaction rate constants were found to be: T (K) k(s*) 273 7.9 x 107 298 3.5 x 105 308 1.4 x 104 318 5.0 x 104 328 1.5 x 10 3 338 4.9 x 103 What is the E, for this reaction in kJ/mol? Use Excel to plot the pertinent data and use linear regression to calculate the slope of the line connecting your data.

The reaction rate for the decomposition of N,O5 to form NO2 and O2 was studied as a function of temperature. The first order reaction rate constants were found to be: T (K) k(s*) 273 7.9 x 107 298 3.5 x 105 308 1.4 x 104 318 5.0 x 104 328 1.5 x 10 3 338 4.9 x 103 What is the E, for this reaction in kJ/mol? Use Excel to plot the pertinent data and use linear regression to calculate the slope of the line connecting your data.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 8RQ

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For a reaction involving the decomposition of a hypothetical substance Y, these data are obtained: Determine the order of the reaction. Write the rate law for the decomposition of Y. Calculate k for the experiment above.
The following rate constants were obtained in an experiment in which the decomposition of gaseous N2O; was studied as a function of temperature. The products were NO, and NO,. Temperature (K) 3.5 x 10_i 298 2.2 x 10"4 308 6.8 X IO-4 318 3.1 x 10 1 328 Determine Etfor this reaction in kj/mol.
The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in automobile engines. Suppose that a series of experiments measured the rate of this reaction at 500 K and produced the following data; [NO] (mol L ’) [OJ (mol L 1) Rate = -A[NO]/Af (mol L_1 s-1) 0.002 0.005 8.0 X 10"'7 0.002 0.010 1.6 X 10-'6 0.006 0.005 2.4 X IO-'6 Derive a rate law for the reaction and determine the value of the rate constant.
Chlorine dioxide oxidizes iodide ion in aqueous solution to iodine; chlorine dioxide is reduced to chlorite ion. 2ClO2(aq)+2I(aq)2ClO2(aq)+I2(aq) The order of the reaction with respect to ClO2 was determined by starting with a large excess of I, so that its concentration was essentially constant. Then Rate=k[ClO2]m[I]n=k[ClO2]m where k= k[I]n. Determine the order with respect to ClO2 and the rate constant k by plotting the following data assuming first- and then second-order kinetics. [Data from H. Fukutomi and G. Gordon, J. Am. Chem. Soc., 89, 1362 (1967).] Time (s) [ClO2] (mol/L) 0.00 4.77 104 1.00 4.31 104 2.00 3.91 104 3.00 3.53 104 5.00 2.89 104 10.00 1.76 104 30.00 2.4 105 50.00 3.2 106
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At 620. K butadiene dimerizes at a moderate rate. The following data were obtained in an experiment involving this reaction: t(s) [C4H6] (mol/L) 0 0.01000 1000.. 0.00629 2000. 0.00459 3000. 0.00361 a. Determine the order of the reaction in butadiene. b. In how many seconds is the dimerization 1.0% complete? c. In how many seconds is the dimerization 10.0% complete? d. What is the half-life for the reaction if the initial concentration of butadiene is 0.0200 M? e. Use the results from this problem and Exercise 45 to calculate the activation energy for the dimerization of butadiene.
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