In the following table are listed the rate constants for the decomposition of N2O5 at different temperatures:t, °Ck, sec 17.87 x 10-7253.46 x 10-5351.35 x 10-4454.98 x 10-4551.50 x 10 3654.87 x 103Determine the energy of activation and find the rate constant at 50°C.E,kJ/mol/sec"For the rate constant please use the format 1.00 x 10^-1

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Answered: In the following table are listed the…

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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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.
11.35 For the reaction 2 NO(g) + 2 H?(g) — N,(g) + 2 H,O(g) at 1100°C, the following data have been obtained: [NOJ [HJ Rate = A(N2]/At (mol L~1) (mol L_1) (mol L-1 s_1) 5.0 X 10’1 0.32 0.012 1.0 X 10~’ 0.32 0.048 1.0 X 10"2 0.64 0.096 Derive a rate law for the reaction and determine the value of the rate constant.
The thermal decomposition of diacetylene, C4H2, was studied at 950 C. Use the following data (K. C. Hou and H. B. Palmer, Journal of Physical Chemistry. Vol. 60, p. 858, 1965) to determine the order of the reaction.
11.51 Peroxyacetyl nitrate (PAN) has the chemical formula CtHjNOj and is an important lung irritant in photochemical smog. An experiment to determine the decomposition kinetics of PAN gave the data below. Determine the order of reaction and calculate the rate constant for the decomposition of PAN. Time, t (min) Partial Pressure of PAN (torr) 0.0 2.00 X 10~’ 10.0 1.61 X 10~} 20.0 1.30 X 10_J 30.0 1.04 X 10"’ 40.0 8.41 X 10-4 50.0 6.77 x 10-4 60.0 5.45 X 10-4
The following values of the rate constant were obtained for the decomposition of nitrogen dioxide at various temperatures. Plot the natural logarithm of k versus l/T and from the graph obtain the energy of activation. Temperature (oC) k (L/mol s) 320 0.527 330 0.776 340 1.121 350 1.607
Experiments have shown that the average frequency of chirping by a snowy tree cricket (Oecanthus fultoni) depends on temperature as shown in the table. Chirping Rate (per min) Temperature (C) 178 25.0 126 20.3 100. 17.3 What is the apparent activation energy of the process that controls the chirping? What is the rate of chirping expected at a temperature of 7.5C?
The following values of the rate constant were obtained for the decomposition of hydrogen iodide at various temperatures. Plot the natural logarithm of k versus l/T and from the graph obtain the energy of activation. Temperature (oC) k (L/mol s) 440 2.69 103 460 6.21 103 480 1.40 102 500 3.93 102
For the reaction QW+X, the following data were obtained at 30 C: [Q]initial (M) 0.170 0.212 0.357 Rate(mol/L/s) 6.68103 1.04102 2.94102 (a) What is the order of the reaction with respect to [Q], and what is the rate equation? (b) What is the rate constant?
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.
Would the slope of a ln(k) versus 1/T plot (with temperature in kelvin) for a catalyzed reaction be more or less negative than the slope of the ln(k) versus 1/T plot for the uncatalyzed reaction? Explain. Assume both rate laws are first-order overall.
The following data have been determined for the reaction: I+OCIIO+CI 1 2 3 [I] 0.10 0.20 0.30 [OCI] 0.050 0.050 0.010 Rate(mol/L/s) 3.05104 6.20104 1.83104 Determine the rate equation and the rate constant for this reaction.
One mechanism for the destruction of ozone in the upper atmosphere is a. Which species is a catalyst? b. Which species is an intermediate? c. Ea for the uncatalyzed reaction O3(g)+O(g)2O2(g) is 14.0 kJ. Ea. for the same reaction when catalyzed is 11.9 kJ. What is the ratio of the rate constant for the catalyzed reaction to that for the uncatalyzed reaction at 25C? Assume that the frequency factor A is the same for each reaction.

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