Answered: 5. Rate constant of a reaction changes…

5. Rate constant of a reaction changes from 0.0125 s¹ to 0.320 s¹ when temperature changes from 411 K to 435K. Calculate energy of activation in kj/mol.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 108CWP: Consider the hypothetical reaction A2(g) + B2(g) 2AB(g), where the rate law is: [A2]t=k[A2][B2] The...

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5. Rate constant of a reaction changes from 0.0125 s¹ to 0.320 s¹ when temperature
changes from 411 K to 435K. Calculate energy of activation in kj/mol.

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For the reaction 2N2O(g)2N2(g)+O2(g) the rate constant is 0.066 L/mol min at 565C and 22.8 L/mol min at 728C. (a) What is the activation energy of the reaction? (b) What is k at 485C? (c) At what temperature is k, the rate constant, equal to 11.6 L/mol min?
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Consider a hypothetical reaction between A and B: A + B products Use the following initial rate data to calculate the rate constant for this reaction. [A] (mol/L) [B] (mol/L) Initial Rate (mol/L s) 0.20 1.0 3.0 0.50 1.0 11.8 2.0 2.0 189.5
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.
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