The activation energy for the reaction 2 NO2(g) → 2 NO(g) + O2(g) is 111 kJ mol- 1. What proportion of the collisions between NO2 molecules have enough energy toresult in reaction when the temperature is (a)20 oC. (b)200 °C? Use collision theory to estimate the pre-exponential factor for the reaction. The experimental value is 2 x 109 dm3 mol-1 s-1. Suggest a reason for any discrepancy.
The activation energy for the reaction 2 NO2(g) → 2 NO(g) + O2(g) is 111 kJ mol- 1. What proportion of the collisions between NO2 molecules have enough energy toresult in reaction when the temperature is (a)20 oC. (b)200 °C? Use collision theory to estimate the pre-exponential factor for the reaction. The experimental value is 2 x 109 dm3 mol-1 s-1. Suggest a reason for any discrepancy.
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
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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The activation energy for the reaction 2 NO2(g) → 2 NO(g) + O2(g) is 111 kJ mol- 1. What proportion of the collisions between NO2 molecules have enough energy toresult in reaction when the temperature is (a)20 oC. (b)200 °C? Use collision theory to estimate the pre-exponential factor for the reaction. The experimental value is 2 x 109 dm3 mol-1 s-1. Suggest a reason for any discrepancy.
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