An unusual atmospheric reaction leading to ozone destruction is CF3O + O3 → CF3O2 + O2 the analysis of which has yielded an Arrhenius frequency factor (A) and activation energy of 2.0 × 10–12 cm3 molecule–1 s–1 and 11.6 kJ/mol, respectively. Calculate the rate constant for this reaction at an altitude of 35 km, where the temperature is –34°C.

Given, Activation energy, Ea = 11.6 kJ/mol = 11600 J/mol Frequency factor, A = 2.0 x 10-12 cm3.molecule-1 s-1 = 2.0x10-12x0.001Lx(6.022x1023mol-1)xs-1 = 12.044 x 108 L.mol-1s-1 Temperature T = -34 °C = (-34 + 273) K = 239 K We know that, According to Arrhenius equation, k = A e-Ea/RT where, k = rate constant R = universal gas constant = 8.314 J.mol-1K-1 k = 12.044 x 108 x e-(11600/8.314x239) k = 3.5 x 106 M-1s-1 Hence, the rate constant = 3.5 x 106 M-1s-1

Answered: An unusual atmospheric reaction leading…

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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An unusual atmospheric reaction leading to ozone destruction is

CF₃O + O₃ → CF₃O₂ + O₂

the analysis of which has yielded an Arrhenius frequency factor (A) and activation energy of 2.0 × 10^–12 cm³ molecule^–1 s^–1 and 11.6 kJ/mol, respectively. Calculate the rate constant for this reaction at an altitude of 35 km, where the temperature is –34°C.

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