The degradation of CF3CH2F (an HFC) by OH radicals in the troposphere is first order in each reactant and has a rate constant of k = 1.6 * 108 M-1s-1 at 4 °C. If the tropospheric concentrations of OH and CF3CH2F are 8.1 * 105 and 6.3 * 108 molecules>cm3, respectively, what is the rate of reaction at this temperature in M>s?

The degradation of CF3CH2F (an HFC) by OH radicals in the troposphere is first order in each reactant and has a rate constant of k = 1.6 * 108 M-1s-1 at 4 °C. If the tropospheric concentrations of OH and CF3CH2F are 8.1 * 105 and 6.3 * 108 molecules>cm3, respectively, what is the rate of reaction at this temperature in M>s?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter8: Properties Of Gases

Section: Chapter Questions

Problem 77QRT

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