Chemistry and Chemical Reactivity (9th Edition)

Published by Cengage Learning
ISBN 10: 1133949649
ISBN 13: 978-1-13394-964-0

Chapter 14 Chemical Kinetics: The Rates of Chemical Reactions - Study Questions - Page 553c: 39


$k_2=0.314\ s^{-1}$

Work Step by Step

From the Arrhenius equation: $ln(k_2/k_1)=-E_a/R(1/T_2-1/T_1)$ $ln(k_2/0.0315\ s^{-1})=-260\ kJ/mol/8.314\ J/mol.K(1/850\ K-1/800\ K)$ $k_2=0.314\ s^{-1}$
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