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 553g: 71


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Work Step by Step

The slow-step is rate-determining. N2O2 is an intermediary since it's not present in the global reaction. For the slow step $r=r_S=k_S[O_2][N_2O_2]$ for the equilibrium back reaction: $r_{-F}=k_{-F}[N_2O_2]=r_F=k_F[NO]^2$ $r=k_S[O_2]r_{-F}/k_{-F}=(k_Sk_F/k_{-F})[O_2][NO_2]^2$ $r=k[O_2][NO_2]^2$
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