(a) Apply the steady-state approximation to the N2O5decomposition mechanism (16.8) and show that r = k[N2O5], where k = kakb/(k−a + 2kb). (Hint: Use the steady-state approximation for both intermediates.) (b) Apply the rate-determining- step approximation to the N2O5 mechanism, assuming that step b is slow compared with steps a and c. (c) Under what condition does the rate law in (a) reduce to that in (b)? (d) The rate constant for the reaction in Prob. 16.50 is numerically equal to the rate constant for the N2O5 decomposition. Devise a mechanism for the reaction in Prob. 16.50 that will explain this fact.
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