The mechanism for the reaction described by 2N2O5 (g) - - - > 4NO2 (g) + O2 (g) is suggested to be (1) N2O5 (g) (k1) - - - > (K-1) NO2 (g) + NO3 (g) (2) NO2 (g) + NO3 (g) - - - > (K2) NO2 (g) + O2 (g) + NO (g)
(3) NO (g) + N2O5 (g) - - - > (K3) 3NO2 (g) Assuming that [NO3] is governed by steady-state conditions, derive the rate law for the production of O2 (g) and enter it in the space below.
Rate of reaction = ∆[O2]/∆t = ?
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