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= d[O2]/dt = ???