The mechanism for the reaction described by

Question

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 = ???

Answer 1

[NO3]

Answer 2

k1k2[N2O5] / k2+k-1

*the numbers following the k's are the subscripts