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 = ???
A) Δ[O₂]/Δt = K₁[K⁻¹][NO₂][NO₃] - K₂[NO₂][NO₃]
B) Rate of reaction = Δ[O₂]/Δt = K₁[K⁻¹][NO₂]/K₂
C) Rate of reaction = Δ[O₂]/Δt = K₁[K⁻¹][NO₃]/K₂
D) Rate of reaction = Δ[O₂]/Δt = K₂[K⁻¹][NO₂]/K₁
