The mechanism for the reaction described by 2N₂O₅(g) → 4NO₂(g) + O₂(g) is suggested to be as follows: (1) N₂O5(g) ⇌ (K-1) NO₂(g) + NO₃(g) (2) NO₂(g) + NO₃(g) ⇌ (K₂) NO₂(g) + O₂(g) + NO(g) Assuming that [NO₃] is governed by steady-state conditions, derive the rate law for the production of O₂(g).
A) Rate of reaction = 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