How can you determine the rate law of the following reaction?
2NO (g) + O2 (g) → 2NO2 (g)
2NO (g) + O2 (g) → 2NO2 (g)
The possible mechanism for the reaction will be
i) NO + O2 ⇌ NO3 (fast)…………………k(equilibrium constant)
ii) NO3+ NO⇌ NO2 + NO2 (slow)…………………..k’
Rate is determined by the slow step, so
Rate = k’[NO3][NO]…………………1)
K= [NO3]/[NO] [O2]
K[NO] [O2] = [NO3]………………a)
By putting values of a) in 1)
Rate = k’k[NO][O2][NO]
=k’k[NO]2[O2]
The rate of the reaction can be determined by
Rate = k[NO]2[O2]1