Question

6. The rate law for the following reaction is rate=k[NO2] (F2]: 2NO2(g) + F2(g) → 2NO2F(g) The mechanism proposed for this reaction is as follows: (i) NO2(g) + F2(g) → NO2F(g) + F(g) (ii) NO2(g) + F(g) → NO2F(g) Which elementary step is the rate-determining step in this reaction? Explain your answer in 1-2 sentences.

Answer 1

y mechanism :- stepa :- not fz » noof to = 193 19) Boj o steps : No + 7 NOF - 19) 6 d e over all - 200 + Fz » 200zF Reacken :- (9) (9) Given, Rate Law : Rale = K[no] Ez] we have a steps for given reaction mechanismo 9 if we assume ist step is slowest in the reaction mechanism then it is rate deteoming Step. - coefficats Rate =k [reactants] = K [no] [F] which is same as given. b if Step 2 is Rote determing step ) Rabe = F2C No] CB ] But É is an intermediate species.

Let assume Step I is reversible kei= [no_f] [E] C , LED - [F] =ko CNo] [E] - [NO, E we should replace F with other species 'cause F is an intermediate Rate = Fz Key (Nor] [F2) Tref] Let ta overall take constant = Kzike, Rate = k [no] [[2] if step II is. Enosf] tote determing step. 2. Any). Step (i) is rate determiny Step for given mechoshanism. since in dota no mentioning of slow loo) fast assume both are Datea determing steps and derive tole Law for them and compose it to given tate Law.