For the reaction of the decomposition of nitramide in aqueous solution: O_2NNH_2

Question

For the reaction of the decomposition of nitramide in aqueous solution: O_2NNH_2(aq) rightarrow N_2O(g) + H_2O(I) with: d[N_2O]/dt = K [O_2NNH_2]/[H^+] As the observed rate law. A proposed mechanism is: O_2NNH_2(aq) doubleheadarrow O_2NNH(aq) + H^+ (aq) O_2NNH'(aq) rightarrow N_2O(g) + OH'(aq) H^+(aq) + OH'(aq) rightarrow H_2O(I) The observed rate law is: a.) Apply Steady-Slate to this mechanism to produce a predicted rate law. What is required in order for the mechanism to fit the observed rate law? b.) Apply the Fast Equilibrium approach assuming that the second step is the slow step. c.) Argue that the SS approach when adjusted is identical in concept to the FE approach.

Explanation / Answer

O2NNH2 -> N2O + H2O

a) in steady state the same produced reacts

O2NNH2 ----------> O2NNH- + H+

  O2NNH- ----------> N2O + OH- the sum of the reacctions give O2NNH2 ----------------> N2O + H2O

V = d(N2O)/d(t) =) d(N2O)/d(t) =k[O2NNH2] the H+ and the OH- have to fast reacction than no affects

need be order 2 whit respect to reacctive for fit

b) for fast equilibrium the low step is  O2NNH- ----------> N2O + OH-

V = d(N2O)/d(t) =) d(N2O)/d(t) =Kk[O2NNH-]/[OH-]

c) used than all decomposes to O2NNH2 ----------> O2NNH- + H+

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