The decomposition of nitramide, O2NNH2, in water has the following chemical equa
ID: 1037058 • Letter: T
Question
The decomposition of nitramide, O2NNH2, in water has the following chemical equation and rate law.
The decomposition of nitramide, O2NNH2, in water has the following chemical equation and rate law O,NNH, rate= k A proposed mechanism for this reaction is 1) o,NNH,(aq) o,NNH-(aq)+H(a)(fast equilibrium) (2) 02 NNH (aq) ? N2O(g) + OH(aq) slow fast) What is the relationship between the observed value of k and the rate constants for the individual steps of the mechanism? Drag the symbols into the numerator or denominator as neededExplanation / Answer
From equation 1 fast equilibrium so Rf = Rb ; K1[O2NH2] = K-1[O2NHN-][H+] .......(a)
We know rate is decided by slow Rxn so from 2 d[N2O]/dt = K2[O2NHN-]............(c) ; [O2NHN-] from (a) to (c) ;
d[N2O]/dt = K2K1[O2NH2]/ K-1[H+] = K [O2NH2]/[H+]
So finally K = K2K1/K-1