The decomposition of nitramide, O2NNH2, in water has the following chemical equa

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 needed

Explanation / 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

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