The decomposition of nitramide, O2NNH2, in water has the chemical equation and rate law O2NNH2(aq)⟶N2O(g)+H2O(l)rate=k[O2NNH2][H
+] A proposed mechanism for this reaction is O2NNH2(aq)⥫⥬=k−1k1O2NNH−(aq)+H+(aq)(fast equilibrium) O2NNH−(aq)−→k2N2O(g)+OH−(aq)(slow) H+(aq)+OH−(aq)−→k3H2O(l)(fast) What is the relationship between the observed value of k and the rate constants for the individual steps of the mechanism?
