Question

The decomposition of nitramide, O 2 NNH 2 , in water has the chemical equation and rate law O 2 NNH 2 ( aq ) ⟶ N 2 O ( g ) + H 2 O ( l ) rate = k [ O 2 NNH 2 ] [ H + ] A proposed mechanism for this reaction is O 2 NNH 2 ( aq ) k 1 ⇌ k − 1 O 2 NNH − ( aq ) + H + ( aq ) ( fast equilibrium ) O 2 NNH − ( aq ) k 2 −→ N 2 O ( g ) + OH − ( aq ) ( slow ) H + ( aq ) + OH − ( aq ) k 3 −→ H 2 O ( l ) ( fast ) What is the relationship between the observed value of k and the rate constants for the individual steps of the mechanism?

Answer 1

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