Composite Reactions & the Steady State Approximation

DECOMPOSITION OF AZOMETHANE

Introduction

Azomethane, (CH3)2N2, decomposes in the gas phase to give ethane and nitrogen:

(CH3)2N2 → C2H6 + N2

Experimental observations have shown that the rate law for this reaction, at low azomethane concentrations, is:

+d[N2]/dt = ka[(CH3)2N2]2

A proposed mechanism for this reaction is:

[Azomethane Mechanism (1)]

In this worked example: An appropriate rate expression will be derived from the proposed mechanism. This rate expression will be compared with the experimental rate law in order to determine whether or not the proposed mechanism and the experimental rate law are consistent.

Note: For the remainder of this example (CH3)2N2 will be represented by AZO and ((CH3)2N2)* will be represented by AZO*, i.e.

Overall ReactionAZO → C2H6 + N2
Experimental Rate Law+d[N2]/dt = ka[AZO]2
Proposed Mechanism[Azomethane Mechanism (1a)]

Composite or Elementary?

The first step is to determine whether or not the reaction is elementary.

If the reaction

AZO → C2H6 + N2
was elementary, the rate law could be written as:

+d[N2]/dt = k[C2H6]

+d[N2]/dt = k[C2H6][N2]

+d[N2]/dt = k[AZO][C2H6][N2]

+d[N2]/dt = k[AZO]

+d[N2]/dt = k[AZO]2