DECOMPOSITION OF AZOMETHANE
Review
Overall Reaction | AZO → C2H6 + N2 | |||
Experimental Rate Law (at low [AZO]) | +d[N2]/dt = ka[AZO]2 | |||
Proposed Mechanism | ||||
Overall Rate of Production of (Azomethane)* | d[AZO*]/dt = + k1[AZO]2 - k-1[AZO][AZO*] - k2[AZO*] | |||
Rate of Production of Nitrogen in the 1st Elementary Step | (d[N2]/dt)1 = 0 | |||
Rate of Production of Nitrogen in the 2nd Elementary Step | (d[N2]/dt)2 = 0 | |||
Rate of Production of Nitrogen in the 3rd Elementary Step | (d[N2]/dt)3 = +k2[AZO*] |
Overall Rate of Production of Nitrogen {+d[N2/dt}
The overall rate of production of (azomethane)* was calculated by summing the production rates in the elementary steps. In the same way the overall rate of production of Nitrogen can be found by summing the Nitrogen production rates in the individual steps:
d[N2]/dt = 0 + 0 + k2[AZO*] = k2[AZO*]
Overall Rates of the other Species
By using the same technique the overall rate of consumption of azomethane {-d[AZO]/dt}, and the overall rate of production of ethane {+d[C2H4]/dt} can be determined as:
-d[AZO]/dt = + k1[AZO]2 - k-1[AZO][AZO*]+d[C2H4]/dt = k2[AZO*]
Application of the Steady State Approximation
Comparing the results, it can be seen that the expression derived from the proposed mechanism
d[N2]/dt = k2[AZO*]does not give the experimental rate law
d[N2]/dt = ka[AZO]2
A (model) plot of the concentration profiles of the species involved in the decomposition of azomethane is given below.
Given this, if the Steady Approximation is to be used, it should be applied to