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344                               Nonelementary Reaction Kinetics   Chap. 7

                          in which case the rate expression follows first-order kinetics,

                                                   - kl k3
                                                'N2  - - cAZO  = kCAZO                (7-20)
                                                      k2
           Apparent reaction   In describing reaction orders for this equation one would say the reaction
                   orders   is apparent Brst-order  at  high  azomethane  concentrations  and apparent  sec-
                         ond-order at low azomethane concentrations.


                         7.2  Searching for a Mechanism

                         In many instances the rate data are correlated before a mechanism is found. It
                         is a normal procedure to reduce the additive constant in the denominator to  1.
                         We  therefore divide the numerator  and denominator of Equation  (7-18) by k3
                         to obtain


                                                                                      (7-21)



                              7:2.1  General Considerations

                              The rules of thumb listed in Table 7-1 may be of some help in the devel-
                         opment of a mechanism that is consistent with the experimental rate law. Upon
                         application  of  Table  7-1  to  the  azomethane  example just  discussed,  we  see
                         from rate equation (7- 18) that:
                              1.  The  active  intermediate,  AZO*, collides  with  azomethane,  AZO
                                 [Equation (7-7)], resulting  in the  appearance  of  the concentration  of
                                 AZO in the denominator.
                              2.  AZO* decomposes spontaneously [Equation (7-9)], resulting in a con-
                                 stant in the denominator of the rate expression.
                              3.  The  appearance  of  AZO in  the  numerator  suggests  that  the  active
                                intermediate AZO* is formed from AZO. Referring to Equation (7-5),
                                we see that this case is indeed true.

                                   TABLE 7-1,  RULES OF THUMB  FOR  DEVELOPMENT OF A  MECHANISM
                         1. Species having the concentration(s) appearing in the denominator.of the rate law probably col-
                           lide with the active intermediate, e.g.,
                                              A + A'  ---+ [collision products]
                         2. If a constant appears in the denominator, one of the reaction steps is probably the spontaneous
                           decomposition of the active intermediate, e.g.,
                                              A* ---+   [decomposition products]
                         3.  Species having  the concentration(s) appearing in the numerator of  the rate law probably pro-
                           duce the active intermediate in one of the reaction steps, e.g.,
                                            [reactant]  ---+  A" + [other products]
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