7.Problem 2.19 in the textbook. Complex Kinetics: \begin{array}{c} A+A \leftrightarrow A+A^{*} \\ A^{*} \rightarrow R+S \end{array} Where, k; and k2 are the rate constants for the forward and reverse reactions involved in the first step, respectively, and k3 is the rate constant for the irreversible reaction to form R and S. 2.19. The decomposition of reactant A at 400°C for pressures between 1 and 10 atm follows a first-order rate law. (a) Show that a mechanism similar to azomethane decomposition, p. 21, \begin{array}{r} A+A \rightleftarrows A^{*}+A \\ A^{*} \rightarrow R+S \end{array} is consistent with the observed kinetics. Different mechanisms can be proposed to explain first-order kinetics. To claim that this mechanism is correct in the face of the other alternatives requires additional evidence. (b) For this purpose, what further experiments would you suggest we run and what results would you expect to find?

Solved: 7.Problem 2.19 in the textbook. Complex Kinetics: \begin{array}{c} A+

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7.Problem 2.19 in the textbook. Complex Kinetics: \begin{array}{c} A+A \leftrightarrow A+A^{*} \\ A^{*} \rightarrow R+S \end{array} Where, k; and k2 are the rate constants for the forward and reverse reactions involved in the first step, respectively, and k3 is the rate constant for the irreversible reaction to form R