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\section{Introduction}  Rates naturally characterize kinetic processes. In chemistry, determining the macroscopic rates of chemical reactions is one approach to learn the microscopic mechanism. The mechanism of molecular transoformations. Quantitatively this often leads to the empirical  mass-action rate laws are empirical results, assuming laws, for example, when  the reaction system is homogeneous with uniform concentration(s) throughout. Heterogeneity and fluctuations in structure, energetics, or concentrations can cause deviations from traditional rate laws. When traditional kinetics breaks down [insert citation], the process is statically and/or dynamically disordered kinetics [insert Zwanzig citation]. Theoretical approaches then adopt a distribution of rate coefficients, or a time dependent rate coefficient. The ability to quantify disorder is essential information for understanding your system. In our previous work a theory was developed for analyzing first order irreversible decay kinetics through an inequality[insert citation]. The convenience of this inequality is through its ability to quantify disorder, with the unique property of becoming an equality only when the system is disorder free, and therefore described by chemical kinetics in its classical formulation. The next problem that should be addressed is that of higher order kinetics, what if the physical systems one wishes to understand are more complex kinetic schemes, they would require a modified theoretical framework for analysis, but should and can be addressed. To motivate this type of development systems such as...... are all known to proceed through higher ordered kinetics, and all of these systems possess unique and interesting applications, therefore a more complete kinetics description of them should be pursued[insert citations].