All chemical reactions have the possibility to be reversible. We must reserve this possibility by writing these reaction networks as reversible reactions in order that a description of the equilibrium state can be given; even in cases that remain far from equilibrium under any practical conditions, the equilibrium state sets constraints on the values of the rate constants and their relationship to one another. When the "missing" reverse reactions are included in both Models I and II, the equilibrium relationships dictated by these reactions are given as shown on the right side of Scheme 11. These equilibrium relations emphasize that this condition holds under equilibrium by using the subscript "eq" for the concentrations [A]eq, [L]eq, and [D]eq, even if the possibility of achieving this state is low. These equations may then be manipulated to show that the relationship between these rate constants, as set by the equilibrium condition, is given by the equation at bottom of Scheme 11, which contains only rate constants (no concentration variables), and which holds under all conditions, near to or far from equilibrium. This relationship demonstrates that only three of the four rate constants are independent; once the values for the three rate constants are set, the fourth is fixed by this relationship. Scheme 11. Proposed models invoking reversibility in asymmetric autocatalytic reactions. Left: reactions proposed in the model; middle: reverse reactions that are "missing", i.e., not considered in the model; right: equilibrium constants for complete reversible reaction network; bottom: relationship between forward and reverse reaction rate constants dictated by chemical thermodynamics for both models, demonstrating that only three of the four rate constants are independent.