Final answer:
The relationship between the dissociation constant (Kd) and the Free Energy of Reaction (ΔG) is characterized by the equation ΔG° = -RTlnK. Kd is the inverse of the formation constant and indicates the concentration of ligands for half occupancy. Knowledge of ΔG or K allows calculation of the other, linking thermodynamics and equilibrium.
Step-by-step explanation:
The relationship between the dissociation constant (Kd) and the Free Energy of Reaction (ΔG) is a fundamental concept in chemistry. According to the given reference, the free energy change (ΔG°) can be related to the equilibrium constant by the equation ΔG° = -RTlnK, where R is the gas constant, T is the temperature in Kelvin, and K could be the equilibrium constant for either concentrations (Kc) or partial pressures (Kp) of reactants and products at equilibrium. When considering the reverse reaction, such as the decomposition of a complex ion, the dissociation constant (Kd) is used instead, and it is the mathematical inverse of the formation constant (Kd = K⁻¹).
It is important to understand that the dissociation constant is associated with the reaction in which a complex ion breaks down into its components, and it reflects the concentration of ligands at which half of the available sites are occupied. Knowledge of either the standard free energy change or the equilibrium constant allows for the calculation of the other, thus connecting thermodynamics with the concept of chemical equilibrium.