𝐺 𝑅/𝑃 = 𝜀 0,𝑅/𝑃 -𝓀 𝐵 𝑇 ln(𝑠𝑇 𝑔 𝑅/𝑃 (𝑇)) (24e) Now, I can write the equilibrium constant (Eq. 25a) and the rate equation (Eq. 25b) in their most simple form with the rate constant 𝑘 𝑓/𝑏 for the forward and backward reaction term (Eq. 25c), respectively. 𝑁 𝑅 can be rewritten in other more common terms, such a concentrations or chemical activities when 𝑟 and 𝑘 𝑓/𝑏 are normalized accordingly. (25c) I can then rewrite Eq. 25c using Eq. 21c and obtain the Eyring equation. Note, that the herein presented derivation does not need to introduce a transfer coefficient and substantiates the convention in the traditional expression of the Eyring equation where the value of such coefficient, commonly 𝜅, is set to unity. However, the Gibbs Free energy in the transition state (Eq. 26c) now possesses a slightly different meaning compared to the traditional transition state theory: It does not refer to an activated complex, that is, as Eyring himself wrote, in all things equal to an actual chemical compound. Instead, its meaning is more complex as 𝜔(𝑇) is the weighted sum of the transfer rates over all configurations. 𝜀 ‡ describes the energy level below which the contribution of the partial sum to the total sum 𝜔(𝑇) is effectively zero. In that sense, the herein presented derivation is more general than the derivation performed by Eyring, while less useful if one attempts to predict 𝐺 ‡ from first principles since it would require near-perfect knowledge over both the configuration space and transition event rates. However, if such knowledge could be obtained, the precise prediction of reaction rates should be possible using the herein-defined expressions.