## Gibbs energy of activation (standard free energy of activation), $$\Delta ^{\ddagger}G^{\,\unicode{x26ac}}$$

https://doi.org/10.1351/goldbook.G02631
The standard @G02629@ difference between the @T06468@ of a reaction (either an @E02035@ or a @S05970@) and the @G02704@ of the reactants. It is calculated from the experimental @O04322@ $$k$$via the conventional form of the absolute rate equation: $\Delta ^{\ddagger}G = R\ T\ \left[\ln (\frac{k_{\text{B}}}{h}) - \ln (\frac{k}{T})\right]$ where $$k_{\text{B}}$$ is the @B00695@ and $$h$$ the @P04685@ ($$\frac{k_{\text{B}}}{h} = 2.083\ 58\times 10^{10}\ \text{K}^{-1}\ \text{s}^{-1}$$). The values of the rate constants, and hence Gibbs energies of @A00093@, depend upon the choice of concentration units (or of the thermodynamic @S05925@).