Gibbs energy of activation (standard free energy of activation), \(\Delta ^{\ddagger}G^{\,\unicode{x26ac}}\)
The standard @[email protected] difference between the @[email protected] of a reaction (either an @[email protected] or a @[email protected]) and the @[email protected] of the reactants. It is calculated from the experimental @O0432[email protected] \(k\) 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 @[email protected] and \(h\) the @[email protected] (\(\frac{k_{\text{B}}}{h} = 2.083\ 58\times 10^{10}\ \text{K}^{-1}\ \text{s}^{-1}\)). The values of the rate constants, and hence Gibbs energies of @[email protected], depend upon the choice of concentration units (or of the thermodynamic @[email protected]).
See also:
enthalpy of activation
entropy of activation
PAC, 1994, 66, 1077. (Glossary of terms used in physical organic chemistry (IUPAC Recommendations 1994)) on page 1118 [Terms] [Paper]
PAC, 1996, 68, 149. (A glossary of terms used in chemical kinetics, including reaction dynamics (IUPAC Recommendations 1996)) on page 166 [Terms] [Paper]