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The relationship between the standard Gibbs free energy change Δ r G o and chemical equilibrium is revealing. This relationship is defined by the equation Δ r G o = -RT ln(K), where K is the equilibrium constant, which is equal to the reaction quotient Q in equilibrium.
An equilibrium constant is related to the standard Gibbs free energy change of reaction by Δ G ⊖ = − R T ln K ⊖ , {\displaystyle \Delta G^{\ominus }=-RT\ln K^{\ominus },} where R is the universal gas constant , T is the absolute temperature (in kelvins ), and ln is the natural logarithm .
In thermodynamics, the Gibbs free energy (or Gibbs energy as the recommended name; symbol ) is a thermodynamic potential that can be used to calculate the maximum amount of work, other than pressure–volume work, that may be performed by a thermodynamically closed system at constant temperature and pressure.
Free energy relationships establish the extent at which bond formation and breakage happen in the transition state of a reaction, and in combination with kinetic isotope experiments a reaction mechanism can be determined. Free energy relationships are often used to calculate equilibrium constants since they are experimentally difficult to ...
Some, perhaps most, of the Gibbs free energy of reaction may be delivered as external work. The hydrolysis of ATP to ADP and phosphate can drive the force -times- distance work delivered by living muscles , and synthesis of ATP is in turn driven by a redox chain in mitochondria and chloroplasts , which involves the transport of ions across the ...
where ln denotes the natural logarithm, is the thermodynamic equilibrium constant, and R is the ideal gas constant. This equation is exact at any one temperature and all pressures, derived from the requirement that the Gibbs free energy of reaction be stationary in a state of chemical equilibrium.
The AMP is regenerated to ATP in two steps, with the equilibrium reaction ATP + AMP ↔ 2ADP, followed by regeneration of ATP by the usual means, oxidative phosphorylation or other energy-producing pathways such as glycolysis. [citation needed] Often, high-energy phosphate bonds are denoted by the character '~'.
For systems at constant volume the Helmholtz free energy is minimum and for systems at constant pressure the Gibbs free energy is minimum. [3] Thus a metastable state is one for which the free energy change between reactants and products is not minimal even though the composition does not change in time. [4]