Linked from

The 66 pages that link to Gibbs free energy, each with the reason it gives.

• Chemical equilibriumRelated: At equilibrium, the Gibbs free energy of reaction is zero under constant-temperature, constant-pressure conditions.

• SolubilityRelated: The balance of enthalpy and entropy changes governs whether dissolution is favorable.

• HydrolysisRelated: Free-energy change distinguishes favorable hydrolysis from merely possible bond cleavage.

• Chemical potentialRelated: At fixed temperature and pressure, chemical potential is the Gibbs free-energy change per amount added.

• Phase transitionRelated: The stable phase minimizes Gibbs free energy under these conditions.

• ThermodynamicsRelated: Its decrease predicts the direction of spontaneous change under common laboratory conditions.

• Phase diagramRelated: The stable phase is the one with the lowest Gibbs free energy under given conditions.

• Nernst equationRelated: Equating reaction free energy with electrical work yields the equation.

• EnthalpyRelated: It combines enthalpy with entropy to assess processes at constant temperature and pressure.

• VolatilityRelated: Free-energy differences help determine which phase is favored under specified conditions.

• Electrochemical cellRelated: Its change sets the maximum electrical work obtainable from a reversible cell.

• Activation energyRelated: Its activation counterpart describes barriers in solution and other condensed phases.

• Equilibrium constantRelated: Its standard reaction change determines the equilibrium constant through an exponential relation.

• Le Chatelier's principleRelated: Equilibrium shifts are the system relaxing toward the lowest Gibbs free energy available.

• Redox potentialRelated: Potential differences translate into reaction free-energy changes through transferred charge.

• Standard electrode potentialRelated: The free-energy change of a redox reaction is related directly to its cell potential.

• Solvent effectRelated: Solvent stabilization changes species’ free energies and therefore reaction equilibria.

• Vapor–liquid equilibriumRelated: Stable coexistence minimizes Gibbs free energy subject to material balance.

• Chemical thermodynamicsRelated: Its change determines whether a reaction is thermodynamically favorable under constant-temperature, constant-pressure conditions.

• Exothermic reactionRelated: Its change combines enthalpy and entropy, clarifying why heat release is not sufficient.

• FugacityRelated: Fugacity encodes the pressure-dependent contribution to a component’s Gibbs chemical potential.

• Critical temperatureRelated: Its equilibrium minima determine which phase is stable at a specified temperature.

• State variableRelated: Its value, computed from state variables, helps predict chemical change.

• ATP hydrolysisRelated: Its change determines whether ATP hydrolysis can drive coupled cellular reactions.

• Phase equilibriumRelated: Stable mineral assemblages minimize this potential under fixed pressure and temperature.

• Reaction quotientRelated: The reaction free-energy change equals RT ln(Q/K), linking composition to spontaneity.

• Van ’t Hoff equationRelated: Combining its equilibrium relation with enthalpy yields the Van ’t Hoff equation.

• Gibbs–Duhem equationRelated: Differentiating its extensive composition dependence gives the fixed-temperature, fixed-pressure form.

• Walther NernstRelated: Its relation to reaction equilibrium underlies the Nernst equation.

• Pourbaix diagramRelated: The favored form in each region minimizes the relevant thermodynamic potential.

• Maxwell relationsRelated: Its natural variables generate relations involving entropy, pressure, volume, and temperature.

• Physical organic chemistryRelated: Free-energy differences connect molecular interactions to equilibrium and reaction direction.

• Chemical energyRelated: Its change accounts for energy available to drive useful work in reactions.

• Reversible reactionRelated: Its change helps determine the favored direction and equilibrium condition of a reaction.

• Allotropes of sulfurRelated: The lowest-free-energy sulfur structure is the stable form under specified conditions.

• Gibbs–Helmholtz equationRelated: The equation tracks how this potential changes with temperature.

• Phase ruleRelated: Phase coexistence is governed by conditions that minimize Gibbs free energy.

• Endothermic processRelated: Its change combines enthalpy and entropy, so positive enthalpy need not prevent spontaneity.

• Entropy of activationRelated: Activation free energy combines the corresponding enthalpic and entropic barrier contributions.

• Intensive and extensive propertiesRelated: Its extensive character and derivatives connect directly to chemical potential and equilibrium.

• Rudolph A. MarcusRelated: The reaction’s free-energy change helps determine its activation barrier in Marcus theory.

• EnzymologyRelated: It distinguishes an enzyme’s effect on reaction speed from its effect on reaction energetics.

• Exothermic processRelated: Its change combines enthalpy and entropy, so exothermicity alone cannot establish spontaneity.

• Reduction potentialRelated: The potential difference of a cell determines the free-energy change of its reaction.

• Energy utilizationRelated: It describes whether cellular reactions can provide or require usable energy.

• Germain Henri HessRelated: Reaction enthalpy from Hess’s law contributes to evaluating Gibbs energy changes.

• Multicomponent systemsRelated: Stable phase assemblages minimize the appropriate free energy.