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Delta G not is the change in gibbs free energy given conditions under standard pressure (1 atm) and with stoichiometric coefficients corresponding to the balanced chemical reaction. Hence, the equation to calculated it is delta G not = -R * T * ln K. The K here represents concentrations at equilibrium ratios. Delta G represents the change in gibbs free energy of reaction not under stoichiometric ratios at equilibrium. Hence, delta G equals delta G not + R * T * ln Q. The Q represents concentrations not at equilibrium ratios.
refers to the Gibbs free energy of a reaction at the STANDARD state whereas refers to the Gibbs free energy under other non-standard conditions. For example, you might want to find when the reaction is occurring at a different temperature T or when it's not at equilibrium (find Q).
∆G is the change of Gibbs (free) energy for a system and ∆G° is the Gibbs energy change for a system under standard conditions (1 atm, 298K). ... Where ∆G is the difference in the energy between reactants and products. In addition ∆G is unaffected by external factors that change the kinetics of the reaction
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