If Keq' > 1, what can be inferred about ∆G°'?

When the equilibrium constant (Keq') is greater than 1, it indicates that at equilibrium, the concentration of products is greater than the concentration of reactants. This scenario suggests that the reaction favors the formation of products. The relationship between the standard free energy change (∆G°') and the equilibrium constant is described by the equation:

∆G°' = -RT ln(Keq')

In this equation, R is the universal gas constant, T is the temperature in Kelvin, and ln is the natural logarithm.

When Keq' is greater than 1, the logarithm of Keq' (ln(Keq')) is positive, which means that -RT ln(Keq') will yield a negative value for ∆G°'. A negative ∆G°' signifies that the reaction is exergonic, meaning that it releases free energy and can proceed spontaneously under standard conditions. This is a key concept in thermodynamics and biochemistry, as reactions with negative free energy changes are thermodynamically favored to occur.

Therefore, when Keq' is greater than 1, it conclusively indicates that ∆G°' is negative, aligning with the definition of exergonic reactions.