The sign of ΔG tells us whether products or reactants are favoured at equilibrium
المؤلف:
Jonathan Clayden , Nick Greeves , Stuart Warren
المصدر:
ORGANIC CHEMISTRY
الجزء والصفحة:
ص243-244
2025-05-15
634
In the equilibrium above, the hydrate is higher in energy than the aldehyde: at equilibrium there is more aldehyde than hydrate, and the equilibrium constant is therefore less than 1. Whenever this is the case (i.e. the equilibrium lies to the side of the reactants, rather than the products) K will be less than 1. This means that its logarithm must be negative and, because ΔG = –RTlnK, ΔG must be positive. Conversely, for a reaction in which products are favoured over reactants, K must be greater than 1, its logarithm will be positive, and hence ΔG must be negative. When K is exactly 1, since ln 1 = 0, ΔG will be zero.
●ΔG tells us about the position of equilibrium.
• If ΔG for a reaction is negative, the products will be favoured at equilibrium.
• If ΔG for a reaction is positive, the reactants will be favoured at equilibrium.
• If ΔG for a reaction is zero, the equilibrium constant for the reaction will be 1.
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