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ChemBench
The bridge between thermodynamics and equilibrium — how energy determines where a reaction settles.
A large negative ΔG° gives a large K (products favored), while a large positive ΔG° gives a tiny K (reactants favored). At ΔG° = 0, K = 1 and neither side is favored — the relationship ΔG° = −RT ln K quantifies exactly how strongly a reaction favors products or reactants.
Even with the same ΔG°, changing temperature changes K because of the RT factor — this is the mathematical basis of Le Chatelier's principle for temperature changes, and it's why some reactions that are unfavorable at room temperature become favorable at high temperatures.
Molar mass of any chemical formula (e.g. H2O, C6H12O6, Ca(OH)2).
OpenPercent composition of an element within a chemical formula.
OpenSimplest whole-number ratio formula from elemental masses or percentages.
OpenPercent yield from actual and theoretical reaction yields.
OpenEquilibrium constant K
7.524
What you entered
−ΔG° ÷ RT
−(-5000) ÷ (8.314 × 298)= 2.0181K = e^(−ΔG°/RT)
e^(2.0181)= 7.5241Result
Equilibrium constant K: 7.524
With ΔG° = -5000 J/mol at 298 K, the equilibrium constant K = 7.524. Products are favored at equilibrium.