Compute ΔG = ΔH − TΔS (ensure consistent units: ΔH in kJ/mol, ΔS in J/mol·K).
Gibbs Free Energy (ΔG)
0.0000 kJ/mol
0.00 J/mol
Formula: ΔG = ΔH − TΔS
Reaction at Equilibrium
Gibbs free energy (G) is a thermodynamic potential that indicates the maximum reversible work obtainable from a process at constant temperature and pressure. ΔG helps predict whether a process is thermodynamically favourable under given conditions.
Note: ΔG addresses thermodynamic spontaneity, not kinetics. A negative ΔG means the reaction is energetically favourable, but it may still be slow without a suitable pathway or catalyst.
ΔG is Gibbs free energy change; negative values indicate spontaneous (exergonic) processes at constant T and P.
ΔH in kJ/mol, ΔS in J/(mol·K), ΔG returned in kJ/mol and J/mol.
ΔS provided in J/(mol·K) is converted to kJ/(mol·K) by dividing by 1000 to match ΔH units.
Temperature must be positive (kelvin). Use absolute temperature.
ΔG indicates thermodynamic favorability, not reaction rate — kinetics and activation energy matter too.
Yes — ΔG depends on temperature; use temperature-specific ΔH and ΔS when available.
ΔG = 0 indicates the system is at equilibrium under the given T and P.
This is a calculator for idealized thermodynamic math; consult literature for empirical values.
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