Chemical Equilibrium
| Formula / Notation | K_eq = [C]^c[D]^d / ([A]^a[B]^b) at equilibrium; ΔG° = −RT ln K |
|---|---|
| Also Known As | Dynamic equilibrium, reaction equilibrium, thermodynamic equilibrium, K_eq |
What is Chemical Equilibrium?
Chemical equilibrium is the state in a reversible reaction where the rate of the forward reaction equals the rate of the reverse reaction, so that the concentrations of reactants and products remain constant over time. Equilibrium does not mean equal concentrations of reactants and products, only that they no longer change. It is described quantitatively by the equilibrium constant K.
Formula & Notation
Other Names / Synonyms: Dynamic equilibrium, reaction equilibrium, thermodynamic equilibrium, K_eq
Properties & Characteristics
Uses & Applications
Safety Information
Always consult the SDS/MSDS before handling any chemical. This information is for educational purposes only.
Key Facts
Frequently Asked Questions
Chemical equilibrium is the state in a reversible reaction where the rate of the forward reaction equals the rate of the reverse reaction, so that the concentrations of reactants and products remain constant over time. Equilibrium does not mean equal concentrations of reactants and products, only that they no longer change. It is described quantitatively by the equilibrium constant K.
Chemical equilibrium principles govern industrial synthesis (Haber process: N₂+3H₂⇌2NH₃; Contact process: SO₂+O₂⇌SO₃), acid-base chemistry (Ka, Kb), solubility equilibria (Ksp), and biochemical reactions. Equilibrium calculations are central to analytical chemistry and thermodynamics.
Systems at equilibrium may release toxic gases (H₂S, SO₂, HCN) if conditions are shifted. Industrial equilibrium processes operate under high pressure and temperature, requiring appropriate engineering controls and pressure safety systems.
The formula or notation for Chemical Equilibrium is: K_eq = [C]^c[D]^d / ([A]^a[B]^b) at equilibrium; ΔG° = −RT ln K