law of mass action
E554718
The law of mass action is a fundamental principle in chemistry stating that the rate and equilibrium position of a chemical reaction depend on the concentrations of the reacting substances, each raised to a power corresponding to its stoichiometric coefficient.
Statements (50)
| Predicate | Object |
|---|---|
| instanceOf |
chemical law
ⓘ
principle of chemical equilibrium ⓘ principle of chemical kinetics ⓘ |
| appliesIn |
biochemical reactions
ⓘ
enzyme kinetics models ⓘ gas-phase reactions ⓘ solution-phase reactions ⓘ |
| appliesTo |
chemical reactions
ⓘ
elementary reactions ⓘ homogeneous reactions ⓘ |
| assumes |
constant temperature
ⓘ
elementary reaction mechanism for direct use of stoichiometric exponents in rate law ⓘ ideal behavior of reacting species ⓘ |
| basisFor |
Michaelis–Menten kinetics derivation
ⓘ
equilibrium constant expressions in analytical chemistry ⓘ mass-action kinetics in systems biology ⓘ |
| countryOfOrigin | Norway ⓘ |
| dependsOn |
stoichiometric coefficients of the balanced reaction
ⓘ
temperature via equilibrium constant K ⓘ |
| describes |
relationship between equilibrium constant and reactant and product activities
ⓘ
relationship between reaction rate and reactant concentrations ⓘ |
| field |
chemical kinetics
ⓘ
chemistry ⓘ thermodynamics ⓘ |
| formulatedBy |
Cato Maximilian Guldberg
NERFINISHED
ⓘ
Peter Waage NERFINISHED ⓘ |
| generalizedBy | statistical mechanics ⓘ |
| hasLimitation |
does not strictly apply to non-ideal solutions without activity corrections
ⓘ
stoichiometric exponents equal kinetic orders only for elementary steps ⓘ |
| historicalPublication | Guldberg and Waage's papers on chemical affinity in the 1860s ⓘ |
| involvesQuantity |
activity
ⓘ
concentration ⓘ equilibrium constant ⓘ reaction rate ⓘ |
| mathematicalForm |
K = ∏a_product^{ν_product} / ∏a_reactant^{ν_reactant}
ⓘ
rate = k ∏[reactant_i]^{ν_i} ⓘ |
| relatedTo |
Arrhenius equation
NERFINISHED
ⓘ
Gibbs free energy NERFINISHED ⓘ Le Chatelier's principle NERFINISHED ⓘ chemical potential ⓘ equilibrium thermodynamics ⓘ |
| states |
at equilibrium the ratio of product activities to reactant activities each raised to their stoichiometric coefficients is constant at a given temperature
ⓘ
reaction rate is proportional to the product of reactant concentrations each raised to a power equal to its stoichiometric coefficient ⓘ |
| symbolizedBy | K for equilibrium constant ⓘ |
| usedFor |
calculating equilibrium compositions
ⓘ
deriving rate laws of elementary reactions ⓘ predicting direction of chemical reactions ⓘ writing equilibrium constant expressions ⓘ |
| yearDeveloped | 1867 ⓘ |
| yearProposed | 1864 ⓘ |
Referenced by (1)
Full triples — surface form annotated when it differs from this entity's canonical label.