Forward and reverse reactions occur at equal rates

No net change in concentrations of reactants and products

Occurs over time in a closed system

Concentrations of reactants and products become constant

Ratio of product concentrations to reactant concentrations

Each concentration raised to the power of its stoichiometric coefficient

K = Products^coefficients / Reactants^coefficients

Used when concentrations are expressed in moles per liter (M)

Used when equilibrium involves gases and their partial pressures

Describes the equilibrium between a solid and its ions in solution

If K > 1, products are favored

If K < 1, reactants are favored

Larger K values mean more complete reaction

K changes with temperature, not with concentration or pressure changes

Does not account for nonideal conditions or realworld complexities

Only describes the position of equilibrium, not how fast it is reached