Search results
The equilibrium constant is the ratio of the concentrations raised to the stoichiometric coefficients. Therefore, the unit of the equilibrium constant = [Mole L-1] n. Where, ∆n = sum of stoichiometric coefficients of products – sum of stoichiometric coefficients of reactants. ⇒ Also Read: Chemical Equilibrium; Ionic Equilibrium
Aug 14, 2020 · The ratio of the rate constants for the forward and reverse reactions at equilibrium is the equilibrium constant (\(K\)), a unitless quantity. The composition of the equilibrium mixture is therefore determined by the magnitudes of the forward and reverse rate constants at equilibrium.
The equilibrium constant always has the same value (provided you don't change the temperature), irrespective of the amounts of A, B, C and D you started with. It is also unaffected by a change in pressure or whether or not you are using a catalyst. Compare this with the chemical equation for the equilibrium.
Every chemical equilibrium can be characterized by an equilibrium constant, known as K eq. The K eq and K P expressions are formulated as amounts of products divided by amounts of reactants; each amount (either a concentration or a pressure) is raised to the power of its coefficient in the balanced chemical equation.
This free textbook is an OpenStax resource written to increase student access to high-quality, peer-reviewed learning materials.
The equilibrium constant, K, describes the relative amounts of reaction species at equilibrium. The expression for K is equal to the concentrations (or partial pressures) of the products raised to their stoichiometric coefficients divided by the concentrations (or partial pressures) of the reactants raised to their stoichiometric coefficients.
Calculate equilibrium concentrations or pressures and equilibrium constants, using various algebraic approaches.
