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Learn how to calculate the equilibrium constant (Kp) using partial pressures in chemical reactions.
The equilibrium constant for a reaction depends on how the balanced equation is written. If the equation is reversed, K is inverted. If the equation is multiplied by a factor n, K is raised to the nth power. If multiple equations are added together, K for the overall equation is the product of the K values for the equations that were summed.
Unit 7: Chemical Equilibrium. Our mission is to provide a free, world-class education to anyone, anywhere. Khan Academy is a 501 (c) (3) nonprofit organization. Donate or volunteer today!
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.
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Autoionization of water, the autoionization constant Kw, and the relationship between [H⁺] and [OH⁻] in aqueous solutions.
The solubility product constant, Kₛₚ, is an equilibrium constant that reflects the extent to which an ionic compound dissolves in water. For compounds that dissolve to produce the same number of ions, we can directly compare their Kₛₚ values to determine their relative solubilities.
We will learn in detail about equilibrium constants, reaction quotient, Le-Chatelier's principle, acids, bases, salts, pH, acid-base equilibria, buffer solutions, and solubility equilibria.
The relationship between standard Gibbs free energy change and the equilibrium constant K. Calculating K when you know the standard free energy of reaction.