The equilibrium constant, $K$, is a ratio that quantifies the concentrations of reactants and products in a chemical reaction at equilibrium. It provides insight into the position of the equilibrium and the extent to which reactants are converted into products.
congrats on reading the definition of equilibrium constant, K. now let's actually learn it.
The value of $K$ is temperature-dependent; it changes with temperature.
For a reaction: $aA + bB \rightleftharpoons cC + dD$, the equilibrium constant expression is given by $K = \frac{[C]^c[D]^d}{[A]^a[B]^b}$.
$K > 1$ indicates that products are favored at equilibrium, while $K < 1$ indicates that reactants are favored.
Pure solids and liquids do not appear in the expression for $K$; only aqueous and gaseous species are included.
$K_p$ is used for reactions involving gases and relates to partial pressures, whereas $K_c$ relates to molar concentrations.
Review Questions
What does it mean if an equilibrium constant, $K$, is greater than 1?
How does temperature affect the value of an equilibrium constant, $K$?
Write the general form of an equilibrium constant expression for a given balanced chemical equation.
Related terms
$Le \ Chatelier's \ Principle$: States that if a dynamic equilibrium is disturbed by changing conditions, the position of equilibrium moves to counteract the change.
$Reaction \ Quotient \ (Q)$: Calculates the ratio of product concentrations to reactant concentrations at any point during a reaction before reaching equilibrium.
$Dynamic \ Equilibrium$: Occurs when the rate of the forward reaction equals the rate of the reverse reaction, resulting in no net change in concentrations of reactants and products.