Editing Reaction quotient (section)

== Applications ==
The reaction quotient can be used to predict the direction and extent of an equilibrium chemical reaction. At equilibrium, the reaction quotient (Q) is equal to the equilibrium constant (K) for the reaction, where Q = K. If Q > K, the formation of reactants is favored. This is because the ratio of the numerator to the denominator in Q is greater than that of K, indicating there are more products than at equilibrium. As [[Le Chatelier's principle|Le Chatelier's Principle]] states systems tend towards equilibrium, the equilibrium shifts in the reverse direction favoring the formation of the products. Similarly, when Q < K, the formation of products is favored and the reaction is progressing in the forwards direction. <ref>{{Cite web |date=2013-10-02 |title=The Reaction Quotient |url=https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Equilibria/Chemical_Equilibria/The_Reaction_Quotient |access-date=2025-05-15 |website=Chemistry LibreTexts |language=en}}</ref>