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- https://chem.libretexts.org/Courses/Los_Angeles_Trade_Technical_College/Analytical_Chemistry/2%3A_Analytical_Chemistry_2.0_(Harvey)/14%3A_Kinetic_Methods/14.2%3A_Chemical_KineticsEvery chemical reaction occurs at a finite rate, making it a potential candidate for a chemical kinetic method of analysis. To be effective, however, the chemical reaction must meet three necessary co...Every chemical reaction occurs at a finite rate, making it a potential candidate for a chemical kinetic method of analysis. To be effective, however, the chemical reaction must meet three necessary conditions: the reaction must not occur too quickly or too slowly; we must know the reaction’s rate law; and we must be able to monitor the change in concentration for at least one species.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Physical_Chemistry_(LibreTexts)/29%3A_Chemical_Kinetics_II-_Reaction_Mechanisms/29.08%3A_A_Catalyst_Affects_the_Mechanism_and_Activation_EnergyThis page covers the role of catalysts in chemical reactions, highlighting their ability to lower activation energy and increase reaction rates without being consumed. It distinguishes between homogen...This page covers the role of catalysts in chemical reactions, highlighting their ability to lower activation energy and increase reaction rates without being consumed. It distinguishes between homogeneous and heterogeneous catalysts and details mechanisms like Langmuir-Hinshelwood and Eley-Rideal in gas-phase reactions on solid surfaces. The importance of surface area is discussed, along with equations for reaction rates and concentrations.
- https://chem.libretexts.org/Bookshelves/General_Chemistry/General_Chemistry_Supplement_(Eames)/Chemistry_Calculations/StoichiometryIn many chemical reactions, both directions are possible; when they are happening at the same rate, that is called dynamic equilibrium, which means "moving equilibrium", because the individual molecul...In many chemical reactions, both directions are possible; when they are happening at the same rate, that is called dynamic equilibrium, which means "moving equilibrium", because the individual molecules are moving back and forth between "reactant" and "product" (which are really just defined by how you write the equation), but the total amounts of reactant and product aren't changing.
