A method to simplify reaction mechanisms by assuming that the rate of formation and depletion of intermediates are equal.
Reaction Rates: The change in the concentration of reactants and products over time in a chemical reaction.
Reaction Mechanisms: The sequence of chemical reactions that occur to convert reactants into products.
Rate Laws: The mathematical relationship between the rate of a chemical reaction and the concentration of the reactants.
Rate Determining Step: The slowest step of a reaction mechanism that restricts the overall rate of the reaction.
Steady-State Approximation: A method to simplify the rate expressions by assuming that an intermediate in a reaction mechanism is in a steady-state concentration.
Michaelis-Menten Kinetics: The model for the enzyme-catalyzed reactions in which the substrate binds to the enzyme to form the enzyme-substrate complex.
Enzyme Kinetics: The study of enzyme-catalyzed reactions in terms of enzyme properties and kinetic parameters.
Kinetic Isotope Effect: The difference in the rate of a chemical reaction between isotopes of the same element.
Temperature Dependence of Reaction Rates: The effect of temperature on the rate of a chemical reaction, which can be described by Arrhenius equation.
Activation Energy: The minimum energy required to start a chemical reaction.
Boltzmann Distribution: The statistical distribution of energy among particles in a system, which can be used to calculate the fraction of molecules with sufficient energy to overcome the activation energy.
Catalysts: The substances that increase the rate of a reaction without being consumed, by lowering the activation energy.
Homogeneous Catalysis: The catalysis in which the catalyst and the reactants are present in the same phase.
Heterogeneous Catalysis: The catalysis in which the catalyst and the reactants are present in different phases.
Kinetic Modeling: The process of developing mathematical models to describe the behavior of a chemical reaction system.