Mediaspace scheduled maintenance: Aug 25, 2026 07:00 - 12:00 AM. During this time, videos will be temporarily unavailable. Check status updates.

Lecture

Reaction Kinetics: Complementary Calculations

Description

This lecture covers reaction kinetics for equilibrium reactions, significant values for Michaelis-Menten, and the Lineweaver-Burk linearization method. The slides provide detailed equations and calculations for reaction rates, equilibrium constants, and enzyme kinetics.

Instructor

Samuel Terrettaz

Official source

Related concepts (22)

Equilibrium constant

The equilibrium constant of a chemical reaction is the value of its reaction quotient at chemical equilibrium, a state approached by a dynamic chemical system after sufficient time has elapsed at which its composition has no measurable tendency towards further change. For a given set of reaction conditions, the equilibrium constant is independent of the initial analytical concentrations of the reactant and product species in the mixture.

Chemical equilibrium

In a chemical reaction, chemical equilibrium is the state in which both the reactants and products are present in concentrations which have no further tendency to change with time, so that there is no observable change in the properties of the system. This state results when the forward reaction proceeds at the same rate as the reverse reaction. The reaction rates of the forward and backward reactions are generally not zero, but they are equal. Thus, there are no net changes in the concentrations of the reactants and products.

Dynamic equilibrium

In chemistry, a dynamic equilibrium exists once a reversible reaction occurs. Substances transition between the reactants and products at equal rates, meaning there is no net change. Reactants and products are formed at such a rate that the concentration of neither changes. It is a particular example of a system in a steady state. In physics, concerning thermodynamics, a closed system is in thermodynamic equilibrium when reactions occur at such rates that the composition of the mixture does not change with time.

Chemical reaction

A chemical reaction is a process that leads to the chemical transformation of one set of chemical substances to another. Classically, chemical reactions encompass changes that only involve the positions of electrons in the forming and breaking of chemical bonds between atoms, with no change to the nuclei (no change to the elements present), and can often be described by a chemical equation. Nuclear chemistry is a sub-discipline of chemistry that involves the chemical reactions of unstable and radioactive elements where both electronic and nuclear changes can occur.

Reaction rate

The reaction rate or rate of reaction is the speed at which a chemical reaction takes place, defined as proportional to the increase in the concentration of a product per unit time and to the decrease in the concentration of a reactant per unit time. Reaction rates can vary dramatically. For example, the oxidative rusting of iron under Earth's atmosphere is a slow reaction that can take many years, but the combustion of cellulose in a fire is a reaction that takes place in fractions of a second.

Related lectures (32)

Chemical Equilibrium: Principles and Applications

Explores chemical equilibrium principles, including Le Châtelier's Principle and equilibrium constants, and discusses the influence of temperature, pressure, and concentration on equilibrium shifts.

Kinetics: Reaction Rates and Equilibrium

Explores reaction kinetics, rate laws, measurement techniques, and binding kinetics between ligands and proteins.

Second Law of Thermodynamics

Explores the Second Law of Thermodynamics, Gibbs Free Energy, equilibrium constants, and Le Châtelier's Principle.

Chemical Equilibrium: Reaction Mechanisms

Delves into chemical equilibrium, equilibrium concentrations, reaction mechanisms, and concentration sketches in consecutive reactions.

Chemical Reactions: Batch Reactor Analysis