Lecture

Temperature Influence on Equilibrium Constant

Graph Chat

Chat with Graph Search

Ask any question about EPFL courses, lectures, exercises, research, news, etc. or try the example questions below.

DISCLAIMER: The Graph Chatbot is not programmed to provide explicit or categorical answers to your questions. Rather, it transforms your questions into API requests that are distributed across the various IT services officially administered by EPFL. Its purpose is solely to collect and recommend relevant references to content that you can explore to help you answer your questions.

Description

This lecture discusses the influence of temperature on the equilibrium constant of a chemical reaction, focusing on the reaction of fumarate in the presence of water in equilibrium with malate. By analyzing the qualitative interpretation and answering whether the reaction is endothermic or exothermic, the instructor explains the relationship between temperature, equilibrium constant, and enthalpy. Through the application of the Le Chatelier's principle and the van 't Hoff equation, the lecture demonstrates how to determine the change in free enthalpy at different temperatures and calculate the equilibrium constant. The instructor also illustrates how to extract the enthalpy change from experimental data and use it to predict the direction and nature of the reaction.

Official source

Related concepts (21)

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 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.

Chemical kinetics

Chemical kinetics, also known as reaction kinetics, is the branch of physical chemistry that is concerned with understanding the rates of chemical reactions. It is different from chemical thermodynamics, which deals with the direction in which a reaction occurs but in itself tells nothing about its rate. Chemical kinetics includes investigations of how experimental conditions influence the speed of a chemical reaction and yield information about the reaction's mechanism and transition states, as well as the construction of mathematical models that also can describe the characteristics of a chemical reaction.

Reaction mechanism

In chemistry, a reaction mechanism is the step by step sequence of elementary reactions by which overall chemical reaction occurs. A chemical mechanism is a theoretical conjecture that tries to describe in detail what takes place at each stage of an overall chemical reaction. The detailed steps of a reaction are not observable in most cases. The conjectured mechanism is chosen because it is thermodynamically feasible and has experimental support in isolated intermediates (see next section) or other quantitative and qualitative characteristics of the reaction.

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.

Related lectures (64)

Second Law of Thermodynamics

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

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.

Chemical Equilibria and Reactivity

Explores chemical equilibria, standard enthalpy changes, and osmotic pressure applications in determining molecular masses.

Chemical Reaction Engineering: Rate Laws

Explores rate laws in chemical reactions, including reaction orders, equilibrium constants, stoichiometry, and energy barriers.

Chemical Thermodynamics: Entropy and Gibbs Energy