Thermodynamics and kinetics

Use of basic principles in equilibrium thermodynamics to predict whether a reaction is possible, in which direction it is spontaneous, and to determine the proportions of reactants at equilibrium based on the equilibrium constant. Application to homogeneous and heterogeneous equilibria and to specific cases of precipitation reactions (acid-base and redox reactions if time permits). Number of hours: 19.5.

In the second part, we will address kinetic aspects and therefore reaction speed. Only simple reaction orders will be studied during this year. Number of hours: 7.5.

Use thermodynamic data (enthalpy, entropy, heat capacity, etc.) to determine, in cases of homogeneous and heterogeneous equilibria, the direction of spontaneous evolution of a chemical reaction, to calculate the equilibrium constant of this chemical reaction, and to predict the quantities or proportions of the different reactants. Understanding the influence of temperature, pressure, and composition parameters on chemical equilibrium and being able to use them to shift this equilibrium in a given direction. Calculating the pH of acidic or basic solutions and mixtures. Interpreting and/or calculating the change in pH of a solution during titration.

Be able to calculate a simple chemical reaction rate and identify the factors that influence it.

Determine the direction of spontaneous evolution of a chemical reaction, calculate the equilibrium constant, determine the quantities of reactants at equilibrium and the rate at which they will appear in the medium.

It is necessary to have previously completed a thermodynamics module. It is essential to be familiar with the vocabulary and know how to use the first two principles of thermodynamics.

High school mathematics, with a particular focus on knowing how to use derivatives and common integrals.