Component
Faculty of Science
Description
Use the basic principles of equilibrium thermodynamics to predict whether a reaction is possible, in which direction it is spontaneous and determine the proportions of reactants at equilibrium from the equilibrium constant. Application to homogeneous and heterogeneous equilibria, and to the special case of precipitation reactions.(acid-base and redox reactions, time permitting). Hours: 19.5 h.
In the second part, we'll look at kinetics and reaction rates. Only simple reaction orders will be studied this year. Hours: 7.5 h .
Objectives
Use thermodynamic data (enthalpy, entropy, heat capacity, etc.) to determine, in the case 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 various reactants. Know the influence of the parameters temperature, pressure and composition on a chemical equilibrium and be able to use them to shift this equilibrium in a given direction. Calculate the pH of acidic or basic solutions and mixtures. Interpret and/or calculate changes in the pH of a solution during titration.
Calculate a simple chemical reaction rate and identify the factors influencing 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.
Necessary prerequisites
A thermodynamics module is a prerequisite. It is essential to know the vocabulary and be able to use the first two principles of thermodynamics.
Mathematics at final year level, with particular emphasis on the use of derivatives and integrals.