On completion of this subject the student should be able to:
1. Identify the concepts of chemical calculations and fundamental applications of chemistry;
2. Explain the manipulation of thermodynamic relationships;
3. Explain the effect of experimental conditions on equilibrium constants;
4. Acquaint with analysing kinetic data and relate it to reaction mechanism;
5. Explain the complementary nature of thermodynamics and kinetics.
Thermodynamics: introduction, importance and limitations, energy changes in relation to work and heat changes, heat capacity of a system and second law of thermodynamics, the concept of entropy and its physical significance, Gibbs free energy, spontaneity of chemical reactions, standard and non-standard conditions, relation between Gibbs free energy change and equilibrium constant, chemical equilibrium and equilibrium constant calculations, Le Châtelier’s principle, examples with effect of concentration, temperature and pressure, acid base equilibria, weak acids and weak bases, buffer solutions, amphiprotic species and solubility equilibrium, chemical (reaction) kinetics, order of a reaction; Reaction rates: first order and second order rate equations, half-life period, mechanisms of complex reactions, rate determining step and concept of activation energy, Arrhenius equation and catalysis.
Atkins, P. W., De Paula, Julio, Elements of physical chemistry, W.H. Freeman, New York, USA, 2005.
Continuous assessment 40%
Written examination 60% (1×2 hrs.)
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