First law of thermodynamics- statement, definition of internal energy and enthalpy, concept of heat and work, calculation of q, W, U and H for reversible and irreversible processes and free expansion of gases (ideal and van der Waals) under isothermal and adiabatic conditions, heat capacity, heat capacities at constant volume and pressure and their relationship, Joule- Thomson effect, Joule-Thomson coefficient for an ideal gas & real gas, inversion temperature.
Self Study: An overview of thermodynamic terms, intensive and extensive properties, state and path functions and their differentials, thermodynamic processes.

Standard state, standard enthalpy of formation, enthalpy of combustion, enthalpy of neutralization, heat of reactions at constant pressure and at constant volume, Hess’s law of constant heat summation and its applications, bond energy, bond dissociation energy and its calculation from thermo-chemical data, Kirchhoff’s equation.

Second law of thermodynamics- need for the law, different statements of the law, Carnot cycle and its efficiency, Carnot theorem, thermodynamic scale of temperature.
Concept of entropy- entropy as a state function, entropy as a function of V & T, entropy as a function of P & T, entropy change in physical processes.
Third law of thermodynamics- Nernst heat theorem, statement and concept of residual entropy, evaluation of absolute entropy from heat capacity data.

Gibbs and Helmholtz functions, Gibbs function (G) and Helmholtz function (A) as thermodynamic quantities, A and G as criteria for thermodynamic equilibrium and spontaneity, their advantages over entropy change, variation of G and A with pressure, volume and temperature.
Equilibrium constant and free energy, thermodynamic derivation of law of mass action. Le Chatelier’s principle, reaction isotherm and reaction isochore, Clapeyron equation, Clausius-Clapeyron equation and its applications.

Introduction to phase, components and degree of freedom, derivation of Gibbs phase rule, phase equilibria of one component system-water, CO₂ and sulphur system.
Phase equilibria of two-component system- simple eutectic – Bi-Cd and Pb-Ag systems, desilverisation of lead.
Solid solutions- compound formation with congruent melting point (Mg-Zn), (FeCl₃ – H₂O) and incongruent melting point (NaCl-H₂O) and (CuSO₄ – H₂O) system, freezing mixtures (acetone – dry ice).