1.1 Exothermic and endothermic reaction.
1.1.1 Energy profile.
1.1.2 Activation energy for reversible and non-reversible reactions.
1.2 Enthalpy and enthalpy change.
1.2.1 Definitions of heats of reaction, enthalpy of combustion and enthalpy of
formation.
1.2.2 Calculation of heats of reaction using standard enthalpy of formation.
1.3 Calorimetry.
1.3.1 Heat capacity and specific heat.
1.3.2 Simple calorimeter and bomb calorimeter.
1.3.3 Calculation of enthalpy of combustion.
1.4 Hess’s law.
1.4.1 Definition and calculation.

2.1 Rates of reaction.
2.1.1 Definition and units.
2.1.2 Determination of rates of reaction.
2.2 Factors affecting rate of reaction.
2.2.1 Collision Theory.
2.2.2 Transition state.
2.3 Rate law and order of reaction.
2.3.1 Rate law for zero, first, second order.
2.3.2 Rate law for reactions higher than second order.
2.3.3 Rate law for fractional order.
2.4 Methods to determine order of reactions.
2.4.1 Initial rate.
2.4.2 Integration.
2.4.3 Half-life.
2.5 Relation between rate and temperature.
2.5.1 Arrhenius equation.
2.5.2 Determination of activation energy by graphical method or calculation using Arrhenius equation.
2.6 Reaction mechanism.
2.6.1 Basic processes – molecularity.
2.6.2 Reversible, series and parallel reactions.
2.6.3 Relationship between rate law and reaction mechanism.
2.7 Catalytic kinetics.
2.7.1 Homogeneous and heterogeneous catalysis.
2.7.2 Acid-base catalysis.
2.7.3 Enzyme catalysis.

3.1 Definition.
3.1.1 Phases.
3.1.2 Components.
3.1.3 Phase rule: Degree of Freedom.
3.2 One component system.
3.2.1 Phase diagram of ice-water-vapour system.
3.2.2 Phase diagram of CO2 system.
3.3 Two components system.
3.3.1 Raoult’s law – effect of volatile and non-volatile solute on vapour
pressure (colligative properties).
3.3.2 Two completely miscible liquids – ideal, positive and negative deviation from Raoult’s law.
3.3.3 Vapour-pressure composition diagram vs boiling point-composition diagram.
3.3.4 Fractional distillation and azeotropic system.
3.3.5 Two completely miscible solids – eutectic system and cooling curves.

4.1 Colloids.
4.1.1 Definition: Colloid, true solution and heterogeneous systems.
4.1.2 Classification of colloids: Based on physical state of dispersed phase and dispersion medium; nature of interaction
between dispersed phase and dispersion medium (Lyophilic and Lyophobic); and type of particle of dispersed phase
(Multimolecular, macromolecular and associated (micelles) colloids).
4.1.3 Lyophilic and lyophobic colloids.
4.1.4 Stability of lyophobic colloid.
4.1.5 Preparation of lyophilic and lyophobic colloid (dispersion and condensation methods).
4.1.6 Property of lyophobic colloid – Brownian, dialysis, Tyndal effect, electric double layer and coagulation.
4.2 Adsorption
4.2.1 Definition.
4.2.2 Types of adsorption: Single and multilayers.
4.2.3 Chemical and physical adsorptions.
4.2.4 Gibbs equation.
4.2.5 Isotherms: Freundlich, Langmuir and BET adsorption isotherms.

A1 : Yes, you must have a basic chemistry background to enroll this course.

A2 : There are 4 topics namely thermochemistry, chemical kinetics, phase equilibrium, colloid and surface chemistry.