THERMODYNAMICS
1.1 Types of System (open, closed, isolated)
1.2 First Law of Thermodynamics
1.2.1 Internal energy, work (pressure-volume) and heat
1.2.2 Specific heat and Heat capacity
1.2.3 Concept of Enthalpy
1.2.4 Effect of temperature on enthalpy
1.2.5 Reversible and irreversible processes
1.2.6 Types of thermal process (isothermal, isobaric, isochoric, adiabatic)
1.3 Second Law of Thermodynamics
1.3.1 Entropy change and spontaneity of a reaction
1.3.2 Gibbs free energy

THERMOCHEMISTRY
2.1 Exothermic and endothermic reactions
2.2 Enthalpy change
2.2.1 Enthalpy of formation
2.2.2 Enthalpy of reaction
2.2.3 Enthalpy of combustion
2.3 Determination of enthalpy change of reaction
2.3.1 Using standard enthalpy of formation
2.3.2 Calorimetry (Simple calorimeter and bomb calorimeter)
2.3.3 Hess’s Law and calculations

IONIC EQUILIBRIUM
3.1 Definitions of acid and base by Arrhenius, Bronsted- Lowry and Lewis
3.1.1 Types of acids & bases
3.1.2 Acid-Base Conjugate pairs
3.2 Calculation of pH and pOH (monoprotic, diprotic & triprotic acid and base)
3.2.1 Definitions of pH, pOH, Kw, pKw, Ka, Kb, pKa and pKb
3.2.2 Strong acids and bases
3.2.2 Equilibria in solutions of weak acids and bases
3.2.3 Degree of dissociation (percent ionization)
3.3 Hydrolysis reaction
3.3.1 Methods producing salt
3.3.2 Acidic, basic and neutral salt solutions
3.3.3 Salt hydrolysis. Calculation of pH/pOH values
3.3.3 Salt hydrolysis. Calculation of pH/pOH values
3.4 Buffer System
3.4.1 Acidic Buffer
3.4.2 Basic Buffer
3.4.3 Simple calculation of pH/pOH of buffer solution

ELECTROCHEMISTRY
4.1 Types of electrochemical cell (Galvanic & Electrolytic)
4.2 Half-reactions and electrodes
4.2.1 Redox reaction
4.2.2 Calculation of standard cell potential, E°cell by Standard Reduction Potential (SRP)(only principle of measurement
is required)
4.2.3 Symbolic representation of a cell (Cell Notation)
4.2.4 Predicting spontaneity of redox reactions
4.2.5 The Nernst equation
4.2.6 Concentration cells
4.2.7 Factors affecting the redox potential
4.3 Electrolysis
4.3.1 Factors affecting electrolysis and Electrochemical series
4.3.2 Faraday’s law and quantitative aspects of electrolysis
4.3.3 Applications of electrolysis (electrorefining, electroplating, manufacturing of
chlorine gas, sodium hydroxide and hydrogen from electrolysis of brine)

CHEMICAL KINETICS
5.1 Rates of reaction
5.1.1 Definition and units
5.1.2 Determination of rates of reaction
5.2 Factors affecting rates of reaction
5.2.1 Collision Theory
5.3 Rate Law and order of reaction
5.3.1 Rate law for Zero, First and Second order of reactions
5.4 Methods to determine order of reactions
5.4.1 Initial rate
5.4.2 Integrated rate law
5.4.3 Half life
5.5 Relationship between rate and temperature
5.5.1 Arrhenius equation
5.5.2 Determination of activation energy using Arrhenius equation by graphical method
and calculation
5.6 Reaction mechanism
5.6.1 Definition: Reaction mechanism, Elementary steps, Molecularity, Rate-determining
step
5.6.2 Relationship between rate law and reaction mechanism
5.6.2.1 A mechanism with a slow step followed by fast step
5.6.2.2 A mechanism with a fast reversible step followed by a slow step
5.7 Catalytic kinetics
5.7.1 Homogeneous and heterogeneous catalysis
5.7.2 Enzyme catalysis

PHASE EQUILIBRIUM
6.1 Definitions & concepts
6.1.1 Phases
6.1.2 Components
6.1.3 Gibbs Phase rule: Degree of Freedom
6.2 One-component system
6.2.1 Phase diagram of water system
6.2.2 Phase diagram CO2 system
6.3 Two-component system
6.3.1 Ideal mixture vs Non-ideal Mixture
6.3.2 Raoult’s Law
6.3.3 Vapour Pressure Lowering: The effect of non-volatile solute on vapour pressure of
solvent, melting and boiling point
6.3.4 Two completely miscible liquids- ideal, positive and negative deviation from
Raoult’s Law
6.3.5 Vapour pressure-composition diagram versus boiling point-composition
diagram for ideal, negative and positive deviation of solutions
6.3.6 Fractional distillation and azeotropic system
6.3.7 Two completely miscible solids – eutectic system and cooling curves
6.4 Colligative properties
6.4.1 Boiling point elevation
6.4.2 Freezing point depression

COLLOID AND SURFACE CHEMISTRY
7.1 Definitions of colloid, true solution and suspension system
7.2 Types of colloid and uses
7.3 Lyophilic and lyophobic sols
7.3.1 Stability of lyophobic sols
7.3.2 Preparation of lyophilic and lyophobic sols (dispersion and condensation methods)
7.3.3 Properties of colloids – Brownian, dialysis, Tyndall effect, electric double layer,
electrophoresis, electro-osmosis & coagulation
7.4 Adsorption
7.4.1 Adsorption phenomenon
7.4.2 Types of adsorption (Differences between chemical adsorption and physical adsorption)
7.4.3 Types of adsorption isotherm (introductory and without calculation)
– Langmuir and Freundlich
– Brunauer-Emmett-Teller (B.E.T)

Q1 : What is Physical Chemistry?
A1 : Physical chemistry is the study of how matter behaves on a molecular and atomic level and how chemical reactions occur. Based on their analyses, physical chemists may develop new theories, such as how complex structures are formed.

Q2 : What is this course about?
A2 : This course deals with selected topics in physical chemistry such as thermodynamics, thermochemistry, ionic equilibrium, electrochemistry, chemical kinetics, phase equilibrium, as well as colloid and surface chemistry.

Q3 : Who can enroll this course?
A3 : Anyone.