Course Syllabus
Thermochemistry
1.1 Exothermic and endothermic reactions. Energy profile for the two types of reactions
1.2 Explanation of activation energies for reversible and nonreversible reactions
1.3 Enthalpy and enthalpy change
1.4 Calorimetry, Heat capacity and spescific heat
1.5 Defination of heat of reactions. Calculations of heat of reaction from standard heat of formation
1.6 Hess''s Law and Calculation
Thermodynamics
2.1 relationship between temperature and equilibrium in reversible and non reversible processes
2.2 explanation of 1st, 2nd and 3rd law of thermodynamics
2.3 First law: work and heat, enthalpy (qp and qv) Cv and Cp, effect of temperature on enthalpy, ideal gas system, explanation of isothermal, adiabatic, reversible and irreversible processes
2.4 Second law : Spontaneous reaction, entropy change (ideal gas, liquid, solid and changing phase), dependance of entropy on variables in a system (variables T and V, variables T and P)
2.5 Third law : explanation of absolute entropy, spontaneity, basic equations for closed system, Gibbs absolute entropy on T and P
Electrochemistry
3.1 Electrode potential and electrochemical cell
3.1.1 Electrode potential and activity (Nerst equation)
3.1.2 Electrochemical cell and cell reaction
3.1.3 Standard hydrogen electrode
3.1.4 Measurement of EMF and sign determination
3.2 Uses of electrode potential and cell EMF; pH determination, selective ionic electrode, potentiometry an determination of equilibrium constant
3.3 Electrode processes, electrolysis and corrosion
Lab 2 : Electrochemistry : Electrochemical cell
Chemical Kinetic
4.1 Rates of reaction. Defination and units
4.2 Factors affecting rates of reaction, reaction rate and stoichiometry
4.3 Concentration and rate
4.3.1 Rate law and overall reaction order
4.3.2 Using initial rates to determine rate laws
4.4 Change of concentration with time
4.4.1 First Order and Second Order reactions
4.4.2 Half-life
4.5 Arrhenius equation
4.6 Reaction mechanism
4.6.1Elementary reactions and their Rate laws uni, bi and termolecular
4.6.2 Rate-determining step for a multi-step mechanism
4.7 Catalytic kinetics: homogeneous, enzyme and heterogeneous catalysis
Lab 3: Chemical kinetic : Factor affecting rates of reaction
Lab 4: Chemical kinetic : Order of reaction
Phase Equilibrium
5.1 One component system: ice-water vapor system and CO2system
5.2 Use of Roult''s law in explaining the effect of nonvolatile solute on vapor pressure of solvent and its melting and boiling points
5.3 Boiling point-composition phase diagram for two component system
5.3.1 Two completely miscible solids - eutectic mixture
5.3.2 Two completely miscible liquids - ideal,positive and negative deviations from Raoult''s law
5.3.3 Azeotropic system and fractional distillation
Lab 5: Phase equilibrium : Solid-liquid phase diagram-Eutectic system
Colloid and Surface Chemistry
6.1 Colloid
6.1.1 Definition. Differences between colloid, true solution and heterogeneous system. Characteristics of each system
6.1.2 types of colloid based on the dispersion medium and dispersed phase and examples. Gel, paste and emulsion
6.1.3 Methods and preparation
6.1.4 Lyophilic and lyophobic colloid. Stability of lyophobic colloid
6.2 Adsorption
6.2.1 Adsorption phenomenon
6.2.2 Single layer and multilayer adsorptions
Lab 6: Colloid : Property of colloidal dispersion
Lab 7: Surface chemistry : Adsorption at a solid surface
1.1 Exothermic and endothermic reactions. Energy profile for the two types of reactions
1.2 Explanation of activation energies for reversible and nonreversible reactions
1.3 Enthalpy and enthalpy change
1.4 Calorimetry, Heat capacity and spescific heat
1.5 Defination of heat of reactions. Calculations of heat of reaction from standard heat of formation
1.6 Hess''s Law and Calculation
Thermodynamics
2.1 relationship between temperature and equilibrium in reversible and non reversible processes
2.2 explanation of 1st, 2nd and 3rd law of thermodynamics
2.3 First law: work and heat, enthalpy (qp and qv) Cv and Cp, effect of temperature on enthalpy, ideal gas system, explanation of isothermal, adiabatic, reversible and irreversible processes
2.4 Second law : Spontaneous reaction, entropy change (ideal gas, liquid, solid and changing phase), dependance of entropy on variables in a system (variables T and V, variables T and P)
2.5 Third law : explanation of absolute entropy, spontaneity, basic equations for closed system, Gibbs absolute entropy on T and P
Electrochemistry
3.1 Electrode potential and electrochemical cell
3.1.1 Electrode potential and activity (Nerst equation)
3.1.2 Electrochemical cell and cell reaction
3.1.3 Standard hydrogen electrode
3.1.4 Measurement of EMF and sign determination
3.2 Uses of electrode potential and cell EMF; pH determination, selective ionic electrode, potentiometry an determination of equilibrium constant
3.3 Electrode processes, electrolysis and corrosion
Lab 2 : Electrochemistry : Electrochemical cell
Chemical Kinetic
4.1 Rates of reaction. Defination and units
4.2 Factors affecting rates of reaction, reaction rate and stoichiometry
4.3 Concentration and rate
4.3.1 Rate law and overall reaction order
4.3.2 Using initial rates to determine rate laws
4.4 Change of concentration with time
4.4.1 First Order and Second Order reactions
4.4.2 Half-life
4.5 Arrhenius equation
4.6 Reaction mechanism
4.6.1Elementary reactions and their Rate laws uni, bi and termolecular
4.6.2 Rate-determining step for a multi-step mechanism
4.7 Catalytic kinetics: homogeneous, enzyme and heterogeneous catalysis
Lab 3: Chemical kinetic : Factor affecting rates of reaction
Lab 4: Chemical kinetic : Order of reaction
Phase Equilibrium
5.1 One component system: ice-water vapor system and CO2system
5.2 Use of Roult''s law in explaining the effect of nonvolatile solute on vapor pressure of solvent and its melting and boiling points
5.3 Boiling point-composition phase diagram for two component system
5.3.1 Two completely miscible solids - eutectic mixture
5.3.2 Two completely miscible liquids - ideal,positive and negative deviations from Raoult''s law
5.3.3 Azeotropic system and fractional distillation
Lab 5: Phase equilibrium : Solid-liquid phase diagram-Eutectic system
Colloid and Surface Chemistry
6.1 Colloid
6.1.1 Definition. Differences between colloid, true solution and heterogeneous system. Characteristics of each system
6.1.2 types of colloid based on the dispersion medium and dispersed phase and examples. Gel, paste and emulsion
6.1.3 Methods and preparation
6.1.4 Lyophilic and lyophobic colloid. Stability of lyophobic colloid
6.2 Adsorption
6.2.1 Adsorption phenomenon
6.2.2 Single layer and multilayer adsorptions
Lab 6: Colloid : Property of colloidal dispersion
Lab 7: Surface chemistry : Adsorption at a solid surface
Frequently Asked Questions
Q1 : What is the suitable references for this mooc?
A1 : I would recommend these references: 1) General Chemistry 2) Physical Chemistry
A1 : I would recommend these references: 1) General Chemistry 2) Physical Chemistry