To teach key principles of physical chemistry. To carry out practical work to support and reinforce some of the theoretical aspects encountered.

Thermodynamics, heat, work, reversible and irreversible systems, state functions; First law of thermodynamics, internal energy, enthalpy, standard enthalpies, second law of thermodynamics, entropy, Gibbs free energies, Chemical equilibrium; effect of temperature, pressure, concentration, Le Chateliers Principle; Ions in aqueous solution; electrochemical cells, electrolytic conductivity, Reaction kinetics: zero, first and second order reactions and enzyme kinetics-Michaelis-Menten.

Thermodynamics 1. Understand and apply the thermodynamic concepts of 'system', 'surroundings', 'universe', heat (q), work (w), internal energy (U), enthalpy (H) and entropy (S). 2. State/recall the zeroth, first, second and third law of thermodynamics as applied to chemistry. 3. Differentiate between exothermic, endothermic, exergonic and endergonic processes 4. Compute thermochemical changes in internal energy, enthalpy, entropy and Gibbs free energy from tabulated data. 5. Calculate equilibrium constants from Gibbs free energy changes. 6. Analyse experimental data for the determination of internal energy change and enthalpy change of reaction. Reaction Kinetics 1. Demonstrate awareness that reactions occur at different rates. 2. Determine the rate of reaction by experiment. 3. Demonstrate knowledge of collision theory and of the energetics of reaction 4. Analyse the reaction mechanism and relate it to the order of reaction for a reactant/product system. 5. Classify types of catalysts used in different situations (including enzymes) and develop mechanisms for catalyzed reactions. 6. Illustrate graphically the energy changes associated with catalyzed and uncatalyzed reactions. 7. Analyse experimental date for the determination of reaction orders, rate coefficients and energy of activation. Dynamic equilibrium 1. Explain the concept of chemical equilibrium with respect to reactions in gaseous and liquid phases. 2. Predict, with reference to entropy, enthalpy and free energy changes, whether reacting systems will reach equilibrium. 3. Apply Le Chateliers Principle and the concept of equilibrium to a commercial / industrial process. 4. Execute calculations of the equilibrium constant (k) if concentrations are known and of concentrations if k is known. 5. Infer conclusion for the equilibrium constant expression and value. 6. Formulate a connection between equilibrium constant and rate constants for a reversible first order system. Ions in solution 1. Identify two different models for acids and bases. 2. Classify an aqueous acid of base solution as either weaker or strong, with reference to ionic conductivity. 3. Analyse/quantify the equilibrium that exist in weak acid or weak base systems or in buffer systems. 4. Identify/label chemical species that are amphiprotic. 5. Solve/perform calculations relating pH, pOH, [H3O+] and [OH-]. 6. Define the Ka and Kb constants. 7. Describe/interpret an indicator as an equilibrium system and justify the choice of indicator for a particular acid-base system using titration curves. 8. Describe and quantify the extent of hydrolysis in salt solutions. Electrochemistry 1. Identify and draw different types of electrochemical cells - Galvanic and Electrolytic. 2. Write the cell diagrams for electrochemical cells using the electrochemical series and calculate the corresponding standard cell potential. 3. Calculate cell potentials using non-standard conditions using the Nernst Equation. 4. Calculate the mass of metal deposited during electrolysis by applying Faradays Law of electrolysis.

To grasp the importance of comprehending key concepts associated with physical chemistry rather than mere reliance on rote learning / memory work

Perform various laboratory experiments relevant to physical chemistry, e.g. the determination of enthalpy changes during chemical reactions via calorimetry; the evaluation of reaction kinetics for chemical reactions; the assembly and use of various electrochemical cells.

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