Physical Chemistry

• reproduce the 3 laws of thermodynamics and distinguish between intensive and extensive properties and between state functions and functions that depend on the path.
• determine the compression factor of a real gas.
• calculate energy transfer as heat and work and the change in internal energy, enthalpy, entropy, Gibbs and Helmholtz free energies for processes.
• calculate standard reaction enthalpy, entropy, Gibbs free energy and equilibrium constants at different temperatures.
• account for and apply equilibrium conditions and spontaneity requirements.
• predict qualitatively the change in equilibrium by a change in pressure or temperature.
• formulate the expression for the chemical potential for pure or mixture gasses, pure liquids and solid phases, and ions in solution, and use these in equilibrium calculations.
• sketch and apply pT-, and pV-diagrams for pure substances and pV- and TS-diagrams for processes.
• calculate the ionic strength and apply it for the determination of mean activity coefficients and equilibrium concentrations, using both models and experimental data.
• derive the cell reaction for an electrochemical cell in which the electrode and electrolyte may be in direct contact and calculate the electromotive force.

The laws of thermodynamics. Internal energy, enthalpy, work, heat, entropy, Gibbs free energy, and chemical potential. Phase equilibrium and chemical equilibrium. Activities of ions. Determination of thermodynamic equilibrium constants. Equilibrium electrochemistry.

26171, The course requires knowledge of general chemistry

Classroom lectures