“chemical engineering”

Assistant proffesor Sarma Valtere

Course description: 4Credit units; 64 hours lectures, 48 hours laboratories

Control forms: Test
Course content:

• 
  General principles of the environmental chemistry. Principles of the environmental toxicology.
  
• 
  Characteristics of the biogenic chemical elements, micro- and macroelements.
  
• 
  Chemical and physico-chemical processes in diferent spheres. The living processes and the bio-geo-chemical cycles.
  
• 
  How society interacts with natural material flows - global antropogenic flows: the unbalanced carbon cycle, the increased nitrogen, phosphorus and sulphur flows.
  
• 
  The main xenobiotics: heavy metals, radionuclides, synthetic organic substances. Response to xenobiotics: chemical carcinogenesis and mutagenesis.
  
• 
  Air pollution: the main antropogenic pollutants. Photochemical chain reactions, photochemical smog. Depletion of stratospheric ozone. Climatic changes. Acidification of environment.
  
• 
  Water and land pollution. Charakteristics of natural water resources. Sources of water pollution: municipal sewage, industrial wastewaters.
  
• 
  Pollution controle: pollution prevention in the sources (cleaner technologies, alternative row materials) purification of flue gases, wastewater treatment, waste disposal and recycling, treatment of hazardous waste.
  

Literature:

1. 
   M. Klavins. Environmental Chemistry. Chemical Pollutants and their cycles (In Latvian). University of Latvia, Riga, 1996, 298 p.
   
2. 
   S. Valtere. Water chemistry (In Latvian). Riga Politechnical Institute, 1987, 66 p.
   

Further Readings:

1. 
   S.F.Zakrzewski. Principles of Environmental Toxicology. American Chemical Society, Washington, DC, 1991, 270 p.
   
2. 
   S.Karlsson, C.Azar, G.Berndes, J.Holmberg, K.Lindgren. Man and Materials Flows. The Baltic University Programme A Sustainable Baltic Region, Booklet N 3, Uppsala Publishing House, 1997, 52 p.
   

Physical Chemistry

ĶNF 686

Associated Professor Augusts Ruplis

Course description: 15Credit units; 64 hours lectures

Control forms: Test
Course content:

• 
  Introduction. What is physical chemistry. Historical background of physical chemistry. Methods of phhysical chemistry.
  
• 
  Principles of chemical themodynamics. First principle. Energy. Heat and work. Methods of thermodynamics. Equivalence of heat and work. Internal energy. Equilibrium. Application of the first law to ideal gases. Heat capacyites. Enthalpy. General application of the first law. Thermochemistry. Heats of reaction. Enthalpies of formation. Kirchoff’s law. Calorimetry. Second law of thermodynamics. The meaning and significance of the second law of thermodynamics. Permissibility and direction of spontaneous processes. Statistical nature of the second law of thermodynamics. Formulation of the second law of thermodynamics. Entropy. Irreversible processes. General relations for isolated system. Entropy and thermodynamic probability. Thermodynamic potentials. Relations between thermodynamic functions. Total differential of the thermodynamic functions. Equations of Gibbs-Helmholtz. Application of second law to ideal gases. Thermodynamics of non- ideal gases. Change of equilibrium
  
• 
  Phase and chemical equilibrium. General conditions of phase equilibrium. The Gibbs phase rule. One component systems. Equilibrium relations in phase equilibrium. The chemical potential. The law of mass action. Equilibrium constants. The equation of the isotherm of a chemical reaction. Chemical affinity. The equation of the isobar and isotherm of a chemical reaction. Chemical equilibrium in heterogeneous reactions. The Nernst heat theorem. Absolute entropies. Calculation of chemical equilibrium. Gibbs free energy of formation of chemical compounds. Indirect calculations of Gibbs energy changes and equilibrium constant. Experimental methods of determining Gibbs energy changes. Calculation of equilibrium by means of the heat of reaction and entropy. Dependence of the equilibrium constant on temperature. Calculation of chemical equilibrium using standard entropies and heats of formation of the reaction components
  
• 
  Solutions Ways of expressing the composition of solutions. Liquid solutions. Dilute solutions. Rauolt’s law. Crystallization temperature of dilute solutions. Boiling point of dilute solutions. Determination of the molecular masse of a solute. Concentrate solutions
  Saturated vapor pressure of a simple system. Saturated vapor pressure in different systems. Activity and activity coefficient. Composition of the vapor of solution. Boiling points of solutions. Distillation of binary mixtures. The lever rule. Rectification. Saturated vapor pressure of systems with limited mutual solubility of components. Solutions of gases in liquids
  
• 
  Phase equilibrium in condensed systems Mutual solubility of liquid systems. The partition law. Isothermal equilibrium in ternary systems. Extraction from solutions Diagram of state for simple system with an eutectic. Systems whose components form compounds. Systems whose components form mixed crystals ( solid solutions) in any relative amounts. Complex systems. Ternary systems. Thermal analysis
  
• 
  Electroconductance of solutions Specific Electroconductance. Measurements of Conductance of Solutions. Equivalent Conductance. Electroconductance of Strong Electrolytes. Electroconductance of Weak Electrolytes. Conductometric Titration. Ion Mobilities. Transport Numbers
  
• 
  Electrode processes and electromotive force Electromotive Force. Reversible and Irreversible Cells. Electrode Potentials and the EMF of Galvanic Cells. Types of Reversible Electrodes. Measurement of Electromotive Force. The Standard Cell. Concentration Cells and Diffusion Potentials. Oxidation-Reduction Electrodes. Thermodynamics of Galvanic Cells. Potentiometric Determination of pH and Potentiometric. Electrolysis. Polarisation. Decomposition Voltage and Overvoltage. The Electrochemical Theory of Metal Corrosion. Protection of Metals Against Corrosion
  

• 
  Chemical kinetics
  

1. Rate of a Chemical Reaction

2. Kinetic Classification of Chemical Reactions

3. First Order Reactions

5. Second Order Reactions

6. Third Order Reactions

7. Experimental Measurements of Reaction Rates

8. Determination of the Order of a Reaction

9. Molecularity of Reactions

10.Complex Reactions

11.Stady State in Complex Reactions

12.Influence of Temperature on the Reaction Rate

!3. Calculation of Reaction Rate Constants and of Activation Energies

14.Chain Reactions

15.Catalysis. Basic Principles

16.Homogeneous Catalysis

17. Heterogeneous Catalysis

18.Theories of Catalysis

19. Photochemical Reactions