Third Thermodynamics Course of 10 days at ChEPS-KMUTT

This time there were 31 participants, more every year. Again it was a great class, thank you all (especially the tutors) for your motivation and hard work and the dinner invitation! It was an honor to teach you.

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Topics of students presentations this time were:

  1. Temperature and pressure dependence of processes and equilibria.
  2. Derive an expression for the Joule-Thomson inversion temperature from the SRK equation of state.
  3. Explain the Lee-Kessler EOS and its extension to mixtures (Plöcker). Give a calculation example.
  4. IAWPS-95 Reference equation for water and steam. Describe the equation and how to calculate the various properties from it.
  5. Calculate the enthalpy of nitrogen and methane at 100 °C between 0 and 500 bar from the SRK-equation using Mathcad and Aspen.
  6. Measurement of pure component vapor pressures.
  7. Derive the activity coefficient from the expression gE/RT = A x1­ x2.
  8. Explain the idea of NRTL-SAC and how to calculate the VLE of a binary mixture.
  9. Explain the Flory-Huggins model and calculate the activity coefficients of the components in a monomer -polymer mixture (molar volumes 70 and 70000 cm3/mol, χ = 0). What is the physical meaning of activity coefficients < 1 in this case?
  10. Verify gE-model BIPs using the DDB.
  11. Experimental determination of activity coefficients at infinite dilution using gas-liquid chromatography.
  12. Chemical theory for vapor dimerization.
  13. Explain the experimental determination of VLE from static and dynamic methods.
  14. The mixture ethanol – benzene shows a Bancroft point. Using experimental activity coefficients from the Dortmund Data Bank, show the temperature range in which the mixture is azeotropic.
  15. Explain the dependence of the K-factor for liquid-liquid extraction in the system water – acetic acid – benzene. Predict the separation factor using UNIFAC in Aspen Plus and discuss the result.
  16. At 60°C, the mixture 1-butanol – water shows a miscibility gap between 1.62 and 44.2 mol% of 1-butanol. Find the binary interaction parameters for the NRTL model from these data points using a non-randomness parameter of 0.2.
  17. Analyze the hydrocarbon solubility in water with respect to the molecular surface.
  18. Explain the absorption of CO­­2 from a biogas stream using an aqueous monoethanolamine solution and how to calculate the gas scrubbing column in Aspen.
  19. Can the pointing factor predict the increase of gas solubility at higher pressures?
  20. Derive an expression for the Henry coefficient from the SRK equation of state.
  21. Explain how to find the eutectic point of the mixture benzene – p-xylene in Aspen Plus.
  22. Calculate the solubility of sucrose in water with and without taking into account the difference between solid and liquid heat capacity (Peres, Macedo 1996).
  23. Calculate the VLE of the mixture CO2 – methane at -20°C.
  24. Explain the acetic acid/sodium acetate buffer solution. What is it good for? Demonstrate the change of PH when adding NaOH or HCl solutions.
  25. Explain in detail how to calculate the activity coefficient in the mixture ethanol – water at 70 °C and x1 = 0.252 using original UNIFAC.
  26. Explain the QVF-process for acetic acid recovery from dilute solutions using residual curve plot and balance lines.
  27. Describe the influence of the boiling point and polarity of the entrainer on the azeotropic distillation of the mixture water – pyridine. Which solvents are used in industrial processes?
  28. Explain the Gibbs minimization method used in the Gibbs reactor unit operation.
  29. At low temperature and sufficiently high pressure, propane and water form a gas-hydrate with 17 water molecules for each propane molecule. Calculate the Gibbs energy and enthalpy of formation of the hydrate using data for the hydrate formation equilibrium.
  30. Explain the process of forward osmosis desalination with ammonium bicarbonate.
  31. Describe the sulphur-iodine cycle for hydrogen production.

 

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