1. Supercritical Fluid Extraction

2. Intermolecular Forces Dipole-Dipole Interactions Dipole-Dipole Interactions London Dispersion Forces London Dispersion Forces Hydrogen Bonding Hydrogen Bonding

3. Dipole-Dipole Interactions Some molecules have an uneven distribution of charge; these are called polar molecules. Some molecules have an uneven distribution of charge; these are called polar molecules. Polar molecules attract one another when the partial positive charge on one molecule is near the partial negative charge on another molecule Polar molecules attract one another when the partial positive charge on one molecule is near the partial negative charge on another molecule

4. London Dispersion Forces Instantaneous uneven electron distributions in a molecule can cause induced dipole-dipole effects called London Dispersion Forces. Instantaneous uneven electron distributions in a molecule can cause induced dipole-dipole effects called London Dispersion Forces.

5. Hydrogen Bonding By far the strongest intermolecular force By far the strongest intermolecular force A hydrogen atom in a polar bond can experience in attractive force with a neighboring Electronegative atom. A hydrogen atom in a polar bond can experience in attractive force with a neighboring Electronegative atom. This is especially applicable when a Hydrogen atom and highly electronegative atom are bonded in a molecule; one of the most polar bonds known. This is especially applicable when a Hydrogen atom and highly electronegative atom are bonded in a molecule; one of the most polar bonds known.

6. Energy of Solvation The energy of forces between the molecules of the solute are in contest with the energy of forces between molecules of solute and solvent. The energy of forces between the molecules of the solute are in contest with the energy of forces between molecules of solute and solvent. Also added to the Energy of solvation is the energy needed to make a cavity in the solvent for each solute molecule to be surrounded. Also added to the Energy of solvation is the energy needed to make a cavity in the solvent for each solute molecule to be surrounded.

7. Carbon Dioxide Carbon Dioxide is used in Supercritical fluid studies because it’s critical point is in an easily reached range. Carbon Dioxide is used in Supercritical fluid studies because it’s critical point is in an easily reached range. At its normal Gaseous state Carbon Dioxide is an extremely bad solvent, but as a liquid it has much better solvent capabilities. At its normal Gaseous state Carbon Dioxide is an extremely bad solvent, but as a liquid it has much better solvent capabilities.

8. Phase Diagram

9. Supercritical Fluid Both Gas and liquid phases have the same densities in this range. Both Gas and liquid phases have the same densities in this range. Carbon Dioxide is normally used since it’s critical point is at 73.8 bar and 31.1 degree Celsius, a very easily reached condition Carbon Dioxide is normally used since it’s critical point is at 73.8 bar and 31.1 degree Celsius, a very easily reached condition Two Separate phases of Carbon Dioxide One Supercritical Phase Of Carbon Dioxide

10. Uses Decaffeinating coffee as well as Sewage Treatment. Decaffeinating coffee as well as Sewage Treatment. Control over Density, and Solvation. Control over Density, and Solvation. Differentiates between enantiomers, paramount in producing medicines. Differentiates between enantiomers, paramount in producing medicines.

11. Experiment Purpose Show proof that a tailor made molecule could be made to enhance extraction. Show proof that a tailor made molecule could be made to enhance extraction. Solves the problem of low extraction results that plagues CO2 extraction. Solves the problem of low extraction results that plagues CO2 extraction.

12. Experiment Setup Uses a CO2 extraction device made in the lab to run super critical CO2 through a powder. Uses a CO2 extraction device made in the lab to run super critical CO2 through a powder. After the CO2 is bubbled through Methanol and this solution is run in a HPLC to discover the contents. After the CO2 is bubbled through Methanol and this solution is run in a HPLC to discover the contents. Different mixtures of chemicals are extracted to see how the chemicals affect each other’s solvation. Different mixtures of chemicals are extracted to see how the chemicals affect each other’s solvation.

13. Results Certain interactions cause a decent increase in product: Certain interactions cause a decent increase in product: Pi-Pi benzene ring interaction Pi-Pi benzene ring interaction Hydrogen bonding between the molecules Hydrogen bonding between the molecules Why? Why?

14. THE END Any Questions?