1 / 39

Chemistry 231

Chemistry 231. Physical Transformations of Pure Substances. The Definition of a Phase. Phase – a region of system inside which we have uniformity of the chemical potential and physical properties. Three Principal kinds of phases Solid – long-range order Liquid – less long-range order

johana
Download Presentation

Chemistry 231

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Chemistry 231 Physical Transformations of Pure Substances

  2. The Definition of a Phase • Phase – a region of system inside which we have uniformity of the chemical potential and physical properties. • Three Principal kinds of phases • Solid – long-range order • Liquid – less long-range order • Gas – random molecular distributions

  3. Phase Transitions • A phase transition is the spontaneous conversion of one phase into another. • Distinguish between • Thermodynamic stability – based on chemical potential differences • Metastable (kinetic stability) – slow conversion of one phase into another

  4. The driving force for phase stability is the chemical potential of the substance in a particular phase The Criteria for Phase Stability

  5. The Criteria for Phase Equilibrium For two phases to be in equilibrium, the chemical potential of the substance in both phases must be equivalent.

  6. The Phase Rule • For a single component system F=3-P • F = degrees of freedom • P = number of phases • For a single component system, with two phases in equilibrium F = 3-2 = 1

  7. The Definition of Vapour Pressure PJ The pressure of the vapour above the liquid is called the vapour pressure PJ. Vapour pressures are temperature dependent.

  8. The Fundamental Equation Applied to Phase Stability • Applying the definition of the chemical potential Assume we apply an infinitesimal change in T or P to two phases in equilibrium

  9. Displacement of the Phase Equilibrium When a pressure (or temperature) change is applied to an equilibrium system of two phases (point a), the equilibrium is disturbed. It can be restored by changing the temperature (or pressure) along the boundary to point b.

  10. The Clapeyron Equation Defining the transition  The slope of any phase boundary can be obtained from the Clapeyron equation

  11. The Solid-Liquid Boundary For the fusion transition A(s)A(l) We can re-write the Clapeyron equation to include the enthalpy of fusion

  12. The Integrated Form The dependence of the melting point on the applied pressure is given as follows

  13. A Picture of the Solid Liquid Boundary From the Clapeyron equation, a typical solid-liquid phase boundary slopes steeply upwards. Most substances increase their melting points behave in this way.

  14. Condensed Phase – Vapour Transitions For the transition between a condensed phase and the vapour phase A(c)A(g) We can re-write the Clapeyron equation to include the enthalpy of the transition

  15. The Clausius-Clapeyron Equation Using the ideal gas equation Note – tr represents vapourization or sublimation.

  16. Boiling Points • The boiling point is defined as the temperature at which PJ equals Pext. • Normal Boiling Point – Pext = 1 atm. • Standard Boiling Point – Pext = 1 bar. • Boiling points are pressure dependent (see later).

  17. Critical Points Critical temperature (Tc) - the temperature above whicha gas cannot be liquefied Critical pressure (Pc) – the minimum pressure that needs to be applied at Tc to bring about liquefaction. Supercritical fluid – fluid at or above the Tc value.

  18. A Picture of the Liquid Vapour Boundary The phase boundary from the plot of the (T,P) equilibrium points. The liquid vapour phase boundary terminates at the critical point (not shown). The solid-vapour phase boundary is identical in shape.

  19. Dependence of Phase Stability on Pressure/Temperature Changes The temperature dependence of the phase stability is related to the numerical value of the molar entropy!

  20. Phase Stability with Pressure The dependence of the chemical potential with pressure depends on the volume of the phase!

  21. Classifying Phase Transitions When we classify phase transitions, we must look at the first and second derivatives of the chemical potentials

  22. The Ehrenfest Classification (I) • A first order transition • At least one of the first derivatives of the chemical potential is discontinuous at the transition point. • The second derivative of  is a singularity!

  23. The Ehrenfest Classification (II) • A second order transition • Both of the first derivatives of the chemical potential are continuous at the transition point. • One of the second derivatives of  is discontinuous!

  24. The Chemical Potential Functions At Phase Transitions The changes in thermodynamic properties for a schematic first-order transition.  Cp,m T Vm T Sm T

  25. Second Order Transitions The changes in thermodynamic properties for a schematic second-order transition. Cp,m Vm T T

  26. The Lambda Transition in Helium The fluid-superfluid transition in helium (the  transition). The heat capacity appears to become infinite (first order). It actually rises smoothly at the transition point, instead of exhibiting a singularity.

  27. Melting Points and Triple Points • Melting Point – the temperature at which the solid and the liquid phases are in equilibrium. • Normal Melting Point – melting temperature at 1 atm pressure. • Standard Melting Point – melting temperature at 1 bar pressure. • Melting Points are pressure dependent.

  28. Phase Diagrams (P,T) regions where the phases are thermodynamically stable. A phase boundary is a curve in (T,P) space where the  values of the substance in the different phases are equivalent.

  29. Triple Point p1 An invariant point where the solid, liquid, and vapour phases are in mutual equilibrium.

  30. Schematic Phase Diagrams

  31. More Complex Water Phase Diagram Water

  32. The Molecular Origin of Surface Tension • Imbalance of intermolecular forces exists at the liquid-air interface • gla= the surface tension that exists at the liquid-air interface

  33. Surface Tensions of Pure Liquids at 293 K

  34. Capillary Action • The tendency of liquids to rise up in narrow tubes - capillary action. • Due to the phenomenon of surface tension.

  35. The Complication of Contact Angles • The balance of forces that results in a contact angle, c. • The contact angle gives information on the ‘wettability’ of a surface.

  36. Capillary Rise • The pressure exerted by a column of liquid is balanced by the hydrostatic pressure. • This gives us one of the best ways to measure the surface tension of pure liquids and solutions.

  37. Meniscus Up or Down?? • For a wetting liquid, a capillary rise is observed. • For a non-wetting liquid, capillary rise is observed capillary wets the

  38. Pressure Differential Across Curved Interfaces • Pressure differential exists across curved interfaces. • Due to surface tension forces

  39. Enhancement of Vapour Pressure • Vapour pressure enhancement above the surface of spherical droplets. • Due to surface tension forces. P

More Related