Transcript Slide 1
At sea level At top of a mountain Water boils at < 100C Water boils at 100C b.P = f(P) P = 1.0133 bar bp = 100C elevation = 8848 m P = 0.26 bar bp = 69C P = 2 atm , b.p = 124C + EG 50/50 (v/v), b.p =129.5 C => b.p = f(P, c) If I specify P, T, and c, what are the stable phases? Phase diagram stability map stability of the state of aggregation Depending on the circumstances, molecules aggregate to form solid, liquid, or gas Phase = region of a substance that is: Uniform in chemical composition physically distinct mechanically separable Examples of single-phase system ( = 1): Pure water (l) White gold (alloy of Au-Ag-Ni) => Ag and Ni substitute Au in its FCC lattice => homogeneous composition throughout => solution Air (N2, O2, Ar, CO2) Examples of dual-phase system ( = 2): Ice cubes in liquid water Milk (fat globules in aqueous solution) Equilibrium = the condition which represents the lowest energy level the properties are invariant with time Component = the measure of chemical complexity 1 2 1 Water (l) diamond Ice cube in liquid water (slush) >1 White gold (Au-Ag-Ni) CCl4 – H2O N s = l coexistence curve =2 Critical point (374C, 218 atm) P (atm) Liquid =1 l = v coexistence curve =2 1 4.58 mm Hg Solid =1 Gas =1 s=v coexistence curve =2 Triple point =3 0 0.01 100 Phase diagram of water T (C) POLYMORPHS Different atomic arrangement at constant composition B : 95,5C and 0,51 Pa C : 115C and 2,4 Pa E : 151C and 1,31108 Pa Phase diagram of sulfur The transformation from one polymorph to another can be : 1. Reversible : two crystalline forms are said to be enantiotropic 2. Irreversibel : two crystalline forms are said to be monotropic Pressure-temperature diagram for dimorphous substances: (a) enantiotropy, (b) monotropy There are tree variables that can affect the phase equilibria of a binary system: T, P, and C P P T c T Two-component phase diagram 3 dimension T-P-c 2 dimension T-P P-c Crystallization: liquid and solid The effect of P can be ignored T-c Diagram T-c Complete solubility in solid and liquid states Change of state (s = l) Metal (Hume-Rothery Rule) Similar crystal structure Similar atomic volumes Small values of electronegativity For interstitial solid solutions, the Hume-Rothery rules are: 1. Solute atoms must be smaller than the pores in the solvent lattice. 2. The solute and solvent should have similar electronegativity. For substitutional solid solutions, the Hume-Rothery rules are: 1. The atomic radii of the solute and solvent atoms must differ by no more than 15%: 2. The crystal structures of solute and solvent must match. 3. Maximum solubility occurs when the solvent and solute have the same valency. Metals with lower valency will tend to dissolve in metals with higher valency. 4. The solute and solvent should have similar electronegativity. If the electronegativity difference is too great, the metals will tend to form intermetallic compounds instead of solid solutions. T Liquid =1 A Tmp Liquidus B Tmp Liquid + solid =2 Solidus Solid =1 A c B Liquidus : l s + l : the lowest T for only liquid (at any c) Solidus : s s + l : the highest T for only solid (at any c) The diagram represents the phase behavior of two components having many similarities (type of bonding, atomic size, crystal structure, etc), we call it ISOMORPHOUS DIAGRAM. The shape of the diagram looks like a lens lens-shape diagram / lenticular diagram. Example: naphthalene - -naphthol Similar Solid solution of naphthalene - -naphthol > Solid solution of naphthalene - -naphthylamine Partial or limited solubility miscibility gap No change of state always liquid or always solid l T = 1 s l1 + l2 =2 + A c Coexistence curve B upper critical solution temperature (upper consolute temperature) Hexane - nitrobenzene lower critical solution temperature (lower consolute temperature) Partial or limited solubility Change of state EUTECTIC DIAGRAM T B Tmp Liquid solution A Tmp l =1 l+ l+ =1 Solid solution (A rich) A =2 =2 =2 c Solid solution (B rich) =1 Eutectic l B Freezing point depression of both components (A and B) Eutectic point is equilibrium of , , and l Eutectic point is unique; it only happens at one T, P, and c Phase diagram for the simple eutectic system naphthalene - benzene Phase diagram for system NaCl – H2O Solution A having composition of xA and enthalpy of HA is mixed adiabatically with solution A having composition of xB and enthalpy of HB. The composition and the enthalpy of the mixture is calculated using material balance: Total balance: mC m A m B Component balance: mC xC m A x A m B x B Combining both equations yields: m A x A mB xB xC m A mB Similarly, if mixture A were to be removed adiabatically from mixture C, the enthalpy and composition of residue B can be located on the straight line through points A and C by means of the equation: mC xC m A x A xB mC m A EXAMPLE Calculate (a) the quantity of heat to be removed and (b) the theoretical crystal yield when 5000 lb of a 30 per cent solution of MgSO4 by mass at 110F is cooled to 70F. Evaporation and radiation losses may be neglected. SOLUTION (a) Initial solution (A) Cooled system (B) Enthalpy change Heat to be removed xA = 0.3 HA = - 31 Btu/lb xB = 0.3 HB = - 75 Btu/lb H = - 44 Btu/lb = (- 44) (5000) = - 220000 Btu (b) The cooled system B is located in the region where MgSO4.7H2O is in equilibrium with solution. The crystal MgSO4.7H2O contains: Weight fraction of MgSO 4 MWMgSO4 MWMgSO4 .7H 2O 120.3 120.3 126 xC = 0.49 From the graph: xA = 0.26 xB x A 0.3 0.26 5000 869.6 mC mB xC x A 0.49 0.26 The MgSO4.7H2O crystal yield is 869.6 lb