The properties of mixtures

1. The properties of mixtures 자연과학대학 화학과 박영동 교수

2. Chapter 6 The properties of mixtures 6.1 The thermodynamic description of mixtures 6.1.1 Partial molar properties 6.1.2 Spontaneous mixing 6.1.3 Ideal solutions 6.1.4 Ideal dilute solutions 6.1.5 Real solutions: activities 6.2 Colligative properties 6.2.6 The modification of boiling and freezing points 6.2.7 Osmosis 6.3 Phase diagrams of mixtures 6.3.8 Mixtures of volatile liquids 6.3.9 Liquid-liquid phase diagrams 6.3.10 Liquid-solid phase diagrams 6.3.11 The Nernst distribution law

3. The partial molar volumes ofwater and ethanol at 25°C. =

4. partial molar volume

5. At 25°C, the density of a 50 per cent by mass ethanol/water solution is 0.914 g cm-3. Given that the partial molar volume of water in the solution is 17.4 cm3 mol-1, what is the partial molar volume of the ethanol?

6. partial molar Gibbs energy, GJ

7. Chap. 5 Pressure dependence of G G = H – TS dG = dH – TdS – SdT = Vdp - SdT = V For liquid or solid, ΔG = VΔp For vapor, ΔG = ∫Vdp = nRT∫(1/p)dp =nRTln(pf/pi) ΔGm=RT ln(pf/pi) ch05f01

10. The Gibbs energy of mixing of two perfect gases of two liquids that form an ideal solution.

11. Chap. 4 The entropy change with isothermal expansion ch04f04

12. The entropyof mixing of two perfect gases of two liquids that form an ideal solution.

13. Raoult's law: pA=xApA*

15. Raoult’s law The partial vapour pressure of a substance in a liquid mixture is proportional to its mole fraction in the mixture and its vapour pressure when pure: Figure 6.6  The partial vapour pressures of the two components of an ideal binary mixture are proportional to the mole fractions of the components in the liquid. The total pressure of the vapour is the sum of the two partial vapour pressures.

16. certain composition makes the solution more volatile CS2 is more volatile

17. Raoult’slaw: for Ideal solution, esp. for solvent The partial vapour pressure of a substance in a liquid mixture is proportional to its mole fraction in the mixture and its vapour pressure when pure: Figure 6.6  The partial vapour pressures of the two components of an ideal binary mixture are proportional to the mole fractions of the components in the liquid. The total pressure of the vapour is the sum of the two partial vapour pressures.

18. chemical potential of a solvent A present in solution at a mole fraction xA is

19. At equilibrium, chemical potential of any given component is same everywhere.

20. Henry’s law, for ideal solutes

21. The experimental partial vapour pressures of a mixture of trichloromethane, CHCl3 (C), and propanone, CH3COCH3 (acetone, A),

23. The chemical potential of the solute has its standard value when the molar concentration of the solute is 1 mol dm−3 (that is, ).

24. G = H – TS dG = dH – TdS – SdT = Vdp – SdT dμ = Vmdp– SmdT μs= μ*– Sm(s) dT μl= μ*– Sm(l) dT + RT lnxA {Sm(l) - Sm(s) }ΔT = RTlnxA μ* • -Sm(s)ΔT RTlnxA • -Sm(l)ΔT μ*+ RTlnxA

25. μg= μ*– Sm(g) dT μl= μ*– Sm(l) dT + RT lnxA {Sm(l) - Sm(g) }ΔT = RTlnxA μ* {Sm(l) - Sm(g) }ΔT = RTlnxA • Sm(g)ΔT μ*+ RTlnxA • Sm(l)ΔT

28. μA(xA=1, p) = μA(xA, p+Π) μA(xA, p+Π) μA(xA=1, p)

32. Understanding fractional distillation • pA=xApA*=apA* • pB=xBpB* = (1-a)pB* • a'= pA/(pA+pB)= apA*/(apA*+(1-a)pB*) • = apA*/(pB* + a(pA*-pB*))

33. Liquid-Vapor Composition and fractional distillation a'= yA= mole fraction in vapor • a'= pA/(pA+pB) • = apA*/(apA*+(1-a)pB*) • = apA*/(pB* + a(pA*-pB*)) • a'= aX/(1+a(X-1)) • where X = (pA* /pB*) a= xA= mole fraction in liquid

34. B: lessvolatile substance 나오는것은 A, 남는 것은 B A: morevolatile substance

35. lever rule and phase diagram

37. low-boiling(positive) azeotrope repeated distillation can never produce a distillate that is richer in constituent X than the azeotrope 끓어나오는 것은 Azeotrope, 남는것은 A나 B

39. 공비(共沸) 혼합물 high-boiling(negative) azeotrope 끓어나오는 것은 A나 B이지만, 남은것은 Azeotrope