can you solve please 3) & 4)

Tutorial on Phase Equilibrium Part 1: The triple point of CO2 is -56.2C, and the vapour pressure of solid CO2 below this temperature is given by: In p = -1353/T + 4.265 where p' is in Pa and T in K. The latent heat of fusion at the triple point is 1990 cal mol!. Use these data to estimate the vapour pressure of liquid CO2 at 0C, stating carefully the assumptions you make. (at the triple point .sv = 231 + alv) Part 2: Ethanol (1) and Water (2) form an azeotrope containing 89.43% molar ethanol, and boiling at 78.15C at a pressure of 1 atm. Pure component vapour pressures are given by the Antoine equations (p in mmHg, T in K): In pi* = 18.5242 - 3578.91/(T - 50.51) In p2 = 18.3443 - 3841.20/(T - 45.16) 1) Check the normal BPt predicted by these equations and compare with the experimental values of 78.4C and 100C. 178.34C, 100.01C] 2) Estimate the van Laar constants A12 & Azi and the Margules constants B12 & B2, from the azeotropic data and compare with the following data in Perry (Table 13-2): A12 = 1.6789; A21 = 0.9227; B12 = 1.6022; B2i = 0.794. N.B. Because yn is very close to 1.0, and hence In(Yu) is very close to zero, small errors in T, and hence pi', can cause large errors in A12. [1.50, 0.97; 1.39, 0.95) 3) Use your estimates of the van Laar & Margules constants to estimate the bubble point and equilibrium vapour composition at 1 atm of a liquid containing 9.66% molar ethanol. Compare with the values given by Perry (Table 13-1): T=86.7C y = 43.75% molar. [van Laar: 87.7C, 41.6% molar; Margules: 88.5C, 40.7% molar) 4) Repeat the calculations of (c) (van Laar only) for the dew point of a vapour containing 61.22% molar ethanol at 1 atm, and compare with Perry's values of T = 80.7C and x1 = 39.65% molar. [81.1C; 35.5% molar