2-E, A liquid mixture of 30 mol benzene. 30 mol toluene, and 40 mol water initially at 70°C and 101.3 kPa total pressure is heated slowly at a constant pressure of 101.3 kPa to 90°C. The vapor generated stays in contact with the remaining liquid. Assuming equilibrium between phases at all times. estimate (a) the temperature at which vaporization begins. (b) the composition of the first vapor. (c) the temperature at which vaporization is complete, and (d) the composition of the last liquid. Note: Watcer is cssentially totally immiscible with benzene and toluene. Each liquid phase contributes to the total vapor pressure. Over the temperature range involved, the vapor prcssure of benzene is 2.60 times that of tolucne, and the vapor pressure of water is 123 times that of toluene. Vapor pressure of water is: T. C 70 | 72 | 74 | 76 78 80 82 84 | 86 90 88 P. kPa 31.2 34.0 36.9 40.1 43.6 47.3 51.3 55.6 60.1 70.1

4.5(b) When a certain liquid freezes at –3.65°C its density changes from 0.789 g cm-3 to 0.801 g cm¯³. Its enthalpy of fusion is 8.68 kJ molH. Estimate the freezing point of the liquid at 100 MPa.

12 (a) (b) Describe how you can obtain the integrated form of the Clapeyron equation as below. State any assumptions you have to make. Afus H (T-T) P₂≈ P₁+ AfusV T₁ The heat of fusion (Afus H) of Hg at its normal melting point (-38.9 °C) is 2.82 cal.g¹. The densities of Hg(s) and Hg(1) at -38.9 °C and 1 atm are 14.193 and 13.690 g cm Estimate the melting point of Hg at 100 atm using the result in (a). respectively. Ans 234.8K or -38.4°C

2-E, A liquid mixture of 30 mol benzene, 30 mol toluene, and 40 mol water initially at 70°C and 101.3 kPa total pressure is heated slowly at a constant pressure of 101.3 kPa to 90°C. The vapor generated stays in contact with the remaining liquid. Assuming equilibrium between phases at all times, estimate (a) the temperature at which vaporization begins, (b) the composition of the first vapor. (c) the temperature at which vaporization is complete, and (d) the composition of the last liquid. Note: Water is essentially totally immiscible with benzene and toluene. Each liquid phase contributes to the total vapor pressure. Over the temperature range involved, the vapor pressure of benzene is 2.60 times that of toluene, and the vapor pressure of water is 1.23 times that of toluene. Vapor pressure of water is: T. °C 70 72 74 76 78 80 82 84 86 88 90 P, kPa 31.2 34.0 36.9 40.1 43.6 47.3 51.3 55.6 60.1 64.9 70.1

Estimate the freezing point (solidification temperature) of benzene at a pressure of 115 bar given that the enthalpy of fusion (AH,jus) of benzene is 9.94 kJ/mol. The corresponding densities of liquid and frozen benzene are 876 kg/m? and 894 kg/m? respectively.

The vapor pressures of the components, A and B, in a binary solution have been modeled and found to obey PA = XAPA* exp(XB²) PB = XBPB* exp(X₁²) A where ΧΑ and XB are the mole fractions, and PA* and PB* are the vapor pressures of each pure substance. (a) If PA* = 0.175 bar and PB* = 0.126 bar, compute the total vapor pressure (in bars) of the mixture when XB XB = 0.68. (b) Assuming that the vapor is an ideal gas, what are the mole fractions of each component in the vapor phase?

3. (a) At 10 °C, the vapour pressures of pure chloroform (CHCI;) and pure dichloromethane (CH2CI2) are 101 mmHg and 235 mmHg, respectively. Assume that a solution made by mixing CHCI3 and CH;Cl2 is ideal. ii. Given the following data for this solution: p (CH2C12) = 1.33 gcm³; p (CHC13) = 1.48 gcm3; partial molar volume of CH2C12 = 56.5 cm³mol·'; partial molar volume of CHC13 = 77.3 cm³mol'. Calculate AmixV

At 25 °C, the vapour pressure of pure benzene is 12.8 kPa and the vapour pressure of pure methylbenzene (toluene) is 3.8 kPa. Consider a liquid mixture with mole ratio 30% benzene-70% methylbenzene, which you can treat as an ideal liquid mixture, in a closed container. a) Calculate the mole ratio of benzene and methylbenzene in the vapour.

Pure liquid A has vapor pressure 200. bar and pure liquid B has vapor pressure 100. bar. In an AB mixture with mole fraction X = 0.500, compute the mole fraction of A in the vapor.

Acetone has a vapour pressure of 53.3 kPa at 39.5 °C and 202.6 kPa at 78.6 °C. From the above data, obtain an equation to correlate the vapour pressure of acetone. (The equation should be in the form In(P)= -A/T + Co where P, is in kPa units. Find numerical values for A and Co) A= 5756 K, Co = 17.989 A= 4756 K, Co = 16.989 A= 3756 K, Co = 15.989 A= 2756 K, Co = 14.989