The excess Gibbs free energy for the liquid mixture chloroform(1)/ethanol(2) at 330 K is well represented by the Margules equation, written: GE = xx(1.42x + 0.59x2) RT Accordingly, the activity coefficients are given by: Y = exp[x2(0.59 + 1.66x)] Y = exp[x(1.42 - 1.66x)] The vapor pressures of chloroform and ethanol at 330 K are 88.04 kPa and 40.75 kPa, respectively. (a) It is known that this binary system forms an azeotrope at 330 K. Determine the pressure and composition of the azeotrope, assuming that vapor phase is an ideal gas mixture. (b) Repeat your calculation in Part (a), if the vapor phase is not ideal but instead can be described by a virial equation of state generalized to binary mixtures, whereby the fugacity coefficients are given by: [B1P+ P(1-)812] $1(T, P, y) = exp RT [B22P+ P(1 - y)812] $2(T, P, y) = exp xp RT = At 330 K, B1 = -963 cmmol-, B2 = 1523 cmmol-, B2 = 52 cmmol- and 12 2B12 B11B22. (Hint: You can get osat by evaluating the above equations at P = Pat and Vi = 1). You will need to solve this iteratively. One possible solutions scheme: Use your answer in (a) as a first guess, then calculate the fugacity coefficients. Using the equilibrium conditions, calculate the ratio of the activity coefficients, Y/Y2. Solve the expression for Y/Y2 for the azeotrope composition. Update the pressure estimate. With the new pressure and composition estimate, repeat the process. Iterate until the pressure and composition does not change any more