A vapor/liquid experiment for the carbon disulfide(1) + chloroform(2) system has provided the following data at 298 K: P1sat = 46.85 kPa, P2sat = 27.3 kPa, x1 = 0.2, y1 = 0.363, and P = 34.98 kPa. Estimate the dew pressure at 298 K and y1 = 0.6, using the Van Laar equation.

Prompt/Given Information: Consider a reversible isothermal expansion of vapor benzene at 450 K from 1 to 0.1 MPa. Assume that the PVT behavior of benzene obeys van der Waals equation of state.                                      P = (RT)/(V - b) - a/V2            for benzene: a = 1884514 (cm6 * MPa)/mol2 and                                  b = 119.47 cm3/mol For your convenience, at 450 K and 0.1 MPa the volume of vapor benzene is 37025 cm3/mol, and at 450 K and 1 MPa it is 3312.4 cm3/mol. R = 8.314 (MPa*cm3)/(mol*K). Note: 1 cm3*MPa/mol = 1 J/mol   Question: What is the change of internal energy? What would be the change of internal energy if the gas was ideal?

Calculate the fugacity of dry ice (CO₂ ice) at the triple point (T=216.55 °K, P-5.12673 bar). Assume that the thermal properties of the vapor phase of carbon dioxide are described by the Peng-Robinson equation of state. Express your result in bar and and round your numerical answer to one decimal digit.

How many intensive variables are necessary to completely specify the state of pure water and pure glycerol at temperatures above 18 degrees C. What are they? If the pressure is fixed at 1 bar, how many intensive variables are necessary?