analyzed sample of the condensed vapour phases and liquid phases collected during the reflux experiment with all binary mixtures. 3. Calculate the experimental value of the acetone/chloroform mole fraction ratio for each examined sample of liquid phases (XA and XC) and, separately, vapour phases (YA and YC). 4. Compile your experimental phase diagram presenting two separate overlaid trends as follows: a. Plot the boiling point temperature (TBP) recorded for the tested chloroform-acetone mixtures vs. the liquid phase mole fraction of chloroform (Xc). b. Plot TBP vs. YC for the gas phase mole fraction of chloroform. Use the 'scatter with data points connected by smoothed lines' MS Excel graph format for both lines. 5. The chloroform-acetone system forms an azeotrope with a maximum boiling point. Compare your phase diagram to those found in the literature; discuss the possible causes of observed discrepancies. Estimate the maximum boiling point and the azeotropic composition from your own data and compare them to those shown in the diagram. 6. Calculate the ideal vapour pressure (P) for chloroform and acetone at each temperature that you recorded when testing the refluxed chloroform-acetone mixtures, using the table data below and the empirical equation: P=10[(0.2185A/T)+8](torr) Note that for the correct results, temperature in Kelvin should be used. Torrs should be converted to atmospheres according to: 1 torr =0.0013158atm. 7. Next, using the tabulated pressure values for each component in the tested binary mixtures (not for the pure acetone and chloroform samples!), apply Raoult's Law to your liquid compositions at each recorded temperature. In order to calculate the theoretical values of the molar fractions in the liquid phuse, recall, that for an ideal solution, Raoult's law states that the total vapour pressure ( Ptotool) of two gaseous compounds depends on their individual vapour pressure values at a given temperature and their respective