CHE 415 - Vapour-Liquid Distillation prelab Report (Data Recorder) 2006

Group 2, Section 2 Pre-Lab (Data Recorder) Liquid-Vapor Equilibrium October 11, 2006 Experimental Results Table 1: Vapour-Liquid Equilibrium Raw Data from Run#1 Time (min) Mass of Solution (g) Volume (ml) Mole Fraction Pressure (psi) Temperature (oC) x y Density of Solution Remaining in Still at the end of experiment: Density of Solution in Receiver at the end of experiment: Sample Calculations The following calculations were done with these theoretical values: Density of Solution Remaining in Still at the end of experiment: 1.5g/ml Density of Solution in Receiver at the end of experiment: 1.8g/ml Therefore, Mole Fraction of Methanol in Receiver: cmeth= ?meth/MWmeth = 0.8/32.05 = 0.025mol/ml cwater= ?water/MWwater = 0.055mol/ml Thus, xmeth = cmeth/c = 0.3125 = x1 Then according to Raoult’s Law: ymethP=xmethPometh (ymeth)(760mmHg)= (0.3125)(26.5mmHg) ymeth = 0.011 = y1 Therefore, the activity coefficients can be found to be used to determine the azeotrope of the binary system: The activity coefficients according to the mole fractions at different temperatures and times throughout the experiment then can be plotted in a ? vs. mole fraction graph to determine if an azeotrope is possible for this binary system. The plot would look similar to Figure 2 on page 5. Expected Plots using Experimental Data Note: The following are graphs will be similar to was is expected when conducting a VLE experiment using a methanol-water binary solution. Figure 1: VLE Diagram for a Methanol-Water System Source: media.wiley.com/product_data/excerpt/85/04717788/0471778885.pdf Figure 2: Activity Coefficient Plot for a Methanol-Water System Source: media.wiley.com/product_data/excerpt/85/04717788/0471778885.pdf 4 4