Data Table: Data Table 1: Measured temperatures for just ethanol and 1-propanol. You will be using the data from here to

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Data Table Data Table 1 Measured Temperatures For Just Ethanol And 1 Propanol You Will Be Using The Data From Here To 1 (56.08 KiB) Viewed 63 times

Data Table Data Table 1 Measured Temperatures For Just Ethanol And 1 Propanol You Will Be Using The Data From Here To 2 (44.42 KiB) Viewed 63 times

Data Table Data Table 1 Measured Temperatures For Just Ethanol And 1 Propanol You Will Be Using The Data From Here To 3 (27.51 KiB) Viewed 63 times

Data Table: Data Table 1: Measured temperatures for just ethanol and 1-propanol. You will be using the data from here to create a graph of Experimental AT versus molar mass Substance T. (°C) T2 (°C) Experimental AT (T1-T2) (°C) ethanol 12.30 13.00 leite 22.78 16.08 1-propanol 6.78 Data Table 2: Measured temperatures for the other 4 liquids. You will be using the experimental AT values found here and comparing them to the extrapolated AT values calculated from the graph made from the data in data table 1. Substance T1 (°C) T2 (°C) Experimental AT Extrapolated AT (T.-T2) (°C) (from graph you created) methanol 23.38 3.68 19.78 1-butanol 22.60 20.00 2.68 acetone 23.00 1.38 21.70 butanone 27.68 9.30 13.46

Post Lab Assignment Graph 1 1. Using Excel, create a graph using the data from data table 1 comparing the Experimental AT to the molar mass for just ethanol and 1-propanol. Add a trendline between the two data points plotted in the excel graph and generate a linear equation for the trendline. 2. Using the equation for the trendline found above, one at a time plug in the molar mass for the four liquids found in data table 2 and calculate the Extrapolated AT values. Fill these calculated values into data table 2. Graph 2 1. Using Excel, create a second graph plotting the Experimental AT values versus molar mass for the four alcohols you investigated (remember alcohols have the oxygen single bonded to hydrogen). Add a trendline between the four data points plotted in the excel graph and generate a linear equation for the trendline. Print out both graphs and turn them in with this lab Post-Lab Questions: 1. In data table 2, some of your Experimental AT values should have been close to the Extrapolated AT values, and some were not close. Please explain why using the concepts of intermolecular forces. 2. Two of the liquids, butanone and 1-butanol have nearly the same molar mass but significantly different Experimental AT values. Please explain why using the concepts of intermolecular forces.

Post-Lab Question (cont.): 3. Given the information on graph 2, what would be the expected change in temperature for evaporation of 1-hexanol (C6H140)? (show work!) 4. Using the information on graph 2, what is the molar mass of an alcohol where the evaporation would no longer cause a measurable temperature change? Given the trend in alcohol structures seen on the ASA, how many carbons would you need in your alcohol to reach this point where no temperature change occurs?