(Picture of the Pre-lab table)
(Picture of the data from the lab)
2. The reasons why there are differences in the amount of temperature lost in these five substances are intermolecular forces and molar mass. Intermolecular forces are the main reason why, however. Since there is an understanding that the stronger the IMF (Intermolecular force), the weaker the vapor pressure, whichever substance has the weakest IMF's will evaporate at a greater rate than the others. However, you may be thinking, "There are multiple substances that have the same number of hydrogen bonds, but they don't evaporate at the same rate. Why is that?" That is because of molar mass. Whenever any two substances have the same amount of bonds, it will come to the molar mass to decide which molecule will evaporate quicker (the one with the least molar mass).
3. Two substances with similar molar masses are methanol and ethanol. The reason that they evaporate at different rates is because of molar mass, since they both only have one hydrogen bond apiece. So, since ethanol is larger than methanol, it will evaporate at a slower pace than methanol.
4. Since all of the substances have -OH bonds, the focus will turn to the number of -OH bonds they have. Methanol and ethanol each only have one -OH bond, and looking at the chart, they evaporated the quickest out of the five. Next came n-Butanol and Water, which each had 2 -OH bonds, meaning that the intermolecular forces on those two substances were stronger than those of methanol and ethanol, and as a result, the evaporated at a slower pace. Finally, there's glycerin, which had 3 -OH bonds, making it the strongest of the five substances, and that shows, as the substance didn't evaporate at all.
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