Why Is Pentane Observed To Have The Highest Evaporation Rate

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Evaporation and Intermolecular Forces Lab
Analysis Questions:
Pentane was observed to have the highest evaporation rate. Isopropanol had the lowest evaporation rate. Pentane is nonpolar and it’s strongest intermolecular force is London Dispersion Force. Because Isopropanol is polar and has strong hydrogen bonds, the bonds are harder to break and the evaporation rate was lower because it took more time to break this force. Pentane has a weaker molecular force than the hydrogen bonds so it evaporated faster than the Isopropanol. Every time the container the substance is in is opened some of it will evaporate, causing the temperature of the liquid to change. As it evaporates, the temperature decreases. The molar mass of a substance can be …show more content…

The evaporation rate for Isopropanol for my group was -0.10913 degrees Celsius per second and the average for the class was -0.11 degrees Celsius per second. For Acetone we got -0.2244 degrees Celsius per second, and the class average was -0.30 degrees Celsius per second. The rate for Hexane we got was -0.17307 degrees Celsius per second, and the class average was -0.13 degrees Celsius per second. The evaporation rate for Pentane was -0.35389 degrees Celsius, while the class average was -0.47 degrees Celsius per second. Pentane had the highest evaporation rate and and Isopropanol had the lowest. This is because Isopropanol is polar and has strong hydrogen bonds that are harder to break than the weak London Dispersion Force in the nonpolar Pentane. Isopropanol took more time to break the bonds, causing a slower evaporation rate than the evaporation rate of Pentane. Pentane evaporated the fastest out of all of the substances because its bonds were so weak. Hexane and Pentane have London Dispersion Force as their strongest intermolecular force, but Hexane has a higher molar mass than Pentane. In the data, it is shown that Hexane has a slower evaporation rate the Pentane, meaning that the intermolecular forces in Hexane are stronger than

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