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Determining The Factors That Affect Evaporation Rates

1149 Words5 Pages

Purpose: Intermolecular force is the strength of the bond between two molecules. It is affected by their molar masses since the more lightweight a molecule is, the easier it is to pull it away from whatever it is bonded to. Although molar mass affects intermolecular forces, it is not the greatest factor in the determination of a bond’s strength. Polarity, or the positive and negative sides of a molecule dictate the intermolecular forces far greater than molar mass. When a molecule only has a small difference in electronegativity (their attractiveness to electrons) between the elements it consists of, the intermolecular force is called london-dispersion. London-dispersion forces are from when a molecule gets a temporary dipole and is weakly …show more content…

However, if the intermolecular force is in a medium range, it can be called dipole-dipole, which means that a permanent charge exits at opposite ends of the molecule and a stronger bond is formed. The purpose of this lab was to determine the factors that affect evaporations rates using multiple different liquids. By measuring the evaporation rates using a LabQuest and probe, it is possible to determine what kind of intermolecular force the liquid has, as well as what factors dictate the strength of the bond, because the faster a liquid evaporates, the weaker the intermolecular forces are due to them breaking apart rather easily to become a gas. The same goes but for the opposite; if a liquid takes longer to evaporate, it has a stronger intermolecular force and thereby the bonds between the molecules hold the substance more tightly together instead of breaking apart to …show more content…

Based on the lab, polarity affects intermolecular forces the greatest because as the polarity increases, the intermolecular forces increase alongside it. However, if the polarity is the same between molecules, the intermolecular force is dependent upon the molar mass since compounds with higher molar masses are harder to rip apart, creating a larger intermolecular force, while lighter molecules are easily separated from the rest making the intermolecular forces small. For each of the alcohols, the polarity was the same (polar/nonpolar) which made it possible to see how intermolecular forces are affected by molar mass as well. For ethanol, the molar mass was 46.07 g/mol and for propanol, the molar mass was 60.10 g/mol. According to the data gathered in the experiment, propanol evaporated significantly slower than ethanol, with ethanol reaching temperatures just under 15℃ while propanol only reached a little over 25℃ during the minute trial. Since ethanol got colder than propanol in a much shorter time, it shows that ethanol gained more energy from breaking apart more easily. A similar event occurred between methanol and butanol with butanol having the larger molar mass at 74.12 g/mol compared to 32.04 g/mol. Butanol evaporated the slowest of all of the substances since it is polar/nonpolar and had one of the largest masses. Methanol on the other hand,

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