Vapour Pressure Experiment Essay

1264 WordsMay 19, 20156 Pages
Abstract In this experiment, the purpose was to investigate the relationship between the vapor pressure of a liquid and its temperature. The purpose of the extension was to prove this relationship using the Clausius-Clapeyron equation, including data found during the main experiment procedure(s). The experimental results obtained supported our hypothesis in this procedure the relationship of vapor pressure to temperature was found. The hypothesis was that the two bore a direct relationship to each other, which means one increasing as the other increases. The data collected supports the original hypothesis. As vapor pressure went up, so did the temperature. One can also infer that increasing the temperature and thus, kinetic energy, increases the vapor pressure and the rate at which random interactions occur. Using this information, one would predict that raising the temperature in a bottle of soda causes the vapor pressure to increase and more molecules to escape faster, leading the soda to go “flat” at a much faster rate. Based on the results, methanol and ethanol exhibit different kinds of intermolecular forces and different vapor pressures. The heat of vaporization (∆Hvap) was found to be 162, which based off of the established value of 37.43, constituted a 332.81% error. Introduction Vapor pressures are an everyday surrounding to us, but many of us do not realize this common occurrence. The simplest way to define vapor pressure is the pressure created by a vapor or gas that forms above a liquid or solid of the same substance.1 Picturing a soda bottle, the bottle itself is pressurized until the hiss sound you hear upon opening the bottle for the very first time. That is the vapor escaping. In a closed soda bottle, gas molecules are converting to liquid and liquid molecules are converting to gas in dynamic equilibrium. Temperature changes (such

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