chee200_ice_lab - absolute, the standard atmospheric...

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. Experimental setup [2] e versus temperature. The liquid phase extends above the curve, vapour phase is below. Theoretical curve also plotted. nverted absolute values. Equation of the trend line and the correlation coefficient are also shown on the graph. Hv = 46.45 kJ Δ o absolute, the standard atmospheric pressure value Fig. 3 equals -ΔHv/R, thus ΔHv was found: −1 ) of the line remains constant. etermined by linear interpolation from the steam tables [1]. I NTRODUCTION The objective of this laboratory experiment was to explore the effects of pressure on the boiling point of water, the temperature at which its vapour and liquid phases are in equilibrium. This was done by bringing water in a flask to boil at different pressures, while measuring both the vapour temperature and pressure using an RTD probe and a pressure transducer. A vapour-liquid equilibrium curve for water was constructed with experimentally determined boiling points of water at various vacuum pressures and compared to the curve plotted using the tabulated (ideal) values. The latent heat of vaporization of water was also calculated with these measurements, using a derivation of the Clausius-Clapeyron correlation, and the determined value was likewise compared against the tabulated latent heat value. T HEORETICAL B ACKGROUND The boiling point of a substance is the temperature at which vapor pressure equals the pressure on the substance, which is simply atmospheric pressure for open-air containers. The vapor pressure is directly proportional to the temperature of the substance; the higher the temperature, the greater the molecular kinetic energy, the more liquid vaporizes and the higher the vapor pressure. [1] [3] Consequently, for lower system
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This note was uploaded on 12/01/2009 for the course CHEM ENG CHEE 200 taught by Professor Yargeau during the Spring '09 term at McGill.

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chee200_ice_lab - absolute, the standard atmospheric...

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