Dissertation
Dissertation > Mathematical sciences and chemical > Chemistry > Physical Chemistry ( theoretical chemistry ),chemical physics > Chemical thermodynamics, thermochemistry, thermodynamic equilibrium > Thermodynamic equilibrium > Phase Equilibria

High Pressure Vapor-Liquid Equilibria of Two Binary Systems Containing Carbon Dioxide and Alkanes

Author HanFang
Tutor TianYiLing
School Tianjin University
Course Chemical Engineering
Keywords CO2 N-octane N-heptane N-hexane High-pressure phase equilibria
CLC O642.42
Type Master's thesis
Year 2004
Downloads 193
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The high-pressure phase equilibrium data of the phase equilibria in the field of research focus particular emphasis on the study of the phase of the binary system consisting of CO 2 and saturated alkanes . The use of a variable- volume autoclave by the static method to study the high-pressure gas-liquid phase equilibria . Determined the the supercritical CO 2 n-octane , n- heptane , n-hexane three binary systems of high-pressure phase equilibrium data to fill at home and abroad of these three systems research gaps . These three systems under different pressure and temperature conditions , a gas-liquid two- phase CO 2 < / sub> is the mole fraction, density and molar volume information obtained by experiments . Experimental results show that : within the scope of the Experimental Study , as the pressure increases , the solubility of CO2 in the liquid phase is increased , the liquid phase density decreases , and the content in the gas phase is reduced , the vapor density increases ; at the critical point the two phases becomes one phase. Select PR and PRSV equation of Van der Waals-1 and Margules mixing rule with four different methods of calculation , using the search method to optimize the calculation of the the above Binary high pressure GLE of experimental data . The results show that : different with different equations of state and mixing rules , different calculation accuracy . For CO 2 Paraffin binary system , Panagiotopoulos-Reid mixing rule better than Van der Waals-1 mixing rule calculation effect .

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