Weight FractionĬonverting from wt fraction of the azeotrope to mole fraction: Thus, the azeotropic mole fraction is greater at P = 1 Kg/cm2 than at 1 atm: vs Although slight, one can begin to see the effect of pressure on the azeotropic point. For ethanol-water, this can be readily done using the molecular weights, MWEtOH =46.07 and MWw = Lecture 5Ħ Azetrope Composition – Mole Fraction vs. Note that the enthalpy- composition plot is presented in terms of weight fractions – we will typically use mole fractions so one must convert between the two. Note the boiling temperatures of the pure components, water and ethanol, and the temperature of the azeotrope are different due to the pressure at which the data was taken: P =đ kg/cm2 (0.97 atm) atm Water oC oC Ethanol Azeotrope Lecture 5 x,y plots for ethanol-water? Lecture 5Ĥ Enthalpy vs. x,y plots for ethanol-water? The azeotrope for ethanol-water is indicated as T = oC and a concentration of Why is this different than that determined from the y vs. Why? Why are the boiling point temperatures of the pure components different than those determined from the y vs. An azeotrope is indicated by the composition at which the isotherm becomes vertical. Points between the saturated liquid line and the saturated vapor line represent a two-phase, liquid-vapor system. Temperature is represented by isothermal tie lines between the saturated liquid (boiling) line and the saturated vapor (dew) line. Composition – Ponchon-Savarit Plotģ phases are shown on the plot – solid, liquid, and vapor. Composition – Ponchon-Savarit Plotģ Enthalpy vs. composition plot to obtain this information. We will also need to employ energy balances, based on enthalpy, for certain separation problems. We have begun to employ mass balances, both total and component.
Composition – Ponchon-Savarit Plot"- Presentation transcript:ġ Enthalpy vs.
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