Difference between revisions of "Thermodynamics"
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==Phase diagram of an ideal solution at fixed temperature== | ==Phase diagram of an ideal solution at fixed temperature== | ||
The following plot shows the vapor-liquid phase diagram for a binary ideal mixture (components: A and B). The vapor pressures of the pure substances are <math>p_A^*</math> and <math>p_B^*</math>, respectively. | The following plot shows the vapor-liquid phase diagram for a binary ideal mixture (components: A and B). The vapor pressures of the pure substances are <math>p_A^*</math> and <math>p_B^*</math>, respectively. | ||
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The number of moles in each phase (liquid or vapor) can be obtained from the lever rule: | The number of moles in each phase (liquid or vapor) can be obtained from the lever rule: | ||
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| − | <math>n^l\overline{BK}=n^v\overline{KR}</math> | + | <math>n^l\overline{\text{BK}}=n^v\overline{\text{KR}}</math> |
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Latest revision as of 09:22, 29 May 2023
Phase diagram of an ideal solution at fixed temperature
The following plot shows the vapor-liquid phase diagram for a binary ideal mixture (components: A and B). The vapor pressures of the pure substances are [math]p_A^*[/math] and [math]p_B^*[/math], respectively.
The blue curve shows the vapor pressure [math]p[/math] of the mixture as a function of the mole fraction of A in the liquid [math]x_A^l[/math]:
[math]p=p_B^*+(p_A^*-p_B^*)x_A^l[/math]
The red curve shows the vapor pressure [math]p[/math] of the mixture as a function of the mole fraction of A in the vapor [math]x_A^v[/math]:
[math]p=\dfrac{p_A^*p_B^*}{p_A^*-(p_A^*-p_B^*)x_A^v}[/math]
In the example below [math]p_A^*=1[/math] (a.u.) and the value of [math]p_B^*[/math] can be changed moving the slider below.
The number of moles in each phase (liquid or vapor) can be obtained from the lever rule:
[math]n^l\overline{\text{BK}}=n^v\overline{\text{KR}}[/math]
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