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11.4: Ideal Solutions obey Raoult's Law

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  • Liquids tend to be volatile, and as such will enter the vapor phase when the temperature is increased to a high enough value (provided they do not decompose first!) A volatile liquid is one that has an appreciable vapor pressure at the specified temperature. An ideal mixture continuing at least one volatile liquid can be described using Raoult’s Law.

    Raoult’s Law

    Raoult’s law can be used to predict the total vapor pressure above a mixture of two volatile liquids. As it turns out, the composition of the vapor will be different than that of the two liquids, with the more volatile compound having a larger mole fraction in the vapor phase than in the liquid phase. This is summarized in the following theoretical diagram for an ideal mixture of two compounds, one having a pure vapor pressure of \(p_B^o = 450\, Torr\) and the other having a pure vapor pressure of \(p_B^o = 350\, Torr\). In Figure \(\PageIndex{1}\), the liquid phase is represented at the top of the graph where the pressure is higher.

    Figure \(\PageIndex{1}\): The liquid phase is represented at the top of the graph where the pressure is higher

    Oftentimes, it is desirable to depict the phase diagram at a single pressure so that temperature and composition are the variables included in the graphical representation. In such a diagram, the vapor, which exists at higher temperatures) is indicated at the top of the diagram, while the liquid is at the bottom. A typical temperature vs. composition diagram is depicted in Figure \(\PageIndex{2}\) for an ideal mixture of two volatile liquids.

    Figure \(\PageIndex{2}\): A typical temperature vs. composition diagram.

    In this diagram, \(T_A^o\) and \(T_B^o\) represent the boiling points of pure compounds \(A\) and \(B\). If a system having the composition indicated by \(\chi_B^c\) has its temperature increased to that indicated by point c, The system will consist of two phases, a liquid phase, with a composition indicated by \(\chi_B^d\) and a vapor phase indicated with a composition indicated by \(\chi_B^b\). The relative amounts of material in each phase can be described by the lever rule, as described previously.

    Further, if the vapor with composition \(\chi_B^b\) is condensed (the temperature is lowered to that indicated by point b') and revaporized, the new vapor will have the composition consistent with \(\chi_B^{a}\). This demonstrates how the more volatile liquid (the one with the lower boiling temperature, which is A in the case of the above diagram) can be purified from the mixture by collecting and re-evaporating fractions of the vapor. If the liquid was the desired product, one would collect fractions of the residual liquid to achieve the desired result. This process is known as distillation.

    Contributors and Attributions

    • Patrick E. Fleming (Department of Chemistry and Biochemistry; California State University, East Bay)

    Thermodynamic potentials of ideal solutions

    As we have seen, an ideal solution obeys Raoult's law:

    \[P_j = x_jP^*_j\]

    When we substitute we find a logarithmic relationship between thermodynamic potential and mole fraction:

    Thermodynamics of ideal mixing

    When we add \(n_1\) moles of component \(1\) and \(n_2\) moles of component \(2\) to form an ideal liquid solution this is generally a spontaneous process. Let us consider the Gibbs free energy change of that process:

    And yes this is always negative, so mixing is spontaneous. However the expression looks suspiciously familiar. Apart from a factor -T is is equal to the entropy of mixing!

    This leaves no room at all for an enthalpy effect:

    Even though in the liquid there are strong interactions between neighboring particles there is no enthalpy change because it does not matter what this neighboring molecule is.

    If we represent the average interaction energy between molecule i and j by Uij we are essentially assuming that

    In practice this is seldom the case. It usually does matter and then the enthalpy term is not zero. As this affects the thermodynamics of the liquid solution it should als affect the vapor pressures that are in equilibrium with it.

    Molar volumes

    From the change of \(G\) in its natural variables we know that:

    \[ \left (\dfrac{\partial G}{\partial P} \right)_T =V \]

    This means that if we take

    \[ \left (\dfrac{\partial \Delta G}{\partial P} \right)_T =\Delta V_{mix} \]

    In the ideal case we get:

    \[ \left (\dfrac{\partial \Delta G^{ideal}}{\partial P} \right)_T =\Delta V_{mix}^{ideal} \]

    \[ \left (\dfrac{\partial RT ( n_1 \ln x_1 + n_2\ln x_2)}{\partial P} \right)_T =\Delta V_{mix}^{ideal} =0\]

    In the ideal case volumes are simply additive and we need not worry about how the partial molar volumes change with composition.