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Behavior of the Regular Solution Model

Above, a ``first-order'' correction to the ideal solution model based on an atomic averaging for the enthalpy of mixing.

This is called the regular solution model.

$\displaystyle \input{equations/24-1A}$ (32-10)

where

$\displaystyle \input{equations/24-1B}$ (32-11)

and

$\displaystyle \input{equations/24-1C}$ (32-12)

Consider both terms:

Figure 32-1: The behavior of enthalpy in the regular solution model.
\begin{figure}\resizebox{6in}{!}
{\epsfig{file=figures/24-1A.eps}}
\end{figure}

Note that \bgroup\color{blue}$ \omega < 0$\egroup favors mixing, and makes sense because \bgroup\color{blue}$ \omega_{AB}$\egroup is more negative than \bgroup\color{blue}$ \ensuremath{\langle \omega_{AA} + \omega_{BB} \rangle}$\egroup.

Figure: The behavior of the ideal entropy of mixing: $ \Delta \ensuremath{{\ensuremath{\overline{S}}}^{\mathcal{IS}}} = -R(X_A \log X_A + X_B \log X_B)$
\begin{figure}\resizebox{6in}{!}
{\epsfig{file=figures/24-2A.eps}}
\end{figure}

So that, taken together: \bgroup\color{blue}$ \Delta \ensuremath{\overline{G^{mix}}} = \Delta \ensuremath{\overline{H^{mix}}} - T \Delta \ensuremath{\overline{S^{mix}}}$\egroup:

Figure 32-3: The behavior of the molar Gibbs free energy of mixing for the regular solution.
\begin{figure}\resizebox{6in}{!}
{\epsfig{file=figures/24-3A.eps}}
\end{figure}

Note that the limiting behavior for pure or extremely dilute solutions is dictated by:

$\displaystyle \input{equations/24-3A}$ (32-13)

A solution can always lower its free energy by dissolving at least a small amount component. There is thermodynamically always some finite solubility (but it can be, and often is, very, very small). This implies that the width of a single-phase region must always be finite.

Consider the case where \bgroup\color{blue}$ \omega > 0$\egroup, so the system will tend to ``unmix'' at low temperatures.

Figure 32-4: The dependence of the regular solution model on temperature for $ \omega > 0$. At low temperatures, the curve develops a ``self-common-tangent'' and is thus unstable at compositions within the tangent points with respect a decomposition into a composition-rich and a composition-poor phase.
\begin{figure}\resizebox{6in}{!}
{\epsfig{file=figures/G-rs-draw.eps}}
\end{figure}

For the case of a regular solution, the curve is symmetric around \bgroup\color{blue}$ X = 1/2$\egroup, and in this case we can calculate the positions of the common tangents:2

$\displaystyle \input{equations/24-4A}$ (32-14)

However, this is hard to solve (see Equation 32-15).

The critical temperate can be determined analytically by noting that as the common tangents form that the curvature changes sign at \bgroup\color{blue}$ X_B = 1/2$\egroup.

$\displaystyle \input{equations/24-5A}$ (32-15)

At \bgroup\color{blue}$ X_B = 1/2$\egroup, the zero first appears at

$\displaystyle \input{equations/Tcr}$ (32-16)


next up previous
Next: Spinodal Decomposition Up: Lecture_32_web Previous: Non-Ideal Solution Behavior
W. Craig Carter 2002-12-03