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(b) A vapor-liquid mixture of carbon tetrachloride(1) and $n$-heptane(2) is at $100 \mathrm{kPa}$. The activity coefficients can be derived from Wilson equation as follows:
$\begin{array}{l}
\ln \gamma_{1}=-\ln \left(x_{1}+x_{2} \Lambda_{12}\right)+x_{2}\left(\frac{\Lambda_{12}}{x_{1}+x_{2} \Lambda_{12}}-\frac{\Lambda_{21}}{x_{2}+x_{1} \Lambda_{21}}\right) \\
\ln \gamma_{2}=-\ln \left(x_{2}+x_{1} \Lambda_{21}\right)-x_{1}\left(\frac{\Lambda_{12}}{x_{1}+x_{2} \Lambda_{12}}-\frac{\Lambda_{21}}{x_{2}+x_{1} \Lambda_{21}}\right) \\
\Lambda_{12}=1.5410 \text { and } \Lambda_{21}=0.5197
\end{array}$
(i) Determine the temperature and its equilibrium composition at $x_{1}=0.4$.
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Answer from Sia

Posted 5 months ago

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Answer

The activity coefficients (γ1 and γ2) can be calculated using the Wilson equation, but without the vapor pressures of the pure components, the equilibrium composition and temperature cannot be determined.

Key Concept

The Wilson equation is used to calculate activity coefficients in a vapor-liquid equilibrium scenario.

Explanation

The activity coefficients are essential for understanding the non-ideal behavior of mixtures and are used in conjunction with Raoult's law to determine the equilibrium composition. However, without the vapor pressures of the pure components, the calculation cannot be completed.

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