Solid Liquid Equilibrium in a Binary System
1. Attach the plots of nine cooling curves to this datasheet, together with the derivative plots.
2. Complete the following table, including the data for pure naphthalene and biphenyl.

Samples    x1 (naphthalene)    x2 (biphenyl)      Freezing point (°C)
1                              0                         1

3. Construct a phase diagram. Plot the freezing temperatures vs mole fraction of biphenyl. Label the different regions of the phase diagram, including the eutectic point. You can insert the phase diagram below with proper figure captions.
4. What is the eutectic point in your experiment?
5. Complete the following table for the literature values.

Sample                Tf            ΔHfusion

Please provide references for the literature values:
6. Use equation 1 to plot the ideal solubility curves (T vs. x) for solutions of naphthalene in biphenyl and solutions of biphenyl in naphthalene, respectively. Use the literature values for the freezing temperatures and the heats of fusion. Please insert the two plots below with proper figure captions.
7. Convert the x-axis of the naphthalene solubility curve from mole fraction naphthalene to more fraction biphenyl. Plot the two solution curves on the same graph. Draw a horizontal line where the two curves cross to represent the eutectic temperature. Label the different regions of the graphs to complete the theoretical diagram. Please insert the theoretical diagram below with proper figure captions.
8. Compare the experimental and theoretical phase diagrams. Regions for comparison should include the freezing temperatures of naphthalene and biphenyl, the eutectic temperature and the eutectic composition.

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