experiment 1 kjgf
TRANSCRIPT
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[1]
[2]
[3]
[4]
EXPERIMENT 1
SOLID LIQUID PHASE DIAGRAM
Important: bring a formatted 3.5 floppy diskette/USB flash drive for this laboratory you will
need it to save your data files!
Introduction
The relation of cooling curves to phase diagrams form the basis of thermal analysis, an
important technique for constructing phase diagrams. In the solid-liquid phase equilibrium chosen
for study here, the two components, although miscible with one another in the liquid phase, are of
limited solubility in one another as solids. Thus, we can consider them as pure solids, plus a two-
component liquid. Such systems exhibit an eutectic temperature at which the three phases can
coexist in equilibrium at a fixed pressure.
Solid-liquid equilibria differ from liquid-vapour equilibria in that they are essentially
independent of pressure changes on the order of a few atmospheres, owing to the small molar
volume change associated with fusion. This is a consequence of the Clapeyron equation:
We shall be concerned here with temperature-composition diagrams atp = 1 atm.
If the liquid solution behaves ideally, the solubility of each component in the liquid
depends on temperature, according to:
where:
XA andXB are the mole fractions of components A and B, respectively,
HA and HB are the heats of fusion of components A and B, respectively, and
TA and TB are the melting points of the pure components.
Equations [1] and [2] can be represented in the following phase diagram:
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Figure 1.1
The eutectic composition (XE) and eutectic temperature (TE) are given by the intersection of
the two liquid curves. With the aid of graph (a) in Figure 1.1, we can predict the general nature of
the cooling curves in a system of this kind. The curves in graph (b) are plots of temperature against
time obtained when liquid solutions of various compositions are allowed to cool.
When a liquid consisting of pure A is cooled, the temperature falls until solid A begins to
form. The temperature then remains constant until solidification is complete, where upon it fallsagain. It is said that the curve shows a thermal arrest. When a liquid having the eutectic
composition is cooled, the behaviour is similar in that a thermal arrest is obtained.
However, when a liquid of some other composition for example, X1 (see graph (a)) is
cooled, solid A begins to form at temperature T1. This tends to deplete the liquid of component A,
so that its composition passes throughX2,X3, ... and the temperature falls as long as solid A alone
continues to come out of solution.
The abrupt change in slope, which occurs when solid A begins to form, is called a break.
When the composition of the solution finally reachesXE, solid B begins to form together with solid
A and the two solids continue to separate from solution at the temperatureTE until no liquid remains,
and thus an arrest occurs.
The binary solid-liquid phase diagram for the naphthalene-diphenylamine system will beconstructed from cooling curves. Several mixtures of different ratios of the two components will
be melted, and temperature versus time curves will be plotted as the mixtures cool. The
temperatures at which these breaks and arrests occur are plotted as a function of composition of the
mixtures to obtain the phase diagram.
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jumbo magnetic stirrer
ice water bath
to Labpro
temperature probe
stir bar
plexiglasscontainerand lid
medium test tube
600 mL beaker
hotplate
Figure 1.2
7. Click on on the Logger Pro software. This will provide a real time plot of thechanging temperature in the sample. The collection will continue for a maximum of 1000
seconds. However, if you observe a distinct arrest or break in the pattern, you may
terminate the acquisition and begin a new run. Note:keep the water bath cold, especially
for the later runs! Remember that the pure compounds and the eutectic mixture should have
only one arrest! Be sure to pull out the stir bar before dumping waste!
8. Save a file for this run by exporting the data as a text file. Excel can later be used to process
this data. Make sure to use file names that will clearly distinguish your data sets.
9. Find the arrests on the curves for the pure compounds, the breaks on all mixtures, and the
eutectic arrest for two of the latter.
Calculations1. Extract the break and arrest temperatures from the cooling curves. Print out plots of your
cooling curves (Excel can be used). Convert all temperatures to the thermodynamic
temperature scale (i.e., Kelvin) and use these units for all of the calculations.
2. Determine the mole fraction,Xnaphthalene, for all of the mixtures. Determine the mole fraction
of diphenylamine,Xdiphenylamine, for runs 6, 7 and 8.
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3. Using the break and arrest temperatures of these mixtures, plot the two limbs of the solid-
liquid phase diagram (i.e., temperature as a function of the mole fraction of naphthalene).
Runs 1-5 will constitute one limb, and runs 6-8 will make up the other.
4. Draw the liquidus curves, identify the eutectic line and identify the phases present in each
area of the diagram.
5. Determine the eutectic composition and eutectic temperature from the phase diagram.6. Using [1] and [2], plot lnXnaphthalene against 1/Tfor runs 1-5 and plot lnXdiphenylamine against 1/T
for runs 6-8. The plots should be linear with:
slope = -Hi/R and
-slope/intercept = Ti (the melting temperature of the pure component.)
7. Calculate the enthalpy of fusion and the melting point for each component, assuming that
an ideal liquid solution is formed. Compare to literature values by calculating the percent
error forfusHand temperature, as well as the absolute error for the temperature.
Lab Questions
1. A series of Ni-Mn mixtures were prepared and allowed to reach equilibrium at various
temperatures. Use the following data to plot a phase diagram (preferably on an Excelspreadsheet) for the Ni-Mn system. Label the different components and number of phases
in each part of the phase diagram.
Mn-Rich mixtures:
T/(oC) 1260 1200 1150 1100 1050 1000
w(Ni)sol 0.00 0.04 0.08 0.13 0.22 0.45
w(Ni)liq 0.00 0.07 0.12 0.18 0.29 0.45
Ni-Rich mixtures:T/(oC) 1050 1100 1150 1200 1250 1300 1350 1400 1450
w(Ni)sol 0.58 0.64 0.70 0.75 0.80 0.85 0.90 0.96 1.00
w(Ni)liq 0.54 0.62 0.68 0.73 0.78 0.83 0.88 0.94 1.00
2. What is the composition of the solid solution in equilibrium with a liquid mixture of Ni and
Mn at 1000 oC? What is this point designated as?
References
1. Atkins, Peter and Julio de Paula. Physical Chemistry. 7th
ed. New York: W. H. Freeman,2002. 144-148.
2. Shoemaker, David P., Garland, Carl W., and Joseph W. Nibler. Experiments in Physical
Chemistry. 6th ed. New York: McGrawHill, 1996. 215-221.
3. Silbey, Robert J., and Robert A. Alberty. Physical Chemistry. 3rd ed. Wiley, 2001.
Chapter 6, Section 6.9.