Overview: properties

How the properties are calculated and definitions used can be found in the section Calculation of properties in the COSMO-RS manual.

Step 1: Start ADFcrs

For this tutorial we assume that you know how start ADFcrs and how to add compounds. Like in tutorial 2 we ask you to add the compounds water, methanol, ethanol, and benzene. One can do this, for example, by opening the .crs file that was created in tutorial 2. Save the file as tutorial3.crs.

Start ADFcrs
Select File → Open...
Select ‘tutorial2.crs’ in the ‘Filename’ field
Select File → Save As
Enter the name ‘tutorial3’ in the ‘Filename’ field

Alternatively on a Unix like system one may copy the COSMO result files (water.coskf, methanol.coskf, ethanol.coskf, and benzene.coskf) in the directory $ADFHOME/examples/crs/Tutorial2 to an empty directory and enter the following command in this directory where the COSMO result files are present:

$ADFBIN/adfcrs benzene.coskf ethanol.coskf methanol.coskf water.coskf &

Note that one has to set the number of ring atoms for the benzene compound.

Select Compounds → List of Added Compounds
Click on the left side benzene
Enter ‘6’ without quotes in the ‘Nring’ field
Select File → Save As
Enter the name ‘tutorial3’ in the ‘Filename’ field

In the compounds window one can also set the vapor pressure of the pure compounds at a given temperature, or set the Antoine parameters. If these values are not specified (if they are zero) then the pure compound vapor pressure will be approximated using the COSMO-RS method. This is relevant, for example, for the calculation of the (partial) vapor pressures of mixtures, calculation of boiling points of mixtures, and calculation of Henry’s law constants.

Step 2: Vapor pressure

The vapor pressure of a solvent at different temperatures can be calculated with Properties → Vapor Pressure Pure Solvents or Properties → Vapor Pressure Mixture.

Select Properties → Vapor Pressure Pure Solvents
Check the ‘+’ button to add ‘methanol’
Select unwanted solvents in the the list
Check the ‘-‘ button to remove these unwanted solvents
Press ‘Run’
/scm-uploads/doc.2016/Tutorials/_images/t3_vaporinput.png

In this case the result is a table with one entry:

/scm-uploads/doc.2016/Tutorials/_images/t3_vaportable.png
Select Celsius for the unit of temperature
Enter ‘0.0’ without quotes in the ‘Temperature from:’ field
Enter ‘100.0’ in the ‘to:’ field
Press ‘Run’

In this case the result is a graph and a table. If one clicks in the graph window at the left or below the axes, a popup window will appear in which one can set details for the graph window. After some manipulation in the details of the graph, the graph can look like:

/scm-uploads/doc.2016/Tutorials/_images/t3_vaporgraph.png

In this case COSMO-RS predicts a vapor pressure of about 0.61 bar (around 455 Torr) at 323.15 K (50.0 °C) for the pure liquid methanol.

/scm-uploads/doc.2016/Tutorials/_images/t3_vaportable2.png

Step 3: Boiling point

The boiling point of a solvent at different pressures can be calculated with Properties → Boiling Point Pure Solvents or Properties → Boiling Point Mixture.

Select Properties → Boiling Point Mixture
Select ‘2 components’ in the popup menu next to Solvent
Select ‘methanol’ for the first component in the Solvent
Select ‘ethanol’ for the second component in the Solvent
Enter ‘0.5’ for the ‘Mole fraction’ of methanol
Enter ‘0.5’ for the ‘Mole fraction’ of ethanol
Select atm for the unit of pressure
Enter ‘0.1’ in the ‘Pressure from:’ field
Enter ‘1.0’ in the ‘to:’ field
Press ‘Run’
/scm-uploads/doc.2016/Tutorials/_images/t3_boilinginput.png

In this case the result (may take several seconds) is a graph and a table.

/scm-uploads/doc.2016/Tutorials/_images/t3_boilinggraph.png

The red curve is the total vapor pressure, the blue curve the partial methanol vapor pressure, and the green curve is the partial ethanol vapor pressure. The table gives the numerical values.

/scm-uploads/doc.2016/Tutorials/_images/t3_boilingtable.png

Thus in this case COSMO-RS predicts a boiling point of 339.8 K (66.7 °C) at 1 atm. for this mixture of 50% mole fraction methanol and 50% mole fraction ethanol. At this temperature COSMO-RS predicts that the vapor consists about 69% of methanol.

Using Graph → Y Axes → one can view different properties in the graph, like activity coefficients and excess energies.

Step 4: Flash point

The flash point of a mixture can be calculated with Properties → Solvent Flash Point, if pure compound flash points are given as input.

Here we mix equal volumes of water (assuming a density of 0.997 kg/L) and ethanol (assuming a density 0.789 kg/L). For a flash point calculation the pure compound flash points are needed as input, since COSMO-RS does not predict pure compound flash points. The ADF COSMO-RS module uses Le Chatelier’s mixing rule to calculate the flash point of a mixture.

Select Compounds → List of Added Compounds
Select ‘ethanol’
Enter ‘286’ for the ‘Flash point’ of ethanol
Select Properties → Flash Point
Change the popup menu ‘Mole fraction’ in ‘Mass fraction’
Select ‘ethanol’ for the first component in the Solvent
Select ‘water’ for the second component in the Solvent
Enter ‘0.442’ for the ‘Mass fraction’ of ethanol
Enter ‘0.558’ for the ‘Mass fraction’ of water
Press ‘Run’
/scm-uploads/doc.2016/Tutorials/_images/t3_flashpointinput.png

In this case the calculated flash point will be close to 25 °C.

/scm-uploads/doc.2016/Tutorials/_images/t3_flashpointtable.png

Step 5: Activity coefficients, Henry coefficients, Solvation free energies

The activity coefficients a solvent and the activity coefficients of infinitely diluted solutes in a solvent can be calculated with Properties → Activity coefficients. At the same time Henry coefficients and solvation free energies will be calculated.

Select Properties → Activity coefficients
Select ‘water’ for the first component in Solvent
Add ‘benzene’, ‘ethanol’, and ‘methanol’ to the list of Solutes
Press ‘Run’
/scm-uploads/doc.2016/Tutorials/_images/t3_activitiesinput.png

If one does not supply a density of the solvent in the input the program calculates the density of the solvent by dividing the mass of a molecule with its COSMO volume. Note that the calculated activity coefficients do not depend on this density. One may improve the results for the calculation of the Henry constants, by selecting a compound in the List of Added Compounds, and include pure a compound vapor pressure at a given temperature.

The result of the calculation is given in the form of a table.

/scm-uploads/doc.2016/Tutorials/_images/t3_activitiestable.png

Relevant for the calculation of the Gibbs free energy of solvation ΔG from the gas phase to the solvated phase is the reference state, used here is 1 mol/L in both phases.

Step 6: Partition coefficients (log P)

Preset Octanol/Water, Benzene/Water, Ether/Water, Hexane/Water

The partition coefficients (log P) of infinitely diluted solutes in a mixture of two immiscible solvents can be calculated with Properties → Solvent Log Partition Coefficients. There are presets for the calculation of Octanol/Water, Benzene/Water, Ether/Water, and Hexane/Water partition coefficients. The presets use compounds that are present in $ADFHOME/atomicdata/ADFCRS. First the preset Octanol/Water is used.

Select Properties → Partition Coefficients (LogP)
Select ‘Preset Octanol-Water’ in the popup menu next to Solvent
Add ‘benzene’, ‘ethanol’, and ‘methanol’ to the list of Solutes
Press ‘Run’
/scm-uploads/doc.2016/Tutorials/_images/t3_logpinput.png

In case of partly miscible liquids, like the Octanol-rich phase of Octanol and Water, both components have nonzero mole fractions. The preset also gives a value for the molar volume quotient of the two solvents.

The result of the calculation is given in the form of a table.

/scm-uploads/doc.2016/Tutorials/_images/t3_logptable.png

User defined

A user can also define 2 phases of a mixture of two (or three) immiscible solvents.

Select Properties → Partition Coefficients (LogP)
Select ‘User Defined 2 components’ in the popup menu next to Solvent
Select ‘benzene’ for the first component in the solvent
Select ‘water’ for the second component in the solvent
Click the check box ‘Use input volume solvent phase 1/phase 2’
Enter ‘4.93’ in the ‘Use input volume solvent phase 1/phase 2’ field
Add ‘ethanol’, and ‘methanol’ to the list of Solutes
Press ‘Run’
/scm-uploads/doc.2016/Tutorials/_images/t3_logpinput2.png

Here an input value is used for the volume quotient of the two solvents. If one does not include such value, the program will use the COSMO volumes to calculate the volume quotient. The COSMO volumes can be found by selecting a compound in the List of Added Compounds.

The result of the calculation is given again in the form of a table.

/scm-uploads/doc.2016/Tutorials/_images/t3_logptable2.png

Step 7: Solubility

The solubility of a solute in a solvent can be calculated with Properties → Solubility in Pure Solvents or Properties → Solubility in Mixture. The solute can either be a liquid, solid, or gas.

Solubility liquid in a solvent

First the solubility of benzene in water for a range of temperatures.

Select Properties → Solubility in Pure Solvents
Check the ‘+’ button to add ‘water’
Select ‘benzene’ for the ‘Solute’
Enter ‘273.15’ without quotes for the temperature in the ‘from:’ field
Enter ‘373.15’ in the ‘to:’ field
Press ‘Run’
/scm-uploads/doc.2016/Tutorials/_images/t3_solubilityinput.png

If a range of temperatures is requested a graph is shown.

/scm-uploads/doc.2016/Tutorials/_images/t3_solubilitygraph.png

The assumption made in the solubility calculation may be invalid in case of a solubility of a liquid in a solvent, especially if the solubility of the solvent in the liquid is high. For binary systems one may check this by calculating the miscibility gap in the binary mixture of the two liquids. An example is given for the calculation of the miscibility gap in the binary mixture of Methanol and Hexane.

Note that experimentally benzene is a solid below 5.5 °C, and a gas above 80.1 °C. This has not been taken into account in this case. See the next examples.

Solubility solid in a solvent

For the solubility of a solid compound it is necessary to include the melting point, the enthalpy of fusion, and optionally, since it is often not so important, the Δ heat capacity of fusion of the pure compound. These values can be given for each compound if one selects Compounds → List of Added Compounds. Here, some experimental values will be included for benzene (see, for example, http://en.wikipedia.org/wiki/Benzene).

Select Compounds → List of Added Compounds
Click on the left side benzene
Enter ‘278.7’ in the ‘Melting point’ field
Enter ‘2.37’ in the ‘Δ_fusion H’ field
/scm-uploads/doc.2016/Tutorials/_images/t3_compoundbenzene.png

Also an experimental value for the density of water will be used:

Select Properties → Solubility in Mixture
Select ‘water’ for the first component in ‘Solvent’
Check the ‘+’ button to add ‘benzene’ in the list of Solutes
Click the check box ‘Use input density solvent (kg/L)’
Enter ‘1.0’ in the ‘Use input density solvent (kg/L)’ field
Change one of the popup menu’s ‘Kelvin’ in ‘Celsius’
Enter ‘0.0’ without quotes in the ‘from:’ field
Enter ‘10.0’ in the ‘to:’ field
Select Graph → Y Axes → solubility (g/L solvent)
Change the popup menu next to Solutes from ‘Liquid’ to ‘Solid’
Press ‘Run’
/scm-uploads/doc.2016/Tutorials/_images/t3_solubilityinput2.png

A graph (and table) is shown, which after some manipulations could look like:

/scm-uploads/doc.2016/Tutorials/_images/t3_solubilitygraph2.png

Solubility gas in a solvent

For the solubility of a gas one should the change the ‘Liquid’ popup menu in ‘Gas’ and enter a partial pressure in the ‘Pressure’ field.

Select Compounds → List of Added Compounds
Click on the left side benzene
Enter ‘1.01325’ in the ‘Pure compound vapor pressure’ field
Enter ‘353.3’ in the ‘at temperature’ field
Select Properties → Solubility in Mixture
Select ‘water’ for the first component in ‘Solvent’
Check the ‘+’ button to add ‘benzene’ in the list of Solutes
Click the check box ‘Use input density solvent (kg/L)’
Enter ‘1.0’ in the ‘Use input density solvent (kg/L)’ field
Use ‘Kelvin’ as unit for the temperature
Enter ‘353.3’ without quotes in the ‘from:’ field
Enter ‘373.15’ in the ‘to:’ field
Change the popup menu next to Solutes from ‘Solid’ to ‘Gas’
Use ‘atm’ units for the pressure
Enter ‘1.0’ for the partial vapor pressure of benzene
Select Graph → Y Axes → solubility (mol/L solvent)
Press ‘Run’
/scm-uploads/doc.2016/Tutorials/_images/t3_solubilityinputgas.png

A graph (and table) is shown, which after some manipulations could look like:

/scm-uploads/doc.2016/Tutorials/_images/t3_solubilitygraphgas.png

The solubility of a gas in a solvent can also be calculated using Henry’s law, which is valid for ideal dilute solutions,

Select Properties → Activity coefficients
Select ‘water’ for the first component in Solvent
Click the check box ‘Use input density solvent (kg/L)’
Enter ‘1.0’ in the ‘Use input density solvent (kg/L)’ field
Use ‘Celsius’ as unit for the temperature
Enter ‘90.0’ for ‘Temperature’
Select only ‘benzene’ in the list of ‘Solutes (infinite dilute)’
Press ‘Run’

The calculated Henry constant for benzene (infinite dilute) in water will be close to 0.049 mol/(L atm) at 90 °C.

Note that for benzene in the compounds window the vapor pressure of benzene at 353.3 Kelvin was entered. If these values are not specified (if they are zero) then the vapor pressure will be approximated using only the COSMO-RS method. This is relevant for all properties where the vapor pressure plays a role, thus it is relevant for the calculation of Henry’s law constants and relevant for the calculation of the solubility of a gas in a solvent.

Step 8: Binary mixtures VLE/LLE

A phase diagram of a mixture of two components can be calculated with Properties → Binary Mixture VLE/LLE. The binary mixture will be calculated for a list of molar fractions between zero and one. This can be done at constant temperature (isothermal) or at constant vapor pressure (isobaric).

Isothermal

A binary mixture is calculated in which the pure compound vapor pressures are approximated using the COSMO-RS method.

Select Properties → Binary Mixture VLE/LLE
Select ‘water’ for the first compound
Select ‘methanol’ for the second compound
Use ‘Kelvin’ as unit for the temperature
Enter ‘298.14’ in the ‘Temperature’ field
Press ‘Run’
/scm-uploads/doc.2016/Tutorials/_images/t3_binmixinput.png

An activity coefficient plot for water(1) and methanol(2) will be shown.

/scm-uploads/doc.2016/Tutorials/_images/t3_binmixactivitycoef.png

The results of the calculation are also given in the form of a table, which shows the molar (and mass) fraction of each compound in the liquid, the activity coefficients, the activities, the temperature, the total and partial vapor pressures, the molar fraction of each compound in the vapor (y), the excess Gibbs free energy GE , the excess enthalpy HE (calculated with the Gibbs-Helmholtz equation), the excess entropy of mixing -TSE , the Gibbs free energy of mixing Gmix , the enthalpy of vaporization Δvap H (calculated with the Clausius-Clapeyron equation).

/scm-uploads/doc.2016/Tutorials/_images/t3_binmixtable.png

These values can also be shown in a graph. The property for the x- and y-axes can be selected from the ‘Graph’ Menu. For example, a graph of the excess energies can be shown by:

Select Graph → Y Axes → excess energies
/scm-uploads/doc.2016/Tutorials/_images/t3_binmixselectexcess.png

A plot of the excess energies will be shown.

/scm-uploads/doc.2016/Tutorials/_images/t3_binmixexcessenergies.png

The red curve is the excess Gibbs free energy GE , the blue curve is the excess enthalpy HE , and the green curve is -T times the excess entropy SE .

Isothermal, input pure compound vapor pressure

A binary mixture is calculated with input data for the pure compound vapor pressures. These can be, for example, experimentally observed pure compound vapor pressures. Note that the calculated partial and total vapor pressures will now depend on these input pure compound vapor pressures.

Select Compounds → List of Added Compounds
Click on the left side water
Enter ‘0.123416’ in the ‘Pure compound vapor pressure:’ field
Enter ‘322.45’ in the ‘at temperature:’ field
/scm-uploads/doc.2016/Tutorials/_images/t3_binmixpvap.png
Click on the left side ethanol
Enter ‘0.294896’ in the ‘Pure compound vapor pressure:’ field
Enter ‘322.45’ in the ‘at temperature:’ field
Select Properties → Binary Mixture VLE/LLE
Select ‘water’ for the first compound
Select ‘ethanol’ for the second compound
Enter ‘322.45’ in the ‘Temperature’ field
Select Graph → X Axes → x2: molar fraction 2
Select Graph → Y Axes → partial and total vapor pressures
Press ‘Run’
/scm-uploads/doc.2016/Tutorials/_images/t3_binmixinput2.png

A vapor liquid equilibrium (VLE) diagram for water(1) and ethanol(2) will be shown.

/scm-uploads/doc.2016/Tutorials/_images/t3_binmixvaporpressures.png

The red curve is the total vapor pressure, the blue curve is the partial water vapor pressure, and the green curve is the partial ethanol vapor pressure. One can also change the x and y axes, for example:

Select Graph → X Axes → x2, y2
Select Graph → Y Axes → total vapor pressure
/scm-uploads/doc.2016/Tutorials/_images/t3_binmixvle.png

Isothermal, miscibility gap, LLE

Water and benzene do not mix well, thus there will be a miscibility gap.

Select Properties → Binary Mixture VLE/LLE
Select ‘water’ for the first compound
Select ‘benzene’ for the second compound
Use ‘Celsius’ as units for the temperature
Enter ‘50.0’ in the ‘Temperature’ field
Enter ‘100’ for ‘Number of mixtures’

In this case a a liquid-liquid equilibrium (LLE) is calculated. The number of mixtures for which the binary mixture is calculated should be not too small, otherwise the properties of the 2 immiscible liquids phases will not be so accurate.

/scm-uploads/doc.2016/Tutorials/_images/t3_binmixmiscibilitygap.png

If the check box Graph → X axes → force 1 liquid phase within possible miscibility gap is deselected, then results will be shown in the graph and table only for those compositions of the mixture, which are outside of the miscibility gap. If the check box Graph → X axes → force 1 liquid phase within possible miscibility gap is selected, then results will be shown also within the miscibility gap, with the unphysical conditions that the two liquids are forced to mix.

Deselect check box
Graph → X axes → force 1 liquid phase within possible miscibility gap
Select check box
Graph → X axes → force 1 liquid phase within possible miscibility gap
/scm-uploads/doc.2016/Tutorials/_images/t3_binmix1liquid.png

Isobaric

A binary mixture is calculated in which the pure compound vapor pressures are approximated using the COSMO-RS method if the input values for the pure compound vapor pressures are zero. Alternative one can click a check box in the ‘Method’ Menu.

Select Method → Parameters
Click on the check box ‘use input (Compounds Menu) pure compound vapor pressures(s)’
to deselect it
/scm-uploads/doc.2016/Tutorials/_images/t3_binmixnotusepure.png
Select Properties → Binary Mixture VLE/LLE
Select ‘methanol’ for the first compound
Select ‘ethanol’ for the second compound
Enter ‘10’ for ‘Number of mixtures’
Select Isotherm, isobar, flash point → isobar
Select Graph → X Axes → x1: molar fraction 1
Select Graph → Y Axes → temperature
Press ‘Run’
/scm-uploads/doc.2016/Tutorials/_images/t3_binmixinput3.png

The calculated boiling points (may take several seconds) for a binary mixture of methanol(1) and ethanol(2) will be shown.

/scm-uploads/doc.2016/Tutorials/_images/t3_binmixtemperature.png

If one clicks in the graph window at the left or below the axes, a popup window will appear in which one can set details for the graph window. In the graph above the ‘Units’ for the ‘Left Y Axes’ were chosen to be ‘Celsius’.

Next the same binary mixture is calculated in which experimental pure compound vapor pressures are used.

Select Method → Parameters
Click on the check box ‘use input (Compounds Menu) pure compound vapor pressures(s)’
to select it
/scm-uploads/doc.2016/Tutorials/_images/t3_binmixusepure.png
Select Compounds → List of Added Compounds
Click on the left side methanol
Enter ‘1.01325’ in the ‘Pure compound vapor pressure:’ field
Enter ‘338’ in the ‘at temperature:’ field
Click on the left side ethanol
Enter ‘1.01325’ in the ‘Pure compound vapor pressure:’ field
Enter ‘351’ in the ‘at temperature:’ field
Select Properties → Binary Mixture VLE/LLE
Press ‘Run’

The calculated graph will look not very different, but it will be more accurate.

Step 9: Ternary mixtures VLE/LLE

A phase diagram of a mixture of three components can be calculated with Properties → Ternary Mixture VLE/LLE. The ternary mixture will be calculated for a list of molar (or mass) fractions between zero and one, for each of the compounds. This can be done at constant temperature (isothermal) or at constant vapor pressure (isobaric).

In this step we will use experimental boiling points as input.

Select Compounds → List of Added Compounds
Click on the left side water
Enter ‘1.01325’ in the ‘Pure compound vapor pressure:’ field
Enter ‘373.15’ in the ‘at temperature:’ field
Click on the left side methanol
Enter ‘1.01325’ in the ‘Pure compound vapor pressure:’ field
Enter ‘338’ in the ‘at temperature:’ field
Click on the left side benzene
Enter ‘1.01325’ in the ‘Pure compound vapor pressure’ field
Enter ‘353.3’ in the ‘at temperature’ field
Click on the left side ethanol
Enter ‘1.01325’ in the ‘Pure compound vapor pressure:’ field
Enter ‘351’ in the ‘at temperature:’ field

Isothermal

Select Properties → Ternary Mixture VLE/LLE
Select ‘methanol’ for the first compound
Select ‘ethanol’ for the second compound
Select ‘benzene’ for the third compound
Use ‘Mole fraction’
Enter ‘10’ for ‘Number of mixtures’
Select Graph → X Axes → x1: molar fraction 1
Select Graph → Y Axes → x2: molar fraction 2
Select Graph → Z Colormap → total vapor pressures
Select Isotherm, isobar, flash point → isotherm
Use ‘Celsius’ as units for the temperature
Enter ‘70.0’ in the ‘Temperature’ field
Press ‘Run’
/scm-uploads/doc.2016/Tutorials/_images/t3_ternarymixinput.png

The result will be a graph and a table. In the table one can find the results of the calculation at 55 (=(n+1)(n+2)/2, with n=10) different compositions. At those compositions the table shows the molar (and mass) fraction of each compound in the liquid, the activity coefficients, the activities, the temperature, the total and partial vapor pressures, the molar fraction of each compound in the vapor (Y), the excess Gibbs free energy GE , the excess enthalpy HE (calculated with the Gibbs-Helmholtz equation), the excess entropy of mixing -TSE , the Gibbs free energy of mixing Gmix , the enthalpy of vaporization Δvap H (calculated with the Clausius-Clapeyron equation).

These quantities can also be shown in the graph as a colormap, in which the color represents the value of the quantity at a certain composition. On the X axes of the graph one can choose the molar (or mass fraction) of one of the compounds, on the Y axes one can choose the molar (or mass fraction) of another compound. The molar (or mass) fraction of the third compound is then fixed, since the sum of the fractions is 1.

In this case the colormap shows the total vapor pressure:

/scm-uploads/doc.2016/Tutorials/_images/t3_ternaryvap.png

One can improve the quality of the graph by increasing the number of compositions. Note that the number of different compositions for n=20 is 231 (=(n+1)(n+2)/2).

Enter ‘20’ for ‘Number of mixtures’
Press ‘Run’

If one clicks in the graph window at the left or below the axes, a popup window ‘Graph details’ will appear in which one can set details for the graph window. If one chooses in the ‘Z Colormap’ part of this popup window as the minimum color magenta, as maximum color red, use 100 as number of colors, and change the minimum and maximum values, then the graph could look like this:

/scm-uploads/doc.2016/Tutorials/_images/t3_ternaryvap2.png

Isobaric

Note that isobaric calculations are more expensive than isothermal calculations. Thus the following example takes quite some time, since again for n=20 the number of different compositions is 231.

Select Properties → Ternary Mixture VLE/LLE
Select ‘water’ for the first compound
Select ‘ethanol’ for the second compound
Select ‘benzene’ for the third compound
Use ‘Mole fraction’
Enter ‘20’ for ‘Number of mixtures’
Select Isotherm, isobar, flash point → isobar
Use ‘bar’ as units for the pressure
Enter ‘1.01325’ in the ‘Pressure’ field
Select Graph → X Axes → x1: molar fraction 1
Select Graph → Y Axes → x2: molar fraction 2
Select Graph → Z Colormap → temperature
Press ‘Run’
/scm-uploads/doc.2016/Tutorials/_images/t3_ternarymixinput2.png

The result will be a graph and a table. Note that this may take some time, since isobaric calculations are more expensive than isothermal calculations. Click in the graph window at the left or below the axes. If one chooses in the ‘Z Colormap’ part of the ‘Graph details’ as the minimum color blue, as maximum color red, use 5 as number of colors, change the unit to Celsius, and change the minimum and maximum values, then the graph could look like this:

/scm-uploads/doc.2016/Tutorials/_images/t3_ternarytemp.png

In addition to the colormap of the temperature, an approximate miscibility gap of the ternary mixture is shown in the graph. In this case, within the miscibility gap there are two immiscible phases of the liquid in equilibrium. The composition of the two phases, which are in equilibrium, can be found at the end points of the tie line that are drawn. The calculated temperatures within the miscibility gap are calculated with the unphysical condition that the three liquids are forced to mix, thus these calculated temperatures (and other quantities) within the miscibility gap should not be used. By inspection of the graph, one can observe that the calculated minimum boiling point (azeotrope) is around 68 °C.

Step 10: A composition line between solvents s1 and s2

A phase diagram of a mixture of two solvents, which both could be mixtures, can be calculated with Properties → Solvents s1 - s2 Composition Line. The mixture will be calculated for a list of molar (or mass) fractions of the solvents between zero and one, and the compositions of solvent 1 and solvent 2 are linearly interpolated. This can be done at constant temperature (isothermal) or at constant vapor pressure (isobaric).

In this step we will try to investigate one of the tie lines of the ternary mixture of water, ethanol, and benzene in more detail. An attempt is made to use the tie line on which ends the calculated minimum boiling point is found, see the tie line which is below the black line in the next picture:

/scm-uploads/doc.2016/Tutorials/_images/t3_compositionlinestart.png

The compositions of solvents s1 and s2 are chosen where the black line in the picture above crosses the boundary of possible compositions. This means that solvent s1 and solvent s2 are mixtures of 2 compounds. Again experimental boiling points are used in the calculation.

Select Properties → Solvents s1 - s2 Composition Line
Use ‘Mole fraction’
Select ‘3 components’ in the popup menu next to Solvent
Select ‘water’ for the first compound
Select ‘ethanol’ for the second compound
Select ‘benzene’ for the third compound
Enter ‘0.0’ for the mole fraction of compound 1 of solvent s1
Enter ‘0.9’ for the mole fraction of compound 1 of solvent s2
Enter ‘0.3’ for the mole fraction of compound 2 of solvent s1
Enter ‘0.1’ for the mole fraction of compound 2 of solvent s2
Enter ‘0.7’ for the mole fraction of compound 3 of solvent s1
Enter ‘0.0’ for the mole fraction of compound 3 of solvent s2
Enter ‘100’ for ‘Number of mixtures’
Select Isotherm, isobar, flash point → isobar
Use ‘bar’ as units for the pressure
Enter ‘1.01325’ in the ‘Pressure’ field
Select Graph → X Axes → s1_x: molar fraction s1
Select Graph → Y Axes → pure compound activities
Press ‘Run’
/scm-uploads/doc.2016/Tutorials/_images/t3_compositionlineinput.png

The result will be a table and a graph.

/scm-uploads/doc.2016/Tutorials/_images/t3_compositionlinegraph.png

The activities of the pure compounds should be equal at the end point of a tie line a1 = a1 ‘,a2 = a2 ‘, and a3 = a3 ‘. If we look at the graph with close inspection this is approximately true for the molar fraction of solvent s1 with (approximately) s1_x = 0.007 and s1_x’ = 0.91. At a molar fraction of 0.91 of solvent s1 the calculated temperature is approximately 67.9 °C.

Next we will use this temperature of 67.9 °C and look at the Gibbs free energy of mixing. This will also give information about the miscibility gap.

Select Isotherm, isobar, flash point → isotherm
Use ‘Celsius’ as units for the temperature
Enter ‘67.9’ in the ‘Temperature’ field
Select Graph → X Axes → s1_x: molar fraction s1
Select Graph → Y Axes → Gibbs energy of mixing wrt pure compounds
Press ‘Run’
/scm-uploads/doc.2016/Tutorials/_images/t3_compositionlineinput2.png /scm-uploads/doc.2016/Tutorials/_images/t3_compositionlinegraphgmix.png

The black line was added to show the miscibility gap more clearly. Indeed at 67.9 °C for molar fractions between s1_x = 0.007 and s1_x’ = 0.91, the Gibbs free energy of mixing will be lower if the liquid has 2 phases.

Note, that one should use isothermal conditions, if one wants to use the calculated Gibbs free energy of mixing to determine whether there is a miscibility gap. Note also, that no miscibility gap is calculated if one uses Properties → Solvents s1 - s2 Composition Line, even if there is one, like in this case. This is because with the calculated values for only 1 composition line between 2 solvents, that involve more than 2 compounds, in general one does not have enough information to determine the exact miscibility gap.