Recommended Liquid–Liquid Equilibrium Data. Part 4. 1-Alkanol ...
Recommended Liquid–Liquid Equilibrium Data. Part 4. 1-Alkanol ...
Recommended Liquid–Liquid Equilibrium Data. Part 4. 1-Alkanol ...
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librium line can be described by the equation used previously<br />
for the solubility of hydrocarbons in water. This equation<br />
adopted for the monomers can be written as follows:<br />
lnN 1/n/1/T =−h 1/R, 1<br />
where N 1 is number of moles of the monomer in solution<br />
consisting of n total number of moles and h 1 is heat of solution<br />
of the monomer. The monomers are in chemical equilibrium<br />
with various associations of the alkanol. Hence, the<br />
total amount of the alkanol dissolved in water is higher than<br />
N 1 and corresponds to the total moles of alkanol n 1. Using<br />
the definition:<br />
= N 1/n 1. 2<br />
One can rearrange Eq. 1 into the following form:<br />
ln x 1/1/T =−h 1/R − ln /1/T, 3<br />
where x1 is the mole fraction of an alkanol in water along the<br />
three-phase equilibrium line. In analogy to the alkane<br />
+water systems, it is assumed that h1 depends linearly on T<br />
going through zero at some temperature T0 . Thus h1/R in Eq.<br />
3 can be approximated with the following equation:<br />
h1/R = C1T − T0, 4<br />
where C 1 is an adjustable parameter depending on alkanol.<br />
For the second term in Eq. 3, the following approximation<br />
is used:<br />
ln /1/T K = 2400. 5<br />
The approximation of Eq. 5 is valid at sufficiently low<br />
temperatures, say below 370 K. This can be seen from an<br />
analysis of the association model used in this work for LLE<br />
calculations. Equations 4 and 5 introduced into Eq. 3<br />
give, after rearrangement,<br />
ln x 1/1/T =−C 1T − T 1,min, 6<br />
where T1,min is defined by<br />
T1,min K = T0 K + 2400/C1, 7<br />
where T1,min is a temperature at which the differential in Eq.<br />
6 is equal to zero. Thus T1,min is a temperature corresponding<br />
to the minimum of the solubility of the 1-alkanol. Equation<br />
6 has the same form as the equation used for solubility<br />
of alkanes, 166 but T1,min is no longer constant as it depends on<br />
C1, which in turn depends on the number of carbon atoms of<br />
the alkanol. This explains the change of T1,min observed in<br />
alkanol+water systems.<br />
Integration of Eq. 6 gives the following equation, which<br />
describes the solubility of alkanols in water as a function of<br />
temperature:<br />
ln x1 =lnx1,min + C1fT1,min/T, 8a<br />
where<br />
fT1,min/T = T1,min/T −lnT1,min/T −1. 8b<br />
The same type of equation was used previously 166 for<br />
alkane+water systems but contrary to the alkane systems Eq.<br />
LIQUID–LIQUID EQUILBRIUM. 4 1393<br />
FIG. 3. Logarithm of mole fractions of alkanols in water ln x 1 vs temperature<br />
T. Experimental points and approximating curves calculated with Eq.<br />
11 with parameters defined by Eq. 12.<br />
8a when applied for alkanols is valid only at temperatures<br />
sufficiently distant from the critical temperature of solubility.<br />
It was found that all investigated 1-alkanol+water systems<br />
can be approximated simultaneously with Eq. 8a provided<br />
that the adjustable parameters ln x 1,min and C 1 are treated as<br />
linear functions of the number of carbon atoms, N c<br />
ln x 1,min = d 1 + d 2N c, 9<br />
C 1 = d 3 + d 4N c. 10<br />
Equations 9 and 10 allow rewriting Eq. 8 in the form:<br />
ln x1 = d1 + d2Nc + d3 + d4NcfT1,min/T. 11<br />
The coefficients d1, d2, d3, and d4 in Eq. 11 as well as T0 in<br />
definition 7 were determined by simultaneous regression of<br />
the experimental data for normal 1-alkanols from 1-pentanol<br />
to 1-hexadecanol at at temperatures from the freezing point<br />
of water to approximately 60 K below the critical temperature<br />
of solubility. Altogether 242 experimental points were<br />
used in the regression. After the regression the most outlying<br />
point was removed and the remaining points were regressed<br />
once more. This procedure was repeated until the deviation<br />
of the most outlying point in the remaining data set did not<br />
exceed three times the estimated standard deviation. This<br />
procedure removed 22 of 242 initial points. The following<br />
values of the parameters were obtained:<br />
d1 = 1.249, d2 = − 1.365, d3 = 7.7, d4 = <strong>4.</strong>2,<br />
T 0 /K = 246.<strong>4.</strong> 12<br />
Equation 11 works well up to 60 K below the critical<br />
temperature of solubility T 2c as is shown in Fig. 3 but the<br />
data above the boiling point of water were reported only by<br />
one source with exception of pentanol. For the higher alkanols<br />
shown in Fig. 4, there are no measurements at high<br />
temperatures. Therefore it is concluded that reliability of Eq.<br />
11 is not sufficiently tested at T373 K.<br />
It was found that Eq. 11 with parameters defined by Eq.<br />
12 can also be applied for branched 1-alkanols provided<br />
J. Phys. Chem. Ref. <strong>Data</strong>, Vol. 35, No. 3, 2006