vapor liquid coexistence and critical behavior
TRANSCRIPT
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VAPOR-LIQUID COEXISTENCE AND
CRITICAL BEHAVIOR OF IONIC LIQUIDS
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ABSTRACT
Ionic Liquids are salts that are liquid near ambienttemperatures.
Experimental determination of critical points and vapor-liquidcoexistence curve is not possible because of thermal stabilityissues as most Ionic Liquids decompose before reaching thecritical point.
The paper reports the first vapor-liquid phase diagram andcritical point for ionic liquids obtained in silico with an atomisticforce field.
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IMPORTANCE OF VLE
VLE gives the nature of intermolecular interactions present inthe liquid and vapor phases.
Useful in developing equations of state and correspondingstate theories
Knowledge of critical points and VLE are key to achievingfundamental understanding of these complex fluids.
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IONIC LIQUID UNDER STUDY
Molecular structure of ionic liquid under study
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EXPERIMENTAL PROBLEMS
Conflicting experimental reports of the way in which propertiessuch as vapor pressure and enthalpy of vaporization vary withfactors such as size of cation, aggregation of ions etc
Most of the experimental uncertainty is due to the pressurebeing too low and temperature being high which makesmeasurements extremely difficult to conduct as even traceamount of impurities can cause a large variations inmeasurements.
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SIMULATION STUDIES
Simulation method used here is Gibbs Ensemble MonteCarlo(GEMC).
Drawback: Reliance on particle exchanges between vapor andliquid phases to equilibrate the chemical potential butconfigurational bias Monte Carlo and other enhanced
sampling techniques are used to circumvent this problem.
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GEMC
Configurational Bias sampling, Parallel computing strategiesand enhanced bias sampling specifically designed for ionicsystems were used to enhance the efficiency.
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COMPUTED VLCC AND CRITICAL POINTS
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ANALYZING VLCC
Compared to non-ionic compounds like alkenes, the VLCCshave a high degree of Asymmetry with a very steep vaporbranch similar to alkyl halides
Effect of a single methylene groupo Critical Temperature decreases with increasing alkyl chain,
Tc decreases by 65K in going from C2 to C6. For alkanesand Alcohols the Tc increases with increasing alkyl chain.
o Critical Density decreases with increasing alkyl chain.
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CRITICAL TEMPERATURE, METHYLENEINCREMENT
It is unclear whether Tc will decrease with increasing chainlength will hold true after C6.
When the chain length becomes very long , it is possible thatthe columbic screening due to alkyl chain becomes saturatedwhile the van der walls interaction due to increasing chain
length continue to increase the cohesive energy, so it ispossible that this trend of decreasing critical temperature withchain length might reverse after certain Cn
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PRESSURE PLOT
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ANALYZING PRESSURE PLOT
Increasing cation alkyl chain length increases the VaporPressure, thus lowering the normal Boiling Point.
One Plausible explanation is increasing the nonpolar contentof the cation weakens the Columbic interaction between ions,resulting in increased volatility
Critical pressure can be computed using critical Temperatureand subcritical saturation pressure.
For ionic Liquids, Pc decreases with increasing alkyl chainlength
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ANALYZING PRESSURE PLOT
Critical compressibility factor (Zc) ranges from 0.038[C1] to0.049[C6]
Zc smaller than simple fluids suggesting highly nonidealbehavior of vapor phase.
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TEMPERATURE DEPENDENCE OF ENTHALPYOF VAPORIZATION
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TEMPERATURE DEPENDENCE OF ENTHALPYOF VAPORIZATION
At high Temperatures, Hvap decreases with increasing sizeof cation, while at lower temperatures Hvap increases withincreasing size of cation.
The Trend reversal maybe due too Significant aggregation in the vapor phaseo Effect of alkyl chain on cohesive energy of condensed
phase upon increasing temperature.
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TEMPERATURE DEPENDENCE OF ENTHALPYOF VAPORIZATION
Hvap ranges from 68-72 KJ/mole which is twice the value ofa H2 bonding liquid like ethanol but lower than energy reqd todissociate.
This suggests that vapor phase exists as ion pairs or largeaggregates and not isolated ions.
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ASSOCIATION IN VAPOR PHASE
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ASSOCIATION OF IONS
Trountons constant for ionic liquids is ~65 J/mol K which islower than nonpolar(~85 J/mol K) and polar (~105 J/mol K).
Associating Liquids like acetic acid also have low Trountonconstants
Significant aggregation of ions in vapor phase lowers the
vapor phase entropy relative to typical fluids where vaporphase consists mainly of isolated molecules.
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CLUSTER ANALYSIS
Cluster analysis performed to address the issue ofaggregation of ions.
2 ions considered part of cluster if their center of mass ofseparation
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DISTRIBUTION OF CLUSTER SIZES AS AFUNCTION OF TEMPERATURE
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TEMPERATURE DEPENDENCE OF IONS INCLUSTER OF SIZE N(AGG)
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AGGREGATION OF IONS
Less than 0.2% of ions are isolated. Single ion pairs account for more than 60% of total clusters. Number of single-ion pairs decreases with increasing
temperature. Number of larger clusters increases with temperature.
Even though individual ion pairs are dominant species in thevapor phase, substantial fraction of ions is present in largeraggregates. This might be the reason for discrepanciesobserved between different experimental techniques.
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CONCLUSION
VLE of Ionic Liquids differs from conventional molecular liquidsbyo Shape of VLCC is highly Asymmetricalo Vapor pressure increases as size of cation increases.o Critical density and temperature decreases as size of
cation increases.o Trountons constant is smaller than that of conventional
fluids, consistent with finding that vapor state consists ofsignificant fraction of aggregated ion pairs.
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REFERENCES
Vapor Liquid Coexistence and critical behavior of Ionic liquids via Molecular Simulations,Neeraj Rai and Edward J. Maginn*
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