Relative volatility

Relative volatility is a measure comparing the vapor pressures of the components in a liquid mixture of chemicals. This quantity is widely used in designing large industrial distillation processes.^[1]^[2]^[3] In effect, it indicates the ease or difficulty of using distillation to separate the more volatile components from the less volatile components in a mixture. By convention, relative volatility is usually denoted as $\alpha$ .

Relative volatilities are used in the design of all types of distillation processes as well as other separation or absorption processes that involve the contacting of vapor and liquid phases in a series of equilibrium stages.

Relative volatilities are not used in separation or absorption processes that involve components reacting with each other (for example, the absorption of gaseous carbon dioxide in aqueous solutions of sodium hydroxide).

Definition

For a liquid mixture of two components (called a binary mixture) at a given temperature and pressure, the relative volatility is defined as

\alpha ={\frac {(y_{i}/x_{i})}{(y_{j}/x_{j})}}=K_{i}/K_{j}

where:
$\alpha$	= the relative volatility of the more volatile component $i$ to the less volatile component $j$
$y_{i}$	= the vapor–liquid equilibrium mole fraction of component $i$ in the vapor phase
$x_{i}$	= the vapor–liquid equilibrium mole fraction of component $i$ in the liquid phase
$y_{j}$	= the vapor–liquid equilibrium concentration of component $j$ in the vapor phase
$x_{j}$	= the vapor–liquid equilibrium concentration of component $j$ in the liquid phase
$(y/x)$	= Henry's law constant (also called the K value or vapor-liquid distribution ratio) of a component

When their liquid concentrations are equal, more volatile components have higher vapor pressures than less volatile components. Thus, a $K$ value (= $y/x$ ) for a more volatile component is larger than a $K$ value for a less volatile component. That means that $\alpha$ ≥ 1 since the larger $K$ value of the more volatile component is in the numerator and the smaller $K$ of the less volatile component is in the denominator.

$\alpha$ is a unitless quantity. When the volatilities of both key components are equal, $\alpha$ = 1 and separation of the two by distillation would be impossible under the given conditions because the compositions of the liquid and the vapor phase are the same (azeotrope). As the value of $\alpha$ increases above 1, separation by distillation becomes progressively easier.

A liquid mixture containing two components is called a binary mixture. When a binary mixture is distilled, complete separation of the two components is rarely achieved. Typically, the overhead fraction from the distillation column consists predominantly of the more volatile component and some small amount of the less volatile component and the bottoms fraction consists predominantly of the less volatile component and some small amount of the more volatile component.

A liquid mixture containing many components is called a multi-component mixture. When a multi-component mixture is distilled, the overhead fraction and the bottoms fraction typically contain much more than one or two components. For example, some intermediate products in an oil refinery are multi-component liquid mixtures that may contain the alkane, alkene and alkyne hydrocarbons ranging from methane having one carbon atom to decanes having ten carbon atoms. For distilling such a mixture, the distillation column may be designed (for example) to produce:

An overhead fraction containing predominantly the more volatile components ranging from methane (having one carbon atom) to propane (having three carbon atoms)
A bottoms fraction containing predominantly the less volatile components ranging from isobutane (having four carbon atoms) to decanes (ten carbon atoms).

Such a distillation column is typically called a depropanizer.

The designer would designate the key components governing the separation design to be propane as the so-called light key (LK) and isobutane as the so-called heavy key (HK). In that context, a lighter component means a component with a lower boiling point (or a higher vapor pressure) and a heavier component means a component with a higher boiling point (or a lower vapor pressure).

Thus, for the distillation of any multi-component mixture, the relative volatility is often defined as

\alpha ={\frac {(y_{LK}/x_{LK})}{(y_{HK}/x_{HK})}}=K_{LK}/K_{HK}

Large-scale industrial distillation is rarely undertaken if the relative volatility is less than 1.05.^[2]

The values of $K$ have been correlated empirically or theoretically in terms of temperature, pressure and phase compositions in the form of equations, tables or graph such as the well-known DePriester charts.^[4]

$K$ values are widely used in the design of large-scale distillation columns for distilling multi-component mixtures in oil refineries, petrochemical and chemical plants, natural gas processing plants and other industries.

References

^ Kister, Henry Z. (1992). Distillation Design (1st ed.). McGraw-Hill. ISBN 0-07-034909-6.
^ ^a ^b Perry, R.H. and Green, D.W. (Editors) (1997). Perry's Chemical Engineers' Handbook (7th ed.). McGraw-Hill. ISBN 0-07-049841-5. {{cite book}}: |author= has generic name (help)CS1 maint: multiple names: authors list (link)
^ Seader, J. D. & Henley, Ernest J. (1998). Separation Process Principles. New York: Wiley. ISBN 0-471-58626-9.
^ DePriester, C. L. (1953), Chem. Eng. Prog. Symposium Series, 7, 49, pages 1-43

External links

Distillation Theory by Ivar J. Halvorsen and Sigurd Skogestad, Norwegian University of Science and Technology (scroll down to: 2.2.3 K-values and Relative Volatility)
Distillation Principals by Ming T. Tham, University of Newcastle upon Tyne (scroll down to Relative Volatility)

[Kister-1] Kister, Henry Z. (1992). Distillation Design (1st ed.). McGraw-Hill. ISBN 0-07-034909-6.

[Perry-2] Perry, R.H. and Green, D.W. (Editors) (1997). Perry's Chemical Engineers' Handbook (7th ed.). McGraw-Hill. ISBN 0-07-049841-5. {{cite book}}: |author= has generic name (help)CS1 maint: multiple names: authors list (link)

[SeaderHenley-3] Seader, J. D. & Henley, Ernest J. (1998). Separation Process Principles. New York: Wiley. ISBN 0-471-58626-9.

[4] DePriester, C. L. (1953), Chem. Eng. Prog. Symposium Series, 7, 49, pages 1-43

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v t e Chemical equilibria
Concepts	Chemical stability Chelation Dynamic equilibrium Equilibrium chemistry Equilibrium stage Free energy Gibbs Helmholtz Le Chatelier's principle Phase separation Reversible reaction Thermodynamic equilibrium
Models	Equilibrium constant determination Phase diagram Predominance diagram Phase rule Reaction quotient Thermodynamic activity
Applications	Buffer solution Equilibrium unfolding Liquid–liquid extraction
Specific equilibria	Acid dissociation Hammett acidity function Binding constant Binding selectivity Coordination complexes Macrocyclic effect Dissociation constant Hydrolysis Self-ionization of water Partition Distribution coefficient Solubility Common-ion effect Vapor–liquid Henry's law

Definition

See also

References

External links