Dehydration reaction

Short description: Chemical reaction in which water is produced as a byproduct

This page is about chemical reactions resulting in the loss of water from a molecule. For the removal of water from solvents and reagents, see Desiccation.

In chemistry, a dehydration reaction is a chemical reaction that involves the loss of an H2O from the reacting molecule(s) or ion(s). This reaction results in the release of the H2O as water. When the reaction involves the coupling of two molecules into a single molecule it is referred to as a condensation reaction. Dehydration reactions are common processes in the manufacture of chemical compounds as well as naturally occurring within living organisms.

The reverse of a dehydration reaction is called a hydration reaction. The reverse of a condensation reaction yielding water is called hydrolysis.

## Contents

* 1 Condensation reactions occurring in living organisms
* 2 Condensation dehydration reactions in organic chemistry
* 2.1 Esterification
* 2.2 Etherification
* 3 Dehydration reactions in organic chemistry resulting in unsaturated bonds
* 3.1 Nitrile formation
* 3.2 Ketene formation
* 3.3 Alkene formation
* 4 Dehydration reactions in inorganic chemistry
* 5 References

## Condensation reactions occurring in living organisms

Condensation dehydration reactions are fundamental to the existence of life as this type of reaction produces proteins from amino acids, DNA and RNA from nucleotides, fats from fatty acids, and polysaccharides (eg. cellulose, starch, sugar, lactose) from monosaccharides (eg. glucose and fructose).

The formation of the pyrophosphate bond is an important dehydration reaction relevant to bioenergetics. Phosphorylation is a type of condensation dehydration reaction that is widely used to catalyze condensation reactions in living organisms. This phosphorylation usually involves the simultaneous dephosphorylation of ATP and therefore does not result in the release of H2O.

These reactions are all mediated by enzymes.

## Condensation dehydration reactions in organic chemistry

### Esterification

The classic example of a dehydration reaction is the Fischer esterification, which involves treating a carboxylic acid with an alcohol to give an ester

RCO2H + R′OH ⇌ RCO2R′ + H2O

Often such reactions require the presence of a dehydrating agent, i.e. a substance that reacts with water.

### Etherification

Two monosaccharides, such as glucose and fructose, can be joined together (to form saccharose) using dehydration synthesis. The new molecule, consisting of two monosaccharides, is called a disaccharide.

## Dehydration reactions in organic chemistry resulting in unsaturated bonds

### Nitrile formation

Nitriles are often prepared by dehydration of primary amides.

RC(O)NH2 → RCN + H2O

### Ketene formation

Ketene is produced by heating acetic acid and trapping the product:[1]

CH3CO2H → CH2=C=O + H2O

### Alkene formation

Alkenes can be made from alcohols by dehydration. This conversion, among others, is used in converting biomass to liquid fuels.[2] The conversion of ethanol to ethylene is a fundamental example:[3][4]

CH3CH2OH → H2C=CH2 \+ H2O

The reaction is accelerated by acid catalysts such as sulfuric acid and certain zeolites. These reactions often proceed via carbocation intermediates as shown for the dehydration of cyclohexanol.[5]

Some alcohols are prone to dehydration. 3-Hydroxylcarbonyls, called aldols, release water upon standing at room temperature:

RC(O)CH2CH(OH)R' → RC(O)CH=CHR' + H2O

The reaction is induced by dehydrating reagents. For example, 2-methyl-cyclohexan-1-ol dehydrates to 1-methylcyclohexene in the presence of Martin's sulfurane, which reacts irreversibly with water.[6][7]

Double dehydration is illustrated by the conversion of glycerol to acrolein:[8][9]

## Dehydration reactions in inorganic chemistry

Various construction materials are produced by dehydration. Plaster of Paris is produced by dehydration of gypsum in a kiln:[10][11]

CaSOA4⋅2HA2O+ heat ⟶ CaSOA4⋅12HA2O+112HA2O (released as steam).

The resulting dry powder is ready to be mixed with water to form a stiff but workable paste that hardens.

## References

1. ↑ Miller, Raimund; Abaecherli, Claudio; Said, Adel; Jackson, Barry (2001). "Ullmann's Encyclopedia of Industrial Chemistry". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a15_063.
2. ↑ Besson, Michèle; Gallezot, Pierre; Pinel, Catherine (2014-02-12). "Conversion of Biomass into Chemicals over Metal Catalysts" (in en). Chemical Reviews 114 (3): 1827–1870. doi:10.1021/cr4002269. ISSN 0009-2665. PMID 24083630. https://pubs.acs.org/doi/10.1021/cr4002269.
3. ↑ Zimmermann, Heinz; Walz, Roland (2008). "Ethylene". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a10_045.pub3. ISBN 978-3527306732.
4. ↑ Zhang, Minhua; Yu, Yingzhe (2013-07-17). "Dehydration of Ethanol to Ethylene" (in en). Industrial & Engineering Chemistry Research 52 (28): 9505–9514. doi:10.1021/ie401157c. ISSN 0888-5885. https://pubs.acs.org/doi/10.1021/ie401157c.
5. ↑ G. H. Coleman, H. F. Johnstone (1925). "Cyclohexene". Organic Syntheses 5: 33. doi:10.15227/orgsyn.005.0033.
6. ↑ J. Brent Friesen; Robert Schretzman (2011). "Dehydration of 2-Methyl-1-cyclohexanol: New Findings from a Popular Undergraduate Laboratory Experiment". J. Chem. Educ. 88 (8): 1141–1147. doi:10.1021/ed900049b. Bibcode: 2011JChEd..88.1141F.
7. ↑ Roden, Brian A. (2001). "Diphenylbis(1,1,1,3,3,3-hexafluoro-2-phenyl-2-propoxy)sulfurane". Encyclopedia of Reagents for Organic Synthesis. doi:10.1002/047084289X.rd409. ISBN 0471936235.
8. ↑ H. Adkins; W. H. Hartung (1926). "Acrolein". Organic Syntheses 6: 1. doi:10.15227/orgsyn.006.0001.
9. ↑ Katryniok, Benjamin; Paul, Sébastien; Bellière-Baca, Virginie; Rey, Patrick; Dumeignil, Franck (2010). "Glycerol dehydration to acrolein in the context of new uses of glycerol" (in en). Green Chemistry 12 (12): 2079. doi:10.1039/c0gc00307g. ISSN 1463-9262. http://xlink.rsc.org/?DOI=c0gc00307g.
10. ↑ Franz Wirsching "Calcium Sulfate" in Ullmann's Encyclopedia of Industrial Chemistry, 2012 Wiley-VCH, Weinheim. doi:10.1002/14356007.a04_555
11. ↑ Staff. "CaSO4, ½ H2O". LaFargePrestia. http://www.lafargeprestia.com/caso4___h2o.html.

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Topics in Organic Reactions

* Addition reaction
* Elimination reaction
* Polymerization
* Reagents
* Rearrangement reaction
* Redox reaction
* Regioselectivity
* Stereoselectivity
* Stereospecificity
* Substitution reaction

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