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Decane
Decane
Decane
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Decane
Skeletal formula of decane
Skeletal formula of decane with all implicit carbons shown, and all explicit hydrogens added
Ball-and-stick model of the decane molecule
Names
Preferred IUPAC name
Decane[1]
Other names
Decyl hydride
Identifiers
3D model (JSmol)
1696981
ChEBI
ChEMBL
ChemSpider
DrugBank
ECHA InfoCard 100.004.262 Edit this at Wikidata
EC Number
  • 204-686-4
MeSH decane
RTECS number
  • HD6550000
UNII
UN number 2247
  • InChI=1S/C10H22/c1-3-5-7-9-10-8-6-4-2/h3-10H2,1-2H3 checkY
    Key: DIOQZVSQGTUSAI-UHFFFAOYSA-N checkY
  • CCCCCCCCCC
Properties
C10H22
Molar mass 142.286 g·mol−1
Appearance Colorless liquid
Odor Gasoline-like (in high concentrations)
Density 0.730 g mL−1
Melting point −30.5 to −29.2 °C; −22.8 to −20.6 °F; 242.7 to 243.9 K
Boiling point 173.8 to 174.4 °C; 344.7 to 345.8 °F; 446.9 to 447.5 K
log P 5.802
Vapor pressure 195 Pa[2]
2.1 nmol Pa−1 kg−1
−119.74·10−6 cm3/mol
Thermal conductivity 0.1381 W m−1 K−1 (300 K)[3]
1.411–1.412
Viscosity
  • 0.850 mPa·s (25 °C)[4]
  • 0.920 mPa·s (20 °C)
Thermochemistry
315.46 J K−1 mol−1
425.89 J K−1 mol−1
−302.1 – −299.9 kJ mol−1
−6779.21 – −6777.45 kJ mol−1
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Flammable, moderately toxic
GHS labelling:
GHS02: Flammable GHS08: Health hazard
Danger
H226, H302, H304, H305
P301+P310, P331
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 1: Exposure would cause irritation but only minor residual injury. E.g. turpentineFlammability 2: Must be moderately heated or exposed to relatively high ambient temperature before ignition can occur. Flash point between 38 and 93 °C (100 and 200 °F). E.g. diesel fuelInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
1
2
0
Flash point 46.0 °C (114.8 °F; 319.1 K)
210.0 °C (410.0 °F; 483.1 K)
Explosive limits 0.8–2.6%
Lethal dose or concentration (LD, LC):
  • >2 g kg−1 (dermal, rabbit)
  • 601 mg/kg−1 (oral, rat)
Safety data sheet (SDS) hazard.com
Related compounds
Related alkanes
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
checkY verify (what is checkY☒N ?)

Decane is an alkane hydrocarbon with the chemical formula C10H22. Although 75 structural isomers are possible for decane, the term usually refers to the normal-decane ("n-decane"), with the formula CH3(CH2)8CH3. All isomers, however, exhibit similar properties and little attention is paid to the composition.[5] These isomers are flammable liquids. Decane is present in small quantities (less than 1%) in gasoline (petrol) and kerosene.[6][7] Like other alkanes, it is a nonpolar solvent, and does not dissolve in water, and is readily combustible. Although it is a component of fuels, it is of little importance as a chemical feedstock, unlike a handful of other alkanes.[8]

Reactions

[edit]

Decane undergoes combustion, just like other alkanes. In the presence of sufficient oxygen, it burns to form water and carbon dioxide.

2 C10H22 + 31 O2 → 20 CO2 + 22 H2O

With insufficient oxygen, carbon monoxide is also formed.

It can be manufactured in the laboratory without fossil fuels.[9]

Physical properties

[edit]

It has a surface tension of 0.0238 N·m−1.[10]

See also

[edit]

References

[edit]
[edit]
Revisions and contributorsEdit on WikipediaRead on Wikipedia

Decane

View on Grokipedia
from Grokipedia
Decane, systematically named n-decane, is a straight-chain with the molecular formula C₁₀H₂₂, consisting of a linear of ten carbon atoms connected by single bonds and saturated with atoms. It appears as a colorless, odorless at , with a of −29.7 °C and a of 174.1 °C. Decane has a density of 0.73 g/cm³ at 20 °C, is insoluble in ( <0.009 mg/L at 20 °C), but is miscible with many organic solvents such as ethanol, and its vapors are heavier than air. As a flammable liquid with a flash point of 46 °C, it is incompatible with strong oxidizing agents and can form explosive mixtures with air. Decane occurs naturally as a minor constituent in the paraffin fraction of crude oil and natural gas, comprising up to 1.8% by volume in some petroleum samples. It is produced industrially through fractional distillation of petroleum or synthesis via methods like the Fischer-Tropsch process, and serves as a reference standard for higher alkanes in fuel analysis. Key applications include its use as a solvent in organic synthesis reactions, a component in the manufacture of petroleum products, rubber, and paper, and as a surrogate fuel for studying jet engine performance and kerosene combustion due to its representation of longer-chain hydrocarbons in aviation fuels. Safety concerns with decane primarily involve its flammability and potential for aspiration hazards, with exposure to high concentrations causing central nervous system depression or skin irritation; it is classified under GHS as a flammable liquid (H226) and aspiration hazard (H304). Environmentally, it is harmful to aquatic life and degrades slowly in air via reaction with hydroxyl radicals (half-life approximately 35 hours).

Nomenclature and structure

Chemical formula and structure

Decane, particularly its unbranched form known as n-decane, has the molecular formula C10H22C_{10}H_{22} and the condensed structural formula \ceCH3(CH2)8CH3\ce{CH3(CH2)8CH3}. This represents a saturated hydrocarbon composed of ten carbon atoms and twenty-two hydrogen atoms, where the carbon chain is fully saturated with no multiple bonds. n-Decane is classified as a straight-chain alkane, featuring a linear sequence of ten carbon atoms connected exclusively by single covalent bonds (C-C), with each carbon atom bonded to the appropriate number of hydrogen atoms via single C-H bonds to satisfy valence requirements. This structure exemplifies the general characteristics of alkanes as saturated acyclic hydrocarbons, where the chain length of ten carbons distinguishes decane from shorter or longer homologues in the alkane series. In structural representations, n-decane's bond-line notation (also known as skeletal formula) is commonly illustrated as a zigzag line depicting the nine C-C bonds connecting the ten carbon atoms, with terminal methyl groups implied and all hydrogen atoms omitted for clarity. This simplified depiction highlights the unbranched, linear topology essential to its chemical identity. Decane exhibits 75 constitutional isomers in total, though the focus here remains on the straight-chain n-decane.

Naming conventions and isomers

The preferred IUPAC name for the unbranched chain isomer of C₁₀H₂₂ is decane, reflecting the systematic nomenclature for alkanes where the root "dec-" indicates ten carbon atoms and the suffix "-ane" denotes a saturated hydrocarbon. This name applies specifically to n-decane, the straight-chain structure, while branched variants receive names based on the longest carbon chain with substituents indicated by prefixes such as "methyl-" or "ethyl-". Historically, n-decane has been referred to as decyl hydride, an older term emphasizing its composition as a hydride of the decyl radical. The term "decane" in scientific and industrial contexts typically refers to n-decane unless a specific isomer is indicated, distinguishing it from the broader set of compounds sharing the formula C₁₀H₂₂. These compounds exhibit constitutional isomerism, where isomers differ in the bonding sequence of atoms, leading to varied chain lengths and branching patterns. In contrast, stereoisomerism—arising from different spatial arrangements of atoms—is absent in n-decane and most simple alkane isomers due to the lack of chiral centers or geometric constraints in acyclic structures; however, certain highly branched isomers may possess optical stereoisomers if they contain asymmetric carbons. The total number of constitutional isomers for C₁₀H₂₂ is 75, encompassing unbranched, mono-branched, and multi-branched forms. Key examples of branched constitutional isomers include 2-methylnonane, which features a methyl group on the second carbon of a nine-carbon chain, and 2,2-dimethyloctane, with two methyl groups on the second carbon of an eight-carbon chain; these illustrate how branching reduces the longest chain length while maintaining the total carbon count. Such nomenclature follows IUPAC rules prioritizing the longest continuous chain as the parent structure, with substituents numbered to yield the lowest possible locants.

Physical properties

Appearance and phase behavior

Decane is a colorless liquid at room temperature and standard pressure, exhibiting a characteristic gasoline-like odor. Under standard conditions, decane exists in the liquid phase, with a melting point ranging from -30.5 °C to -29.2 °C and a boiling point between 173.8 °C and 174.4 °C. This phase behavior reflects its nonpolar molecular structure, which limits intermolecular forces and results in relatively low transition temperatures compared to more complex hydrocarbons. The density of decane is 0.730 g/mL at 20 °C, contributing to its lower density than water and thus its tendency to float on aqueous surfaces. Its surface tension measures 0.0238 N/m, indicative of weak cohesive forces typical of nonpolar liquids. Decane is insoluble in water due to its hydrophobic nature but readily soluble in organic solvents such as ethanol and ether.

Thermodynamic and spectroscopic properties

The standard molar entropy of liquid n-decane at 298 K is 364.6 J·K⁻¹·mol⁻¹. The standard enthalpy of formation for the liquid phase is -300.9 kJ/mol at 298 K. The enthalpy of vaporization is 51.42 kJ/mol at 25 °C. The standard enthalpy of combustion for the liquid is -6778.33 ± 0.88 kJ/mol at 298 K. Infrared spectroscopy of n-decane reveals characteristic absorption bands for aliphatic C-H stretching vibrations in the 2850–3000 cm⁻¹ region, including asymmetric CH₂ stretch near 2925 cm⁻¹ and symmetric CH₂ stretch near 2850 cm⁻¹, along with weaker C-C stretching modes around 800–1000 cm⁻¹. These features are typical of long-chain alkanes and aid in structural confirmation. Proton NMR spectroscopy of n-decane in CDCl₃ displays distinct signals: a triplet at approximately 0.88 ppm (3H, terminal -CH₃ groups) and a multiplet at around 1.26 ppm (16H, -CH₂- groups), reflecting the symmetric chain structure with equivalent methylene environments in the interior. The refractive index of n-decane is 1.4102 at 20 °C. Its dynamic viscosity is 0.838 mPa·s at 25 °C, decreasing to 0.359 mPa·s at 100 °C, indicative of typical alkane flow behavior.
PropertyValueConditionsSource
Standard enthalpy of formation (liquid)-300.9 kJ/mol298 KNIST
Enthalpy of vaporization51.42 kJ/mol25 °CPubChem
Enthalpy of combustion (liquid)-6778 kJ/mol298 KNIST
Refractive index1.410220 °CPubChem
Viscosity0.838 mPa·s25 °CPubChem

Chemical properties and reactions

General reactivity of alkanes

Decane is a saturated hydrocarbon classified as an , characterized by a linear chain of ten carbon atoms connected exclusively by strong single C-C bonds, with hydrogen atoms attached to satisfy the tetravalency of each carbon. This structure results in the general formula C₁₀H₂₂, where all carbon valences are fully occupied by sigma bonds, rendering it chemically inert under standard conditions. The low reactivity of decane arises from the high bond dissociation energies (BDEs) of its C-C and C-H bonds, which require substantial energy to break. Typical BDEs for primary C-H bonds in alkanes are approximately 423 kJ/mol (101 kcal/mol), while secondary C-H bonds are slightly weaker at around 413 kJ/mol (99 kcal/mol); C-C bonds range from 335 to 368 kJ/mol (80-88 kcal/mol) depending on substitution. These robust, nonpolar bonds resist cleavage by most reagents at ambient temperatures, limiting interactions with acids, bases, or oxidizing agents. The linear structure of decane further supports stable radical intermediates during any bond-breaking events, similar to shorter alkanes. Unlike unsaturated hydrocarbons, decane exhibits resistance to addition reactions because it lacks pi bonds, precluding facile electrophilic attack. Electrophilic substitution is also unfavorable, as forming a carbocation intermediate from a saturated C-H or C-C bond demands prohibitively high activation energies, often exceeding the thermal energy available under mild conditions. Instead, alkanes like decane preferentially undergo free radical mechanisms, such as halogenation, where homolytic cleavage predominates; for instance, the activation energy for hydrogen abstraction by a chlorine radical is low, around 16 kJ/mol (3.8 kcal/mol). Reactivity trends among alkanes show minimal dependence on chain length for n-decane compared to shorter homologs like methane or hexane, as BDEs for corresponding bond types remain largely consistent—primary C-H bonds hover around 423 kJ/mol and secondary around 413 kJ/mol across the series. Longer chains like decane offer more secondary C-H sites, potentially increasing overall reaction rates in radical processes per molecule, but the intrinsic reactivity per bond is comparable, emphasizing the general inertness of the alkane class.

Specific reactions including combustion

Decane, as a straight-chain alkane, undergoes complete combustion in the presence of ample oxygen to produce carbon dioxide and water vapor, releasing significant energy. The balanced chemical equation for the combustion of one mole is: \ceC10H22+15.5O2−>10CO2+11H2O\ce{C10H22 + 15.5 O2 -> 10 CO2 + 11 H2O} This process is highly exothermic, with a standard enthalpy of combustion (Δ_c H^° ) of approximately -6778 kJ/mol. Under oxygen-limited conditions, such as in enclosed spaces or inefficient burners, decane experiences incomplete , yielding (CO) and elemental carbon in the form of , alongside . These products pose environmental and health risks, contributing to and . of decane proceeds via free radical substitution, typically initiated by ultraviolet light or heat when exposed to gas. This reaction replaces one or more atoms with , producing a mixture of monochlorinated and polychlorinated decane isomers, such as 1-chlorodecane and 2-chlorodecane. The process shows moderate selectivity, with secondary hydrogens abstracted preferentially over primary (relative reactivity ~1:3.8 per H), but still yields a distribution of products due to the abundance of both types in decane. Thermal or catalytic cracking of decane at elevated temperatures (typically above 500 °C) cleaves its carbon-carbon bonds, generating shorter alkenes and alkanes useful in processes. For instance, under supercritical conditions, decane decomposes into light olefins like ethene and propene, as well as smaller alkanes such as and , with yields depending on temperature, pressure, and catalysts. Decane also undergoes oxidation reactions relevant to its use as a surrogate, including autoignition and low-temperature oxidation pathways that contribute to engine knock in systems.

Production

Industrial production from petroleum

Decane, specifically n-decane, is primarily produced on an industrial scale through the of crude , where it emerges as part of the middle distillate fractions. Crude oil is heated in a distillation column, allowing hydrocarbons to separate based on their ; n-decane, with a of approximately 174°C, is collected in the fraction, which typically spans a of 150–275°C. This straight-run process yields decane as a mixture alongside other C9–C14 alkanes, cycloalkanes, and aromatics present in the feedstock. n-Decane occurs naturally in trace amounts in various fractions, constituting less than 1% by weight in (primarily C5–C12 hydrocarbons) but appearing more prominently in and light diesel oils, where it can reach concentrations of around 1–2% in jet fuel variants like JP-5. These fractions are derived directly from the tower, with containing 0.04–0.50% n-decane depending on the crude source and refining specifics. , used for and heating fuels, incorporates n-decane as part of its paraffin content, which overall comprises up to 25% normal and iso-alkanes in typical formulations. To obtain purer forms of n-decane for specialized applications, additional refining steps beyond initial are applied, including selective adsorption processes using molecular sieves (such as 5A type) to separate straight-chain normal paraffins from branched and cyclic hydrocarbons. These methods, often conducted under pressure, exploit the linear shape of n-decane for preferential adsorption and desorption, yielding high-purity (>99%) product streams. While and processes in refineries primarily enhance ratings in by producing branched isomers and aromatics, they indirectly support n-decane isolation by generating suitable feedstocks for further paraffin separation. n-Decane can also be produced industrially via the Fischer-Tropsch process, which converts (carbon monoxide and ) into a range of hydrocarbons, including linear alkanes like n-decane in the C9–C16 fraction, depending on catalyst and conditions. This synthetic route is used in gas-to-liquids plants to produce clean fuels from or . Global production of n-decane is not quantified independently due to its status as a minor component in bulk products; instead, it scales with overall crude oil refining, which is projected at 83.5 million barrels per day (mb/d) for 2025 according to September 2025 estimates. This ties decane output to the industry's capacity, with major producers like those in the and contributing the bulk through integrated refineries processing diverse crudes. High-purity n-decane, however, represents a segment produced by specialized chemical firms via advanced purification of distillate streams.

Laboratory synthesis methods

One common laboratory method for synthesizing n-decane involves the catalytic of 1-decene or its isomers. This reaction adds across the carbon-carbon , converting the to the corresponding under mild conditions. Typically, the process employs heterogeneous catalysts such as (Pd/C) or nickel-on-kieselguhr, with gas at elevated and moderate . For instance, hydrogenation of 1-decene using nickel-on-kieselguhr at 170°C and 500 psi yields n-decane in approximately 97% efficiency, followed by to achieve high purity. Coupling reactions, exemplified by the , provide another route for n-decane synthesis by linking shorter alkyl chains. In this method, two equivalents of 1-bromopentane or 1-chloropentane react with sodium metal in dry , forming a carbon-carbon bond to produce n-decane as the primary product, though side products like alkenes may form due to elimination. The reaction proceeds via radical intermediates, with yields varying based on halide purity and conditions; historical studies report decane formation from amyl halides with sodium, highlighting its utility for symmetrical alkanes despite limitations in scalability for longer chains. Emerging laboratory approaches include biosynthetic routes using genetically engineered microorganisms to assemble chains. These methods leverage pathways such as the acyl-ACP reductase and aldehyde-deformylating oxygenase system, originally from , heterologously expressed in hosts like to produce medium-chain alkanes from renewable feedstocks like glucose. Initial demonstrations focused on C13–C17 hydrocarbons, with further engineering enabling production of shorter chains, though specific C10 production remains limited, with titers up to several hundred mg/L through of . Following synthesis, purification of n-decane from reaction mixtures or isomers is essential for analytical or research applications. Fractional distillation under reduced pressure or at atmospheric conditions exploits the narrow boiling point range (174°C for n-decane), achieving purities exceeding 99.8 mole percent through multi-stage reflux. For higher resolution, especially from complex mixtures, column chromatography on silica gel or reversed-phase supports separates n-decane based on polarity differences, often using non-polar eluents like hexane; this technique ensures isotopic or structural purity for subsequent studies.

Applications

Solvent and chemical uses

Decane serves as a nonpolar in various industrial applications due to its low and chemical inertness, which allow it to dissolve nonpolar substances effectively without interfering in reactions. In , it is employed to facilitate reactions involving hydrophobic compounds, providing a stable medium for processes such as and initiations. Additionally, decane is utilized in the rubber industry as a for natural and synthetic rubbers, aiding in the dissolution of polymers during and steps to ensure uniform material distribution. In paper manufacturing, it functions as a aid to extract resins and impurities from pulp, improving the quality and brightness of the final product. As a , decane is incorporated into and fragrances at low concentrations, leveraging its low reactivity and minimal to dilute active ingredients without altering product scent or stability. This property makes it suitable for formulating lotions, creams, and bases where nonpolar carriers are needed to blend oils and waxes homogeneously. Decane acts as a key chemical intermediate in the production of higher-value compounds, particularly through dehydrogenation to form 1-decene, which is further processed into for detergents and emulsifiers. It also contributes to synthesis by serving as a precursor for linear alpha-olefins used in polyalphaolefin base stocks, enhancing and thermal stability in industrial oils. In , decane-derived olefins are polymerized to create and other polyolefins for packaging and coatings. Specific applications include its role as an extraction solvent and in techniques, where it aids in the separation and quantification of volatile organic compounds in complex mixtures like paints and solvents. In , decane is used as a reaction medium for handling air-sensitive compounds, such as in the suspension and manipulation of metal nanoparticles or complexes, due to its noncoordinating nature.

Role in fuels and standards

Decane, particularly its straight-chain isomer n-decane, serves as a minor but significant component in diesel and fuels, typically comprising part of the C9-C14 fraction that influences ignition characteristics. In , n-decane contributes to the , a key measure of ignition delay and efficiency, with n-decane itself exhibiting a of 76-78 as determined through experimental blending and engine tests. This value positions n-decane as a reference compound in surrogate formulations for diesel, helping to model and predict overall performance in compression-ignition engines. Similarly, in -based jet fuels, n-decane is incorporated as a surrogate component to replicate the behavior of complex distillates, given its prevalence in the lighter range of these fuels. In gasoline, n-decane occurs at low concentrations, generally less than 1% by volume (averaging 0.26% across various formulations), where it acts as a heavier-end component that modestly affects volatility and profiles without dominating the lighter fractions. Beyond fuel compositions, n-decane functions as a standardized reference in , notably in (GC) for analysis. It is routinely used as an or retention time marker in GC methods for quantifying (TPH), particularly delineating the aliphatic C10-C28 range in environmental and fuel samples. This application leverages n-decane's distinct elution behavior and purity to ensure accurate peak identification and calibration in complex mixtures. n-Decane's precisely known physical properties also make it a preferred calibration substance in thermometry and . For instance, its has been measured across wide and ranges to validate cross-correlation densimeters, achieving relative uncertainties as low as 1.1% for high-temperature applications relevant to processing. These well-characterized traits, including coefficients derived from densitometric data, support its use in calibrating instruments for quality assessments.

Safety and toxicology

Flammability and handling hazards

Decane is a highly , posing significant fire and risks due to its low of 46.0 °C and autoignition temperature of approximately 210 °C. These properties indicate that decane can ignite at relatively low temperatures from open flames, sparks, or hot surfaces, and it may self-ignite in air without an external ignition source under certain conditions. Under the Globally Harmonized System (GHS), it is classified as a (Category 3) with the hazard statement H226: "Flammable liquid and vapour," requiring appropriate labeling and safety protocols in industrial and settings. The vapors of decane are denser than air, with a vapor density of 4.9 (air = 1), which allows them to travel along the ground and accumulate in confined or low-lying spaces, potentially forming explosive mixtures with air. This behavior heightens the risk of flash fires or explosions in poorly ventilated areas. Decane is incompatible with strong oxidizing agents, which can accelerate combustion or lead to violent reactions. Safe handling of decane requires storage in cool, well-ventilated areas away from ignition sources, heat, and incompatible materials, with containers kept tightly closed to prevent vapor release. Grounding and bonding should be used during transfer to avoid static discharge. In case of fire, suitable extinguishing agents include alcohol-resistant foam, carbon dioxide (CO₂), or dry chemical; spray may be used for cooling but is unsuitable for direct application on the fire as it may spread the burning liquid.

Health and environmental effects

Decane exhibits low to moderate , primarily manifesting as to the skin and eyes upon direct contact, and it poses a severe aspiration if swallowed, potentially causing or death (GHS H304, Category 1). Dermal exposure can cause defatting of the skin, leading to dryness, cracking, or mild , while ocular exposure may result in redness, pain, and temporary . Inhalation studies in rats indicate low acute lethality, with an LC50 exceeding 5.6 mg/L over 4 hours and >1,369 ppm over 8 hours, suggesting that high concentrations are required to produce adverse effects such as or . Chronic exposure to decane is associated with potential narcotic effects and (CNS) depression at elevated levels, though the overall profile remains low. Repeated inhalation may lead to reversible neurobehavioral changes, with a (NOAEL) of 1.5 g/m³ in rats based on subchronic studies. Decane demonstrates low carcinogenic potential, with no evidence from animal or human studies indicating tumor formation, and mutagenicity data suggesting minimal genotoxic activity. Bioaccumulation of decane in organisms is limited due to its rapid metabolism via cytochrome P450 enzymes in the liver, kidneys, and lungs, primarily to hydroxylated and keto derivatives that are excreted as carbon dioxide or in urine. Its bioconcentration factor (BCF) of approximately 40 indicates moderate potential in lipid-rich tissues, but low water solubility and quick dissipation prevent significant long-term accumulation in aquatic or terrestrial biota. As a (VOC), decane contributes to atmospheric through and photochemical reactions, with an air half-life of about 9-35 hours. In environmental media, it volatilizes rapidly from surfaces (half-life 3.5 hours in rivers) and adsorbs moderately to soils and sediments (Koc ≈1,500), while being readily biodegradable under aerobic conditions, achieving 77-85.5% degradation in 28-38 days. Decane is listed on the Toxic Substances Control Act (TSCA) inventory as an active chemical substance. Occupational exposure is regulated under the OSHA (PEL) of 500 ppm (time-weighted average) for petroleum distillates, which encompasses decane, to mitigate inhalation risks.

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  45. https://www.sciencedirect.com/science/article/pii/S0378381224002292
  46. https://www.inchem.org/documents/icsc/icsc/eics0428.htm
  47. https://cameochemicals.noaa.gov/chemical/3070
  48. https://www.fishersci.com/store/msds?partNumber=O2128500&countryCode=US&language=en
  49. https://www.cpachem.com/msds?num=SB411&dnl=sd_-_n-Decane_%255BCAS_124-18-5%255D_%2528SB411%2529_%2528EU%2529.pdf
  50. https://hhpprtv.ornl.gov/issue_papers/Decanen.pdf
  51. https://www.tera.org/Peer/VCCEP/n-alkanes/VCCEP%20n-Alkanes%20Submission%20Jun%2017%202004%20-%20revised.pdf
  52. https://louisville.edu/micronano/files/documents/safety-data-sheets-sds/decane/
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