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Dimethylpyrrole’s story sits within the broader movement of heterocyclic chemistry. Many years back, organic chemists started digging into the properties of pyrroles, looking for compounds that could feed progress in materials science, dye chemistry, and pharmaceuticals. Dimethylpyrrole—basically a pyrrole ring with two methyl groups placed strategically—was crafted soon after synthetic routes for parent pyrrole became refined. The chemical structure’s stability offered practical advantages for those chasing both new molecules and improved yields. Back then, nothing guaranteed quick scale-up; researchers honed small-batch protocols in glassware, aiming to secure high purity and consistent reactivity. The drive to decorate the ring with methyl groups led to deeper looks at substitution patterns, as each tweak can nudge both reactivity and toxicity up or down. Over time, chemists learned how to control methylation—first sticking with classical catalysts, later adopting more selective and cleaner approaches. Each generation of chemists left footprints behind: shifts in preferred reagents, safer solvent swaps, and persistent work on reaction yields.
Dimethylpyrroles pop up in specialty chemicals and research labs. These compounds bring versatility, serving as building blocks for more complicated molecules. In my own experience in the lab, a bottle labeled ‘dimethylpyrrole’ signals that synthetic pathways might explore new pigment structures or medicine scaffolds. It never carries the bluster of a blockbuster chemical, but its value shows up among chemists who prize compounds that can stabilize intermediates or introduce subtle electronic effects. Methyl groups often tune properties—easing purification, decreasing side reactions, or opening new possibilities in ring chemistry. The fine line between lab-scale specialty use and broader industrial application often discourages splashy headlines, but anyone who spends time in process or research labs will recognize it as a useful stock item.
Dimethylpyrrole’s basic properties tell you what kind of handling and design issues you’ll face. The compound is a small, typically liquid or low-melting solid, depending on methyl group positions. Pyrroles themselves already come with a faint amine-like odor, and methylation tends to intensify scents. The nitrogen in the ring brings basicity—though much weaker than typical amines—along with notable electron density. Dimethylpyrroles show moderate polarity; in many cases, they stay soluble in both common organic solvents and, to some extent, polar ones. Light affects its color and stability; a clear, pale yellow color isn’t unusual for fresh samples, but exposure to air or light can darken it quickly. I’ve seen first-hand how sample handling needs special care: oxidation and polymerization aren’t just theoretical risks but real-day annoyances. This compound won’t survive months on the benchtop, especially with humidity and open air.
Labels on bottles don’t just mark a name and formula. For dimethylpyrroles, purity levels matter: trace impurities, especially those from incomplete methylation or oxidation, can change downstream outcomes. Most labs demand purity above 95 percent for synthetics or analyticals. Labels also spell out isomer identity—2,3- or 2,5-dimethylpyrrole, for instance—a critical issue for research work. Color and storage info accompany the specs, warning against direct sunlight and oxidation-prone environments. I’ve known accidents caused by ignoring such advice, turning a clear solution murky and halting progress for the day. Commercial suppliers sometimes provide spectral data, since NMR and GC-MS are the tools to quickly check authenticity in a pinch.
Synthesis hasn’t always been straightforward. Traditionally, chemists started from simple aldehydes or ketones and passed them through condensation reactions with ammonium salts to assemble the core ring. In the case of dimethylpyrrole, methyl groups might be introduced early—through methylated starting materials—or by selective methylation after ring construction. Each method has pros and cons: earlier introduction sometimes simplifies purification, but can lead to side reactions. Post-ring methylation runs the risk of overalkylation, leading to tarry materials or reduced yield. In recent years, more eco-friendly approaches have received attention—these include phase-transfer catalysis, microwave methods, or greener solvents, echoing the chemical industry’s larger shift to sustainable practices. My colleagues prioritize robust, repeatable syntheses, so new protocols get close scrutiny for cost and scalability as well.
Once you have dimethylpyrrole, it doesn’t just sit idle. The two methyl groups protect the pyrrole ring, making some sites less reactive while highlighting others for further chemistry. Alkylation and acylation often target the available positions, while the ring nitrogen opens up options for N-derivatization. In my hands, oxidative coupling of dimethylpyrrole can swing toward byproducts fast, especially without fine-tuned control of oxidant or temperature—a reminder that textbook transformations sometimes fail spectacularly at scale. Cross-coupling reactions, such as Suzuki or Heck, benefit from methyl substituents, as sterics and electronics shift outcomes in favor of desired products. Hydrogenation can break the aromaticity, but harsh conditions risk over-reduction. Each new modification lets chemists chart routes to pigments, drugs, and advanced materials—showing why this modest molecule remains a valuable chemical “chassis.”
Many chemicals wear multiple hats, and dimethylpyrrole is no exception. Depending on who’s writing, you’ll see ‘2,3-dimethylpyrrole’, ‘2,5-dimethylpyrrole’, or plain ‘dimethylpyrrole.’ In German- or French-based texts, older names still crop up—a situation that trips researchers up in database searches. CAS numbers provide more certainty. Even so, product names from commercial suppliers can stretch the truth or simplify distinctions. I always double-check the structure, not just the name, to avoid confusion between isomers. A moment reading the fine print means the difference between advancing a project or chasing a dead end caused by the wrong material.
Safety takes the front seat every time you reach for dimethylpyrrole. Volatility and reactivity give it a whiff of danger; improper storage or poor ventilation can make for an unpleasant or risky day in the lab. The molecule’s structure means it can penetrate gloves or polymer seals if you aren’t careful. Many colleagues I’ve worked with tell stories of unexpected spills or odd odors from improper capping. Labs ought to install good fume hoods and keep spill kits on hand. Avoid open flames—aromatic pyrroles can flash under the right conditions. Safety data sheets point to respiratory irritation and potential sensitization, so eye shields and gloves count as basic requirements. Waste disposal has its own headaches; pyrrole-based molecules require incineration or specialized chemical neutralization, aligning with broader environmental rules around nitrogen-rich industrial waste.
Dimethylpyrrole carves out space in several chemistry sectors. Dye chemistry leans on pyrrole rings to craft vivid, stable pigments; methylation tweaks color hues and lightfastness. Pharmaceutical discovery treats dimethylpyrroles as versatile templates: adding new substituents or chaining rings builds anti-inflammatory or antimicrobial candidates. Organic semiconductors have benefited, as methylation changes conduction band structures, offering specialized functions in thin-film electronics. In academic labs, these compounds feed curiosity, letting graduate students and postdocs push mechanisms and methods further. From my own time in the lab, dimethylpyrrole’s impact comes less from being a household name and more from its ability to bridge synthetic ambition and real materials or medicines.
Ongoing research tells a story of slow, consistent refinement. Chemists explore reactions that waste less solvent, rely on less hazardous reagents, or cut down hazardous byproducts. Better catalysts—the kind that shave hours or boost yields—rotate through the literature every year. The expanding push for renewable materials shows up here too, with work on bio-based pyrrole precursors or recyclable production protocols. Analytical teams hone faster tools for purity checks: LC-MS, NMR, fluorescence detection, each cutting hours off routine analyses. Collaboration matters—academic labs share methods, private industry tackles scale-up, and government agencies offer funding or regulatory oversight. From the outside, incremental progress looks dull, but each step brings safer, cleaner, and cheaper ways to make and use this core molecule.
Dimethylpyrrole sits in a group of molecules where safety data keeps evolving. Animal research points to modest acute toxicity, mostly through inhalation or skin contact. Chronic studies suggest that methylated pyrroles pass through metabolic pathways that break the ring, often resulting in less acute danger; but some breakdown products may carry their own hazards. The National Institute for Occupational Safety and Health and similar groups recommend careful tracking of chronic exposure. Among researchers I know, accidental splashes cause minor but memorable irritation—quick washing and airing out usually solves the problem. Still, a lack of long-term epidemiological data means unknowns linger, especially in high-volume manufacturing settings. Modern protocols require both medical monitoring and personal protective equipment, reinforcing the need for practical caution alongside scientific curiosity. Green chemistry goals nudge the community to keep pushing for alternatives that deliver similar results with even less risk.
Industries and researchers keep finding new tricks for dimethylpyrrole. Demand stays steady, buoyed by organic electronics, specialty dyes, and pharmaceutical pipelines. The move toward greener and safer synthesis won’t slow down, reshaping how future batches get made and where the waste ends up. The molecule’s flexibility—how it fits into larger chemical structures and makes possible precision tuning of materials—promises new applications in photonics and next-generation battery technology. I expect ongoing research to unlock further roles in medical imaging, agrochemical discovery, and environmental sensors. Broadening safety knowledge and sharpening production methods can only boost confidence among those putting dimethylpyrrole to work. People—whether they wear lab coats or run processing plants—will keep pushing this not-so-humble molecule into new territory.
Chemistry often hides just below the surface of daily routines. Products on shelves or the colors in packaging come from complex compounds—and one of those unsung contributors is Dimethylpyrrole. For those who haven’t heard the name, that's not surprising. It doesn’t get splashed across headlines or commercials, yet it plays a quiet role in several products and industries.
Dimethylpyrrole stands out in the world of pigment creation. Anyone who’s marveled at a vibrant red in a print or the deep tone in a piece of art couldn’t see it, but this compound helps build that! Manufacturers use it as a building block to make special dyes and pigments, especially those in the family of phthalocyanines. These complex molecules get used in printing inks, paints, plastics, and even automotive finishes. The appeal isn’t just in their color. The pigments hold up well in sunlight, giving car colors that recognizable resilience.
Researchers know the world needs safer, more sustainable options. Traditional pigments sometimes carry environmental baggage, so chemists have pivoted to exploring new ways to make intense, lasting colors without the toxic ingredients. Dimethylpyrrole brings a kind of versatility to the lab bench, and it’s not just about the shades it offers but also the stability it brings to new pigment inventions.
Looking at lab research, Dimethylpyrrole serves as a raw material to build larger, more complex molecules. Many pharmaceutical compounds begin with simple building blocks, and this compound has caught the attention of medicinal chemists. Projects aimed at discovering new drugs sometimes turn to chemical structures that include this component, trying to unlock better ways to treat disease or improve diagnostics.
In schools and universities, synthetic chemistry classes introduce students to transformations and product design using this compound. I remember making it in an undergraduate lab, amazed by how something starting as a colorless liquid would eventually help produce a pigment so strong it could stain my gloves for days.
Manufacturing any chemical comes with responsibility. Dimethylpyrrole shares the same need for care. It has a sharp odor and can irritate skin or lungs. Handling it safely—well-ventilated spaces, gloves, chemical fume hoods—remains standard in labs and factories. Accidents still happen. I remember a colleague who ignored recommendations and paid with headaches and a visit to the nurse; ignoring precautions never ends well.
Waste treatment and environmental release always stir debates. Many companies now invest in closed systems to limit exposure and emissions. Innovations in green chemistry push for less toxic starting materials and cleaner synthesis routes. Regulation also plays catch-up, with tighter limits designed to keep both workers and surrounding communities a bit safer.
Dimethylpyrrole deserves a place in stories about modern chemistry, not for glamour, but for the impact it whispers across products and industries. Good science keeps searching for ways to minimize the risks while capturing the benefits. Solutions grow from better education, tighter safety protocols, and honest reporting of both success and setbacks. The work never ends, but each step makes labs, products, and workplaces just a little safer.
Dimethylpyrrole, a member of the pyrrole family, pops up in chemical research, pharmaceuticals, and as an intermediate in dye production. Its structure sits close to that of regular pyrrole, but two added methyl groups shift its character and potential risk. A person who has handled plenty of lab solvents can tell you: just because something smells faint and looks harmless, doesn’t mean safety can sit on the back burner.
Peer-reviewed research, safety datasheets, and chemical databases agree on some basics. Skin contact with dimethylpyrrole may cause irritation or redness. Prolonged exposure could break down the skin’s natural barrier, leading to increased sensitivity. The eyes react badly too; a splash can sting and blur vision. If inhaled, the vapor may irritate nasal passages and lungs, similar to most small nitrogen-based ring compounds. Anyone handling substances like this indoors learns quickly — working near an open flame or spark becomes risky business. Pyrroles catch fire easily.
Swallowing a chemical like dimethylpyrrole isn’t part of anyone’s daily diet, and for good reason. Direct ingestion, even in small doses, can upset the digestive tract or result in more serious toxic effects. Researchers tracking toxicity levels in rodents and cell cultures found that some substituted pyrroles disrupt liver enzymes at higher doses. Chronic exposure could eventually wear down organ function, though concrete evidence on this particular variant remains limited.
Pouring dimethylpyrrole down the sink or into ordinary trash introduces risks to water tables and soil quality. As with most organic solvents, its breakdown in the environment doesn’t always run clean and fast. Bacteria and sunlight help, but full decomposition takes time. Concentrated spills threaten aquatic animals, especially those sensitive to nitrogen-containing organics. Organizations like the EPA recommend specially managed disposal — sealed containers, proper labeling, and transfer to chemical waste handlers.
Years spent working in research and teaching labs taught me a few rules to live by. Labels matter, even on small vials. Treating every bottle as a potential hazard brings fewer accidents. I remember one accident with a similar-looking solvent where a cracked glove led to mild chemical burns. Dimethylpyrrole doesn’t grab headlines like mercury or benzene, but complacency multiplies risk. Adequate ventilation, gloves, and goggles can prevent nearly every common accident. If a spill happens, absorbent pads and well-stocked eyewash stations become your best friends.
Company policies and university guidelines cover most of the right steps: replace old containers, avoid eating where work gets done, and do not mix waste streams. Training sessions scare up some eye-rolls, but a single mistake changes plans for weeks. New lab workers sometimes think small molecules like dimethylpyrrole work as stand-ins for water. Just because the danger isn’t obvious doesn’t mean you’re in the clear.
Chemicals like dimethylpyrrole serve important roles in industry and research, but respect for their hazards keeps people safe. Avoiding direct contact, wearing personal protective equipment, and following disposal instructions protect not just workers, but the environment and the wider community. People sometimes cut corners after hundreds of routine tasks, yet every year brings fresh reports of preventable injuries. Safety takes less time than recovering from an accident, and reliable information from safety authorities points out real risks instead of relying on luck or rumor. Experience proves: treating every chemical with care — even the quiet, colorless ones — pays off, every single time.
Anyone who has tackled organic chemistry remembers the first time a five-membered ring with a nitrogen atom—pyrrole—showed up in class notes. Dimethylpyrrole is just that structure with two methyl groups stuck on, replacing the hydrogen atoms on the ring. The chemical formula for dimethylpyrrole is C6H9N. This formula might seem straightforward, but it opens the door to a lot of science and industry talk that affects us far more than a simple chemistry quiz ever could. My own time in a lab taught me that a formula is just a foot in the door; the way a compound behaves, what it’s used for, and the safety steps it demands matter even more.
No one talks about dimethylpyrrole at a family dinner or brings it up for fun at coffee shops. Yet this little molecule finds its way into a surprising number of products and processes. Chemists and engineers reach for it while designing dyes, medicines, and materials that color things or help transfer light energy. It takes part in the building of porphyrins—the functional block in hemoglobin, chlorophyll, and vitamin B12. Changing two hydrogens for methyl groups might seem like a small tweak, but those changes reshape the entire way the molecule connects with others.
Researching new treatments, for instance, often needs tweaks to simple pyrrole. Adding methyl groups can help drugs get to the right place in the body or hold up longer before being broken down. Pharmaceutical companies look at each arrangement for new opportunities to treat diseases or bolster health. C6H9N as a building block hands chemists a way to tune performance and safety for drugs, pigments, or materials.
Plenty of people might imagine a chemical like dimethylpyrrole as a bubbling, mysterious flask in a movie scientist’s lab, but these compounds come with real risks in any workplace. Handling dimethylpyrrole takes respect. The nitrogen in the ring and the methyl groups change how the vapor acts or how it can react in the environment. Lab workers and plant staff need equipment that blocks fumes, gloves, and good storage—which is something I learned quickly when my own hands nearly picked up the sharp scent after a hurried, careless move at a school lab bench. Mistakes nearly always come from skipping steps or ignoring the properties listed on that bottle’s label.
Prolonged exposure to volatile organics leads to headaches, breathing struggles, or worse. Risks aren’t only about inhaling; spills and splashes threaten skin and eyes. Detailed safety sheets (SDS) break down what servers in bars often call “the fine print”—it might seem excessive until a few droplets remind you otherwise.
Knowledge travels fast in science, but sometimes best practices lag. For dimethylpyrrole and related compounds, open information sharing helps keep people safe. Industry can adopt newer sensors that spot leaks, train every user with smart drills, and move toward less hazardous alternatives where possible. Safety culture grows as more voices share lessons from real situations, not just textbook hypotheticals.
This focus—on molecules, their formulas, their roles in products, and the humans handling them—keeps the science both approachable and responsible. Talking about C6H9N as just a formula misses the fingerprint it leaves on real work and real lives. Anyone crossing paths with organics, whether in research, manufacturing, or even paint mixing, benefits from seeing beyond the skeleton drawing and staying sharp about risks and reasons for safe handling. This isn't knowledge to memorize and forget. It's part of daily life for anyone who works where chemistry meets the world.
Dimethylpyrrole doesn’t belong in the same basket as household chemicals or bulk solvents. This compound comes with its own quirks. On a practical level, it has a reputation for sensitivity to air and light. Left open to oxygen, it can oxidize, changing its chemical makeup and turning into something no chemist wants to use. Exposure to light doesn’t help; that promotes slow decomposition, kicking off side reactions that can complicate both safety and results in the lab.
I’ve worked with enough reactive organics to know that ‘cool and dry’ isn’t just a phrase people throw around to sound cautious. In my own hands-on experience, storing Dimethylpyrrole below room temperature slows down the subtle chemical changes that might otherwise slip past detection. Ideally, a refrigerator kept between 2°C and 8°C works well. Freezing isn’t needed and risks breaking glass containers, but avoiding warm shelves or windowsills keeps the chemistry honest.
The bottle itself makes a difference. Standard amber glass bottles act as shields against light and don’t react with the compound, unlike some plastics that can leach or soften. A tight-fitting cap, preferably screw-type with a PTFE liner, stops air from sneaking in. In practice, I’ve seen people transfer sensitive samples to small sealed ampoules flushed with inert gas—usually nitrogen or argon—to stretch shelf life. For non-routine users, a bottle with minimal headspace and a regular-looking desiccant packet inside can ward off moisture and keep air out, which matters because Dimethylpyrrole can absorb water vapor over time.
Look at the safety data: Dimethylpyrrole has a flash point below 110°C, making it flammable. In the real world, any workplace using this compound should keep it far from heat sources and open flames. Flammable storage cabinets earn their keep here, especially ones with fire-resistant seals and grounded doors to knock back static discharge threats. I’ve seen well-maintained labs organize their chemical shelves by hazard class, so no one finds Dimethylpyrrole next to oxidizers or acid bottles. This simple physical separation reduces both cross-contamination and the risk of dangerous reactions if spills happen.
Spills aren’t a hypothetical—people make mistakes, glass breaks, caps get misplaced. Having solid absorbents like vermiculite on hand and a clear spill kit nearby keeps panic in check. Lab training often mentions that personal protective equipment comes first, but I’ve watched enough spill drills to know gloves and lab coats, plus safety goggles, save more than clothing—especially if cleanup gets rushed.
Skipping labeling or skipping date checks builds regrets, not safety. Every bottle needs a clear date of receipt and opening, plus a hazard label. Most labs keep a running inventory, noting the expiry to ensure nobody ends up running reactions with months-old or decomposed Dimethylpyrrole. In my own record-keeping, I log the source, batch number, and even any transfers between bottles, because surprises in chemistry almost never end well.
Nobody gets trusted with sensitive chemicals without real training. Watching a mentor demonstrate the best spots in the fridge, explain why some stoppers just don’t cut it, and run through emergency plans builds the kind of habits that carry through careers. I’ve learned that the right storage isn’t just about following a checklist. It’s about understanding what the compound does, what risks it brings, and how your own storage space and habits protect both you and everyone sharing your working environment. Keeping Dimethylpyrrole safe shows respect for both the chemistry and the people using it.
Anyone who has worked with chemicals in research, manufacturing, or analysis quickly learns how much difference purity makes. Dimethylpyrrole steps into this story as a specialty chemical with strict standards. I have found that for chemical synthesis, researchers typically look for purity greater than 98%. Why? Impurities can throw off reaction results. In fields like pharmaceuticals and electronics, even small amounts of contamination spell wasted time and money. Suppliers often provide dimethylpyrrole grades at 98% or 99%, sometimes offering HPLC or GC documentation for those who need assurance.
Fresh dimethylpyrrole often pours as a transparent, colorless, or faintly yellow liquid. Problems show up as it gets older or suffers from poor storage. Exposure to air or light invites oxidation, and suddenly the liquid starts adopting a brownish hue. I once received a batch that had sat unchecked—its deep color warned me something changed inside, even before any tests. The distinctive color changes become an early warning system for degradation or contamination. Thin, watery consistency and lack of floating material tell the same story. When a chemical remains clear, without haze or sediment, most users nod in approval and get to work, confident nothing unexpected will cloud their process.
Dimethylpyrrole’s chemical backbone gives off a unique aroma that lingers in rooms long after use. People who’ve handled it recognize the scent at once. That smell sometimes acts as a quick check—in my experience, if the odor feels off, testing soon reveals a purity problem. Chemically, its structure makes it sensitive to light and air. Embedding the compound in tightly sealed containers, away from UV, saves many headaches down the road. Refrigeration can also slow the progress of natural decay, but hardly anyone leaves it on a shelf for long, not if they care about results. Small changes in color offer hints toward peroxides or other unwanted byproducts. Even before any analytical equipment steps in, a trained eye and nose often catch early warning signs.
Research, especially in organic chemistry, relies on predictable building blocks. Contaminated dimethylpyrrole throws off results and sometimes introduces unknown variables that take weeks to track down. Losing track of purity isn't just about bad luck; it sets back work schedules and budgets. Small labs need to keep sealed aliquots, while larger operations invest in air- and moisture-free handling. Maintaining logs tracing batches from arrival to use saves trouble in case a reaction misbehaves. It’s tempting to save a few dollars on a lower grade, but the risks rarely pay off. I have learned to trust suppliers that can prove consistency, and always demand certificates of analysis. When dimethylpyrrole arrives clean, clear, and traceable, everyone along the supply chain benefits—from the chemists at the bench to the manufacturers scaling up production.
Simple practices keep this compound useful. Check appearance before use. Store away from light. Only open containers in dry, controlled spaces. Rotate stock and never mix old and new. Small efforts at the storage cabinet save thousands at the workbench. Using reliable suppliers with a track record for transparency builds trust and reduces the chance of failure in the field. For anyone counting on reaction consistency, purity matters as much as any scientific technique.
| Names | |
| Preferred IUPAC name | 1,2-Dimethyl-1H-pyrrole |
| Other names |
1,2-Dimethyl-1H-pyrrole 2,5-Dimethylpyrrole 2,5-Dimethyl-1H-pyrrole NSC 41781 |
| Pronunciation | /daɪˌmiːθəl.pɪˈroʊl/ |
| Identifiers | |
| CAS Number | 2411-98-5 |
| 3D model (JSmol) | ``` 3Dmol.js?cid=93138 ``` |
| Beilstein Reference | **136186** |
| ChEBI | CHEBI:31281 |
| ChEMBL | CHEMBL317117 |
| ChemSpider | 66957 |
| DrugBank | DB08793 |
| ECHA InfoCard | ECHA InfoCard: 100.008.571 |
| EC Number | 210-792-6 |
| Gmelin Reference | 8097 |
| KEGG | C18730 |
| MeSH | D000603 |
| PubChem CID | 69783 |
| RTECS number | UJ8575000 |
| UNII | 151PN67X9C |
| UN number | UN2821 |
| Properties | |
| Chemical formula | C6H9N |
| Molar mass | C6H9N : 95.147 g/mol |
| Appearance | Colorless to yellow liquid |
| Odor | amine-like |
| Density | 0.971 g/mL |
| Solubility in water | slightly soluble |
| log P | 0.90 |
| Vapor pressure | 0.15 mmHg (25 °C) |
| Acidity (pKa) | 16.5 |
| Basicity (pKb) | 12.41 |
| Magnetic susceptibility (χ) | -62.0·10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.505 |
| Viscosity | 1.35 mPa·s (25 °C) |
| Dipole moment | 1.96 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 296.6 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -13.56 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -3113.7 kJ/mol |
| Pharmacology | |
| ATC code | Dimethylpyrrole does not have an ATC code. |
| Hazards | |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS02,GHS07 |
| Signal word | Warning |
| Hazard statements | H226, H302, H312, H315, H319, H332 |
| Precautionary statements | P210, P264, P280, P305+P351+P338, P337+P313, P370+P378 |
| NFPA 704 (fire diamond) | 1-2-0-W |
| Flash point | 30 °C (86 °F; 303 K) |
| Autoignition temperature | 215 °C |
| Explosive limits | 1.8–10.0% |
| Lethal dose or concentration | LD50 (oral, rat): 2000 mg/kg |
| LD50 (median dose) | LD50 (median dose): 400 mg/kg (rat, oral) |
| NIOSH | KK7175000 |
| PEL (Permissible) | PEL for Dimethylpyrrole is not specifically established by OSHA. |
| REL (Recommended) | 25 µg/m³ |
| IDLH (Immediate danger) | 100 ppm |
| Related compounds | |
| Related compounds |
Methylpyrrole Pyrrole Trimethylpyrrole Tetramethylpyrrole Dimethylaminopyrrole |
