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Chemistry has a way of bringing unsung heroes into the spotlight, and Fumaroyl Chloride ranks among these, especially for professionals who lived through the rubber and plastics revolution of the late twentieth century. Watching how chemicals like Fumaroyl Chloride shaped material sciences, I saw labs transform from places of pure experimentation to engines of practical innovation. Historical records connect Fumaroyl Chloride to the larger network of dicarboxylic acid derivatives, sharing roots with basic fumaric acid—an ingredient found both in industrial synthesis and even in trace amounts in natural processes like human metabolism. In time, chemists unlocked its potential by reacting fumaric acid with chlorinating agents, creating new pathways to specialty polymers, crosslinking agents, and custom chemical syntheses. During the 1970s and 1980s, chemists studying polyesters and fine chemicals found Fumaroyl Chloride invaluable for introducing double bonds precisely. Practical lab work, rather than theoretical design, set up many of the applications we see today.
Most folks who know Fumaroyl Chloride recognize its role as a key crosslinking and bridging molecule. This compound lines up as a trans-isomer of the diacid chloride family, sporting two reactive acyl chloride groups held across a rigid double bond. That rigidity, coming from the trans configuration of the fumarate backbone, sets it apart from its cis cousin (maleic chloride). That small tweak in geometry makes the molecule tougher and less prone to unwanted side reactions. Its chemical signature—sharp, stinging odor reminiscent of other acid chlorides—reminds every lab worker that this is a tool, not a toy. In my own lab experiences, improper handling led to hydrochloric acid vapors and harsh coughing fits, reinforcing the need for proper ventilation and PPE every time. Fumaroyl Chloride appears as a colorless or faintly yellow liquid or crystalline solid, depending on temperature and impurities. It doesn’t mix with water; it decomposes vigorously, spitting out HCl and heat. In solvents like dichloromethane or toluene, though, it dissolves easily and reacts efficiently.
Chemists handling Fumaroyl Chloride pay attention to purity and packaging much more than with everyday lab staples. For any synthesis that requires tight controls, the smallest traces of water, acids, or stabilizers can ruin a batch. My experience tells me most reputable producers ship it in amber glass or lined steel to keep sunlight and moisture out. Labels offer more than regulatory compliance—they serve as real warnings. The hazard pictograms—acid corrosion, quick deterioration—aren’t for show. A good bottle always comes with clear lot numbers, manufacturing dates, and concentration details that help trace problems if any reactions go sideways. The need for accurate, transparent labeling has increased steadily; as someone who’s dealt with mislabeled reagents causing unpredictable results, I won’t touch a bottle unless it comes from a trusted batch and is marked for high-purity work.
Old-school chemists mixed fumaric acid with thionyl chloride or phosphorus pentachloride under anhydrous conditions to create Fumaroyl Chloride. Even now, these age-old routes dominate most industrial and research settings. These reactions drive off sulfur dioxide or phosphorus oxychloride as byproducts, which brings up both safety headaches and environmental responsibilities. Over the years, green chemistry has nudged the field to look for milder reagents or recycling methods to lower waste and cost. In practice, though, the classic synthesis—where dry, carefully measured reagents meet in glass reactors with efficient off-gas handling—still rules. My own experiments with academic research teams overlooked shortcuts, sticking to the tried-and-true for reliability, especially since small variations in procedure could lead to inconsistent yields or dangerous side products.
What’s most fascinating about Fumaroyl Chloride is how its reactive sites allow endless modifications. I’ve watched organic chemists, polymer researchers, and even pharmaceutical formulating groups run into big problems and solve them with this tool. Each acyl chloride group can swap places with water, alcohols, amines, or thiols, giving rise to an amazing range of products—from polyesters and polyamides to new medicinal agents. At the benchtop level, using Fumaroyl Chloride to introduce unsaturation into a backbone or lock a molecule into a trans double bond has shaped the development of resilient, flexible plastics and strong adhesives. Those who dwell in the world of chemical process scale-up have to keep a tight grip on temperature and atmospheric moisture to keep unwanted hydrolysis in check. The reactivity that makes the compound so useful also means that every lab protocol requires discipline and respect for the scale of potential hazards.
Some chemicals baffle new students with endless alternate names, leading to mistakes and mix-ups. Fumaroyl Chloride pops up as trans-Butenedioyl dichloride, trans-1,2-Ethylenedicarboxyl chloride, and E-Butenedioyl chloride depending on the text or supplier. Seasoned professionals learn to always double-check CAS numbers and structural diagrams rather than trusting a name alone. I’ve seen synthesis go awry after a colleague grabbed maleic instead of fumaroyl variant—highlighting why clarity in naming isn’t just bureaucracy, but a real solution to lab safety and research integrity.
Handling Fumaroyl Chloride pulls no punches, even for those with decades in the field. Its volatile and reactive nature calls for gloves, goggles, lab coats, and immediate access to eyewash stations. In my working years, I saw the cost of ignoring even a few drops spilled on the bench—corroded surfaces, punctured gloves, and, in the worst cases, chemical burns. Manufacturers build storage protocols around constant containment: sealed bottles, cool and dry cabinets, and well-ventilated hoods. Emergency procedures focus on neutralizing spills, minimizing exposure, and faster-than-usual response plans. Proper training, updated MSDS sheets, and regular audits make the ultimate difference—years of running safety drills and reviewing incident logs taught me that prevention, not just paperwork, keeps chemists and facilities safe.
In industry and research, Fumaroyl Chloride has grown from a tool for producing basic esters and amides to a critical building block for high-performance polymers, advanced pharmaceuticals, specialty coatings, and agrochemical intermediates. My time consulting for plastic formulation groups opened my eyes to the way this compound fuels the creation of everything from medical implants to flexible electronics. The medical sector leans on the ability of Fumaroyl Chloride-derived compounds to crosslink biological polymers, crafting strong hydrogels and wound-sealing materials. Electronics and aerospace engineers chase its ability to toughen epoxy matrices, giving rise to lighter and more durable composites—an effort that goes far beyond textbook examples. The reach even extends into flavor and fragrance synthesis, where strict requirements for chemical purity rule all decisions. Every day, new patents and journal articles showcase innovations that rely on carefully designed reactions with Fumaroyl Chloride.
Watching grant applications and startup proposals over the years, I see a hunger for greener, more efficient uses of industrial chemicals—Fumaroyl Chloride included. Trends push innovation toward lower-waste synthesis, safer alternatives to hazardous reagents, and broader application of computer modeling for predicting reaction outcomes. Real progress happens, sometimes quietly, in university pilot plants and R&D labs where teams test how Fumaroyl Chloride might enable biodegradable plastics or smarter drug delivery platforms. The rise of click chemistry and high-throughput screening draws more eyes to old reagents, questioning whether better catalysts or alternative solvents could reduce cost and boost performance. Seasoned chemists know that direct experience—running the reactions, troubleshooting failed batches, and poring over spectroscopic data—often reveals issues textbooks miss. Practical know-how, built over years at the lab bench, keeps research grounded even as theoretical models grow ever more complex.
Fumaroyl Chloride, like many acid chlorides, punches above its weight in potential hazards. Inhaling its vapors or spilling it on skin brings out aggressive hydrolysis, sharp burns, and in some cases, long-lasting damage. I’ve known more than one researcher sidelined by careless handling, forced to relearn the importance of fume hoods and personal safeguards the hard way. Animal studies, regulatory filings, and incident reports collectively show the seriousness of its irritant and corrosive properties, pushing everyone to stay vigilant. Long-term exposure remains rare, thanks to rigorous containment and training protocols. Still, ongoing toxicity research digs deeper into chronic and downstream risks—especially for those who work intensively with this and related compounds. For those in management, it’s not about avoiding the compound altogether, but about institutionalizing a culture where safety never slips into the background.
As environmental and regulatory standards tighten, the industry’s future with Fumaroyl Chloride will be defined by how well it adapts to greener, safer manufacturing. My work organizing industry panels and workshops has shown me just how seriously both scientists and business leaders take the move toward sustainability. Advances in catalysis, circular economy thinking, and digital tracking of chemical usage offer hope for smarter resource use and better stewardship. Some universities are already testing ways to generate Fumaroyl Chloride from biobased fumaric acid, carving out a lower-carbon path. On the application side, demand for new polymers and advanced coatings ensures continued research and investment. Any progress must rest on honest dialogue—chemists, regulatory agencies, and manufacturers learning from mistakes and successes alike. Those who know this compound best understand that real advancement—efficiency, safety, and sustainability—comes from integrating hard-won lab experience with big-picture thinking.
Walk through a modern lab or peek at a list of fine chemicals, and sooner or later, fumaroyl chloride shows up. This chemical, with its trans configuration, draws a lot of attention in the world of organic synthesis. The layout of its structure—two acid chloride groups spread across a double bond—turns out to be more than just a curiosity. Chemists pick it for its ability to act as a bridge or building block, connecting molecules in ways that aren't easy with other chemicals.
Few industries push chemical building blocks harder than pharmaceuticals. Fumaroyl chloride steps up here, often serving as a reagent for making key ingredients. Drug development leans on chemicals like this for producing complex molecules with targeted effects. For instance, it helps in forming amide and ester bonds—crucial links in many new medicines. These reactions don’t just matter for new drugs; many generic medicines also owe their existence to steps involving this compound. Speed, reliability, and the precision of its reactivity give scientists more confidence during scale-up, making this substance tough to replace.
Fumaroyl chloride has found a home in making specialized polymers, especially where stability and straight-line geometry matter. Its rigid double-bonded structure creates polymers that resist bending and breaking. Manufacturers often use it to design resins and coatings with added toughness. For example, putting this chemical into the mix gives certain plastics a fire-resistant edge. The result: only specific chemicals with tight structural features—like this one—deliver these benefits.
Stepping outside the pharma bubble, other sectors use fumaroyl chloride on an industrial scale too. Agricultural companies rely on this chemical when engineering new pesticides and herbicides. It often opens the door for linking active ingredients to molecules that last longer or break down at a safer pace. Without such starting materials, companies would struggle to meet modern regulatory standards for safety and performance.
Fumaroyl chloride isn’t something you want to spill on your hands. Its reactive acid chloride groups make it hazardous, and it produces strong fumes. Handling it requires good fume hoods, personal protective gear, and sharp focus. The risks make training and engineering controls important in any workspace that uses it. Reports of eye and lung irritation aren’t rare, and the push for safer working environments keeps growing. Companies and labs respond by emphasizing closed systems and extra monitoring—not just for regulatory reasons, but also to keep their teams safe.
Chemists keep searching for ways to get the same results with fewer hazards. Some labs experiment with alternative reagents, safer solvents, or better process controls. The green chemistry movement, aiming to shrink waste and lower toxicity, nudges researchers to rethink formulas that rely on this compound. As regulations shift and safety expectations rise, new syntheses might one day push fumaroyl chloride out of the spotlight. Until then, its unique structure gives it a place among the tools that help build the medicines, materials, and crop protectants needed around the world.
Fumaroyl chloride [trans] carries the chemical formula C4H2Cl2O2. Every time I've encountered this compound, the structure stayed true to its roots in organic chemistry — a trans configuration between two acid chloride groups across a simple double bond. The molecule stems from fumaric acid, which forms the backbone for building many specialty chemicals.
In the lab, drawing out fumaroyl chloride meant sketching two chlorine atoms double-bonded to carbonyl groups. These groups then hug a central carbon-carbon double bond, forming a planar, symmetric shape. The term "trans" actually points out that the chlorocarbonyl groups stand on opposite sides of that double bond, keeping the molecule rigid and nonpolar. If you ever smell it — which, full disclosure, wouldn’t be safe — you’d pick up a sharp, biting scent typical of acid chlorides.
To spell out the structure: ClOC-CH=CH-COCl. Imagine the molecule stretched out, both chloride groups locked across from each other, never folding over. This configuration isn’t just a detail; the shape affects how the compound reacts with other chemicals and even what sort of products it can help create. I’ve seen this geometry matter when it comes to selectivity in chemical reactions, especially in synthesizing pharmaceuticals or polymers.
Sometimes a small change — even the location of a single atom — completely shifts a molecule’s properties. In industry, mistakes in the arrangement lead to unwanted side products or less efficient yields. Fumaroyl chloride [trans] offers selective reactivity and is prized for the rigidity it brings, especially for medical chemists looking to lock building blocks into a precise arrangement. There’s no trading off the trans form with its close cousin, the maleoyl chloride (cis), as that swap would open doors to entirely different polymer or pharmaceutical products. In my days running student labs, confusion between cis and trans forms often meant the difference between a clean reaction and a mess to sort out by column chromatography.
Fumaroyl chloride isn’t the friendliest compound in the stock room. It reacts quickly with water, releasing hydrogen chloride gas and forming the corresponding acid. I remember donning my thickest gloves and double-checking the fume hood, because a splash or inhalation can cause severe burns. Labs everywhere enforce tight temperature controls and keep this stuff away from any chance encounter with moisture. Training up on proper storage, air control, and emergency protocols ranks right up there with academic knowledge. For industries scaling up synthesis, investing in closed systems and automated dispensers helps protect workers. Manufacturers should also push clear, accessible hazard communication so no one ends up learning safety lessons the hard way.
Questions around health, environment, and workplace safety keep regulators and chemists alike on their toes. Acid chlorides, including fumaroyl chloride [trans], pose risks throughout handling and disposal. As interest in green chemistry rises, researchers have shifted toward alternative synthesis techniques. One promising path involves activating the same double bond in fumaric acid through enzyme catalysis or milder reagents, cutting down on hazardous byproducts and reducing the tally of dangerous intermediates. I’ve watched conference sessions where a single shift — like using safer electrophiles — meant more sustainable, worker-friendly labs without sacrificing the specificity that trans compounds like fumaroyl chloride deliver.
Fumaroyl chloride stands out as one of those chemicals that keeps even experienced lab workers on their toes. This compound pulls double duty as both a strong irritant and a reactive agent. It does more than sting eyes or skin—fumes from a small spill can start a coughing fit that doesn’t let up for hours. A friend of mine once popped open a bottle in a fume hood that wasn’t drawing strong enough, and he learned fast how sharp the pain in your throat can get from a single whiff. Bottom line: nobody ignores best practices twice.
Handling this stuff demands gloves built for chlorinated chemicals—think butyl rubber or laminated film rather than standard nitrile. I once saw a new tech grab latex gloves, and the result was burned skin within minutes and a ruined pair of gloves that melted at the fingertips. Protective goggles must fit snugly because even a light splash means an emergency eye wash trip. Lab coats aren’t just about cleanliness in this case—they actually shield arms and keep skin out of harm’s way. Since the fumes cause respiratory irritation and can trigger asthma attacks, working inside a well-ventilated fume hood isn’t optional. Some workplaces even require a full-face respirator when decanting larger volumes, because one mistake can set off a cascade of health issues.
Everybody in a lab knows not to shove all bottles into one cabinet, but with fumaroyl chloride, storage rules carry extra weight. This chemical reacts violently with water, releasing hydrogen chloride gas, so humidity control makes a big difference. I never store this one near sinks, water baths, or anywhere that’s likely to catch a spill or leak. Incompatible chemicals—anything with active hydrogen atoms, amines, or alcohols—sit in their own bins, far from the chloride shelf. The container should seal tightly, and safety data sheets even warn against opening bottles except inside a vented enclosure.
Disposing of leftovers isn’t something you eyeball. Any waste goes straight into designated hazardous waste bins, labeled with the chemical name and hazard class. Never rinse glassware or bottles into the sink—that turns a minor mishap into a major cleanup with legal consequences. For spills, a sand or soda ash barrier soaks up the liquid, preventing it from running across benches or down drains. I once watched a senior chemist act within seconds, building a quick dike so the spill didn’t reach water lines. Fast action made the difference between a contained incident and a building evacuation.
Not every workplace takes training seriously. That gets people hurt when handling something as touchy as fumaroyl chloride. Every tech and student deserves a run-through using the real safety data sheets, mock spill drills, and a clear rundown of emergency eyewash and shower locations. Too often, I’ve seen labs that skip these steps and pay the price later. Regular, hands-on sessions cut down on the sort of hesitation that turns small incidents into emergencies.
The best solution often comes from not using dangerous compounds at all. Safer alternatives can step in for many applications. Some researchers already lean toward less hazardous reagents for similar transformations. Managers and safety officers should regularly review whether traditional chemicals still serve the best interest of both research and personal well-being. For some labs, the only real fix is swapping out the risky stuff for something much less likely to turn a bad day into a trip to the emergency room.
Fumaroyl chloride packs a punch where reactivity is concerned. In my own time working with reactive acyl chlorides, I learned first-hand that neglecting proper storage never ends well. This substance gives off a biting, acidic smell and combines easily with water or humid air, releasing heat and fumes. Skin, eyes, lungs—all at risk. Chemistry only goes so far on paper; practical experience underscores the need for strong habits to avoid nasty accidents.
Every good chemist keeps a close eye on container seals. With fumaroyl chloride, airtightness means everything. Even a little moisture spells trouble, leading to corrosion or pressure buildup. I learned early on—never reuse bottles, and always dry new ones first. Glass with a PTFE-lined cap usually does the trick, but after a bad spill with an old rubber stopper, I never skimped again.
Cool, dry places beat a sunny windowsill every time. Direct sunlight speeds up decomposition and, in the worst cases, can crack glass or deform plastics. I always stored bottles in a dedicated chemical cabinet—marked as corrosive and separated from bases, water, and oxidizers. You never mix acids with bases unless you want an accident, and keeping everything labeled and separated became second nature. Anything less, and you invite cross-contamination or reactive explosions.
A cluttered lab has no place for a compound like this. Labels with clear hazard symbols matter—even late into the night or during emergencies. Once, a colleague mistook a bottle of acyl chloride for a harmless solvent. Quick thinking and a good label prevented a trip to the emergency room. Double-checking dates and hazard codes helps everyone know what’s inside, even during high-pressure moments.
Locked storage might seem like overkill, but unauthorized access leads to theft, accidents, or improper disposal. After a near-miss, we switched to cabinets with lock-and-key access. That policy kept everyone accountable. I never regretted the extra step.
Well-ventilated rooms turn potential disasters into manageable annoyances. Fumaroyl chloride’s fumes set off alarms if ventilation fails, so regular system checks matter. Personal protective equipment (PPE) like gloves, goggles, and lab coats stay close.
I never open a new acyl chloride without spill kits nearby: neutralizing agents, absorbents, and step-by-step guides for quick cleanup. Quick response limits exposure and protects everyone in the vicinity.
Stockpiling seems tempting, especially with supply chain hiccups, but holding onto large amounts only raises risks. I keep inventories lean, updating records every few weeks. Old or degraded bottles go straight into hazardous waste, handled by licensed professionals. One time, ignoring an expiration date led to broken glass and a ruined shelf. Now, we purge expired chemicals on schedule, with no exceptions.
Facts back these practices: Occupational Safety and Health Administration (OSHA) and National Fire Protection Association (NFPA) guidelines set industry standards for a reason. Following their lead saves headaches and lives. For every chemical in the lab, especially something as unyielding as fumaroyl chloride, vigilance and routine build the safest workspaces—day in and day out.
Fumaroyl chloride catches the eye of chemical manufacturers and specialists because of its double reactive chlorine groups and a sturdy, trans-alkene backbone. These features turn this compound into a handy tool for adding the fumarate structure onto larger molecules. People with experience in organic synthesis know the difference a reliable reagent can make. A bottleneck in pharmaceutical or polymer production can stall months of work, so stable reagents like fumaroyl chloride shape progress behind the scenes.
Every researcher working on small molecule drug development gets familiar with a core group of building blocks. Fumaroyl chloride belongs in this club, helping chemists form amide and ester bonds. These bonds matter. In my days speaking with process chemists, I learned that forming a robust bond with minimal fuss and waste truly helps a project. Several antifungal and anti-inflammatory drugs use fumarate linkages made using fumaroyl chloride. Its low cost and ease of handling let it scale from bench-top to industrial vats. It gives drug scientists a dependable path to make prodrugs or modify old medicines so they last longer or absorb better.
Step into a plant producing resins or specialty plastics and you notice a heavy use of fumaroyl chloride. The compound adds structural integrity to polyesters. Think construction panels, automobile interior parts, and even pipes that line industrial plants. Fumaroyl chloride doesn’t work alone, but it lets people in the field design materials that hold steady despite heat or aggressive chemicals. I’ve spoken with polymer engineers who say using this building block gives them more control over a polymer’s rigidity or flexibility. Its reactivity is key—just a hint of it in the reaction mixture can change final material properties, which matters to folks troubleshooting with customers.
Modern agricultural solutions rely on chemicals that need to function under tough conditions. Many pesticide and herbicide makers use fumaroyl chloride to tweak the molecule’s structure, swapping in fumarate groups to improve how the chemical holds up in sunlight or rain. Early in my career, I spent two growing seasons observing how certain fumigants lost power too quickly in hot fields—until formulators switched to ingredients derived from fumaroyl chloride. The changes stretched the active period by days, which helped farmers keep pests under control with fewer applications.
Workplaces focusing on performance coatings and specialty adhesives grab attention for their use of fumaroyl chloride. Flooring, electronics, and even packaging makers reach for fumarate cross-linkers to add durability and chemical resistance. As more industries search for chemical recyclability and lighter, tougher surfaces, the use of fumaroyl chloride only grows.
Using strong acid chlorides can lead to tricky handling issues. I’ve seen plant safety managers go to great lengths to keep fumes contained and to protect workers from splashes. Regulatory scrutiny around chlorine-containing compounds encourages companies to design safer processes and push for alternatives or greener waste treatment systems. Embracing good ventilation, sealed reactors, and titration-based use keeps risks in check. Forward-thinking firms also look for ways to recycle byproducts into other chemical streams, shrinking environmental impact.
As industries chase better performance, cost savings, and reduced waste, specialists keep fumaroyl chloride in their toolkit. Demand in drug, polymer, and agrochemical markets shows no signs of dipping. New research on recyclable plastics and tailored bioactive molecules means the story of fumaroyl chloride is still being written, one reaction at a time.
| Names | |
| Preferred IUPAC name | (E)-but-2-enedioyl dichloride |
| Other names |
trans-Fumaroyl chloride trans-Butenedioyl chloride trans-1,2-Ethenedicarbonyldichloride trans-1,2-Ethenedicarbonyl chloride Trans-But-2-enedioyl chloride |
| Pronunciation | /ˈfjuː.mə.rɔɪl ˈklɔː.raɪd/ |
| Identifiers | |
| CAS Number | 430-67-1 |
| 3D model (JSmol) | `JSmol` string for **Fumaroyl Chloride [Trans]** (C4H2Cl2O2): ``` ClC(=O)/C=C/C(=O)Cl ``` |
| Beilstein Reference | 1461314 |
| ChEBI | CHEBI:52217 |
| ChEMBL | CHEMBL143303 |
| ChemSpider | 532615 |
| DrugBank | DB07855 |
| ECHA InfoCard | ECHA InfoCard: 100.007.787 |
| EC Number | 208-684-2 |
| Gmelin Reference | 6769 |
| KEGG | C01500 |
| MeSH | D016229 |
| PubChem CID | 10008 |
| RTECS number | WN7878000 |
| UNII | L8K73P83C2 |
| UN number | UN2515 |
| CompTox Dashboard (EPA) | DTXSID10729221 |
| Properties | |
| Chemical formula | C4H2Cl2O2 |
| Molar mass | 163.97 g/mol |
| Appearance | Colorless to pale yellow liquid |
| Odor | Pungent odor |
| Density | 1.44 g/cm³ |
| Solubility in water | Decomposes |
| log P | 0.8 |
| Vapor pressure | 0.2 mmHg (25 °C) |
| Acidity (pKa) | -0.5 |
| Basicity (pKb) | Basicity (pKb): -1.7 |
| Magnetic susceptibility (χ) | -47.5e-6 cm³/mol |
| Refractive index (nD) | 1.5150 |
| Viscosity | 1.916 mPa·s (20 °C) |
| Dipole moment | 2.95 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 340.9 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -393.5 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -620.2 kJ mol-1 |
| Pharmacology | |
| ATC code | D08AX02 |
| Hazards | |
| GHS labelling | GHS02, GHS05, GHS06 |
| Pictograms | GHS05,GHS06 |
| Signal word | Danger |
| Hazard statements | Hazard statements: "H302, H314, H317, H319, H335 |
| Precautionary statements | P280-P261-P305+P351+P338-P302+P352-P304+P340-P310 |
| NFPA 704 (fire diamond) | 3-2-2-W |
| Flash point | 62 °C (144 °F; 335 K) |
| Autoignition temperature | 360 °C (680 °F; 633 K) |
| Lethal dose or concentration | LD50 oral rat 233 mg/kg |
| LD50 (median dose) | LD50 (median dose) for Fumaroyl Chloride [Trans]: 78 mg/kg (rat, oral) |
| NIOSH | GL2275000 |
| PEL (Permissible) | PEL (Permissible Exposure Limit) for Fumaroyl Chloride [Trans]: "No OSHA PEL established |
| REL (Recommended) | 500 mg |
| IDLH (Immediate danger) | IDLH: 3 ppm |
| Related compounds | |
| Related compounds |
Maleic anhydride Fumaric acid Maleic acid Succinic acid Phosgene |
