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The chemical industry has always thrived on new catalysts and initiators. Bis(4-Chlorobenzoyl) peroxide, part of the organic peroxide family, made its entry in the post-war era, riding on a wave of advances in polymer science and synthetic chemistry. Early work focused on improving polymer yield and controlling reaction rates in processes dominated by high pressure and unpredictable kinetics. Chemical titans eyed this compound not just for its ability to kickstart chain reactions but also for its halogenated structure, which offered unique reactivity compared to its simpler cousins like benzoyl peroxide. As a result, manufacturers started using it extensively in specialty polymer production and select oxidative processes. Even today, tracing a lab notebook’s scribble from the sixties, the compound's footprint is clear: chemists leaned on it when classic initiators fell short, especially in scenarios calling for a reliable source of free radicals with a chlorine twist on their action.
From a product perspective, this compound usually appears as a powder or granular solid with a useful, though somewhat limited, content window capped at 77%. Maintaining content below that mark isn’t arbitrary; it’s about balancing strength and safety. Anyone who’s handled peroxide initiators for a living knows storage isn’t the main headache—stability during actual use is. Peroxides, by nature, walk a fine line between being robust enough to spark the reaction and not so unstable that they ignite on a humid day. Chlorination adds another challenge, often making the compound more reactive and more of a handful during shipping or long-term warehouse storage. Many technical teams learned this the hard way, giving rise to tight content specifications and strict temperature ranges during transport.
Open a bottle of Bis(4-Chlorobenzoyl) peroxide, and you’ll find a white to off-white powder that gives off a faint, sometimes pungent, odor. Its melting range hovers around the relatively low marks common among organic peroxides, which is a double-edged sword for process chemists. Too low, and you’re looking at runaway decomposition. Too high, and the initiator loses its ready-to-go charm. This compound stands out due to its double benzoyl structure, each ring adorned with a para-positioned chlorine atom. That feature stacks on extra electron-withdrawing power, making the molecule both eager and slightly more dangerous as a source of radicals. Solubility marks another consideration; it mingles better with certain organic solvents than with water, demanding expertise when adding to reaction vats. Both in bench chemistry and industrial systems, the peroxide’s decomposition profile, combined with those chlorine atoms, can lend itself to chain reactions not achievable with plainer molecules.
Regulators and producers don’t shrug off technical specs. One glance at the packaging and you see hazard pictograms and the familiar red-framed labeling—warning handlers about both explosive risks and toxic decomposition products. Labs and factories must manage stricter quality controls to keep impurities and content in check, a lesson hammered into any operations manager’s head after seeing what happens if thresholds slip. Units typically package it under inert atmospheres, with cooling packs if shipping over long distances. Documentation, MSDS sheets, and batch certificates may not make thrilling reading, but they exist for a reason. In industrial settings, process engineers tweak dosages based on the content heights, running regular tests to ensure that the content doesn’t drift above safe levels, especially since organic peroxides have a notorious habit of breaking down faster than the paperwork can keep up.
The journey from raw 4-chlorobenzoic acid to final peroxide follows a careful path. Through acyl chloride formation and subsequent reaction with hydrogen peroxide, the process walks a careful balance between conversion and control. Yield matters, but safety matters more. Anyone who’s run such syntheses knows that reaction runaway isn’t a theoretical risk; it’s something every team member trains to avoid. Homemade chemistry and shortcuts have no place here. Commercial routes prioritize slow addition, rigorous temperature monitoring, and, in some cases, in-line quenching—a reminder that, even in a highly automated plant, experience trumps automation when handling peroxides. More forward-thinking firms pump significant resources into process flow equipment, aiming to minimize operator exposure while holding tight on thermal runaway risk.
Bis(4-Chlorobenzoyl) peroxide doesn’t just start free-radical polymerizations or cross-link polyethylene; it acts as a workhorse in specialty elastomer synthesis and oxidative steps where precision matters. I’ve watched teams explore how those para-chlorines change polymer microstructure—everything from branching density to molecular weights. In research circles, this compound shows promise in controlled radical polymerizations, where initiator performance translates directly into product properties. Some labs focus on further modifications—trying to tweak the basic molecule with other ring substituents or using it as a template for custom initiators. Data from academic journals show how that small structural shift defines reactivity and, by extension, final material performance, guiding a new generation of controlled polymer production.
You won’t always see “Bis(4-Chlorobenzoyl) peroxide” on ingredient lists or shipment invoices. Synonyms range from 4-Chlorobenzoyl peroxide dimer to simply chlorinated benzoyl peroxide. Commercial suppliers add their tradenames, usually combination codes or shortened forms, though savvy chemists quickly learn manufacturers often substitute among close cousins depending on sourcing issues or price swings in upstream chemicals. For regulatory tasks, knowing synonyms helps ensure compliance—since a mislabel can delay shipments and upend production lines.
Day-to-day, workers respect Bis(4-Chlorobenzoyl) peroxide because mistakes can cost lives or cripple plants. Unstable peroxides evoke caution—rightly so, given well-documented incidents of fires and explosions in facilities that underestimate storage temp or ignore contamination risks. Direct contact, inhalation, or improper handling produce both acute and chronic health effects, including corrosive burns and respiratory issues. Experienced plant managers rely on strict PPE guidelines, double-insulated storage drums, and real-time temperature monitoring. Oversight from agencies like OSHA isn’t paperwork; it’s a reflection of hard-earned experience. Ongoing training, regular drills, and both label clarity and redundancy cut accident rates. Safe transfer systems and continuous video monitoring aren’t technology for technology’s sake; they wrap layers of precaution around every stage from delivery to disposal. Waste streams get neutralized under watchful eyes, not casually dumped.
Polymers gain new functionality and reliability from initiators like Bis(4-Chlorobenzoyl) peroxide. The PVC and rubber industries, for instance, depend on precisely-tuned radical initiators to shape molecular structure—everything from tensile strength to resistance against harsh weather. In electronics and adhesives, adding this compound to the recipe can mean the difference between a brittle bond and a flexible seal. My time in industrial R&D made clear: even a minor change in initiator dosage or purity feeds directly into product defects or recalls. That’s why in automotive parts, construction membranes, and specialty coatings, experienced engineers spend years optimizing recipes for both safety and performance. As downstream users demand less-toxic alternatives and tighter emissions controls, application scientists experiment with novel blends, recycling methods, and more sustainable production cycles—many built around lessons learned with chlorine-containing peroxides.
Academic and private research focus heavily on improving both the efficiency and the safety profile of Bis(4-Chlorobenzoyl) peroxide. Research teams model the molecule's decomposition path, probing ways to modulate energy release and radical yield. There is an ongoing push for dual-function initiators—compounds that not only kickstart reactions but also impart unique features to end products. Researchers examine microencapsulation techniques to stabilize peroxides or develop carrier systems that release initiator only when specific conditions arise, sharply reducing workplace hazards. Publications appear yearly on routes to recycle or detoxify spent peroxide residues, recognizing the environmental footprint. At the same time, collaborations between academia and industry test greener manufacturing protocols, using safer solvents or renewable feedstocks.
Toxicity research around Bis(4-Chlorobenzoyl) peroxide never slows down. Studies circle around its decomposition products, particularly those containing chlorinated aromatics. Lab animal tests and workplace exposure reports linked high exposures to respiratory and skin irritation, plus concerns over possible mutagenicity or long-term health effects. Regulators and industry leaders take cues from this toxicology data, updating permissible limits and best practices every few years. In my experience, many firms go above regulatory minimums out of both liability fear and corporate conscience. There’s an evolving attitude, one that rewards early adoption of safer chemical practices and transparent reporting of exposure incidents. Regular investment in better monitoring—both environmental and biological—now factors into every corporate strategy session.
The next chapter for Bis(4-Chlorobenzoyl) peroxide isn’t just about tweaking content or effluent treatments; it’s a chance to reimagine how high-powered initiators fit into cleaner, more circular chemical economies. As new regulations limit hazardous emissions and push for green chemistry, R&D centers target new catalysts that maintain performance with lower toxicity. Some look toward bio-based alternatives, others invest in purification schemes to reduce contaminants that exacerbate hazard. Stakeholders recognize that stewardship now underpins not just regulatory compliance, but brand value and consumer trust. Forward-looking firms encourage knowledge-sharing, lean on collective global experience, and stay nimble as novel risks and opportunities emerge. Progress depends as much on transparent conversation—between labs, regulators, and the public—as it does on technical achievement, setting a higher bar for safety, efficacy, and environmental mindfulness around this ever-relevant chemical.
Bis(4-Chlorobenzoyl) peroxide plays a straight-up crucial role in manufacturing many plastics we use every day. In polymer chemistry, this compound starts chain reactions that turn small molecules into the polymers forming products like PVC pipes, vinyl floors, and sealants. I’ve seen firsthand how the quality of the final polymer hinges on picking the right initiator. This peroxide helps control the reaction speed and affects the properties of the end product. In practice, small changes in the peroxide’s quality can shift the strength, color, or heat resistance of the final plastic in a big way.
Manufacturers rely on bis(4-chlorobenzoyl) peroxide to create resins found in specialty paints, coatings, and inks. Imagine a glossy finish on a car or the smooth, resilient topcoat on a kitchen countertop—these rely on complex polymers kicked off by peroxides like this one. In my experience with coating applications, the stability and performance under heat or sunlight boil down to how well these byproducts of the curing process are managed. Improper mixing or handling can result in bubbles, weak spots, or yellowing, which can ruin a high-value batch. The attention to detail with initiators directly links to the durability and appearance of what ends up in a showroom or inside someone’s home.
Rubber goods that demand toughness, like industrial gaskets or high-performance tires, get their structure from crosslinking processes. Here’s where bis(4-chlorobenzoyl) peroxide steps in. By bonding together long chains of rubber, it builds resistance to heat and solvents, which ordinary rubber can't handle. From my work on site at a tire plant, even minor tweaks to the peroxide dose determine whether a batch stays flexible or becomes brittle. Safe handling matters, too—this chemical can break down violently if misused. Facilities benefit from strict controls and clear training to keep workers and products safe.
In thermoset plastics—those used for electronics casings, appliance parts, and structural panels—bis(4-chlorobenzoyl) peroxide promotes a quick, thorough cure. Unlike thermoplastics, thermosets won’t remelt, so full crosslinking is key for strength and stability. I’ve been on teams where a slow or uneven cure wasted thousands of dollars in scrapped panels. Consistent initiation from this peroxide streamlines production and cuts losses. This benefit matters even more as companies look to boost productivity and lower energy use.
While effectiveness draws manufacturers to this peroxide, its reactivity makes safe handling central. Storage requires cool, dry places. Spill protocols stay at the ready. Reporting from the field points to rare, but dangerous, incidents if shortcuts get taken. Companies can adopt better ventilation, fire suppression, and real-time monitoring of temperature and pressure. Substituting with less hazardous initiators, when possible, continues to gain ground, but in tough or high-spec jobs, bis(4-chlorobenzoyl) peroxide remains a top pick.
Bis(4-chlorobenzoyl) peroxide stands at the crossroads of productivity, product performance, and workplace safety in advanced plastics and rubber. Experience on the ground shows that with smart controls, training, and ongoing chemical research, industries can keep using this powerful material while putting worker safety and environmental responsibility first.
Chemical safety isn’t something reserved for labs and factories. Plenty of folks keep chemicals in places they don’t think twice about. I’ve seen a mechanic store solvents in old soda bottles under a cluttered workbench. I’ve seen cleaning supplies shoved next to food in kitchen pantries. Ask any firefighter, and they’ll tell you about dangerous surprises in garages and sheds.
People underestimate the risks these substances carry. Many chemicals release toxic fumes or can catch fire with just a spark. A leaky cap or a careless shove can turn a harmless-looking bottle into an emergency. Without the right storage and handling steps, even routine activities become dangerous.
Experience shows that original containers work best. Manufacturers design these bottles and drums to withstand the chemical inside, plus they label them with crucial information—hazards, expiration dates, and emergency directions. Transferring chemicals into random jars or bottles causes confusion and increases the risk of accidents. Labels peel off, and nobody remembers what “yellow stuff” means a year later.
Most chemicals stay stable in cool, dry, and well-ventilated spaces. Humidity can corrode containers, and mixing products with water sometimes triggers reactions. Sunlight can break down certain compounds or weaken plastics, so stash containers out of the sun. A garage shelf away from heat sources works better than splitting storage between a soggy basement and a hot attic.
Never stack incompatible chemicals together. Bleach and ammonia don’t mix in any sense of the word; their fumes prove dangerous when combined. Pesticides, acids, and oxidizers all need separate lockers or bins. Some warehouses color-code storage areas. Home users can at least sort products with simple, clear dividers.
Handling chemicals safely starts well before a spill or splash. Gloves—nitrile or neoprene work for most non-acidic products—protect skin from burns and irritation. Goggles shield eyes from clouds, splatters, or powder, which can cause vision damage in seconds. Throw in a cotton apron and solid shoes to keep mishaps minor.
Ventilation matters more than most folks realize. Vapors from paints, solvents, or pool chemicals linger in closed spaces and can send you reeling long before anyone smells trouble. Cracking windows, running a fan, or stepping outside for mixing jobs makes a real difference. For confined spaces like utility rooms, even a small exhaust fan lines up with best practice.
A routine helps avoid mistakes. Check labels for hazards at least twice a year—or every time you clean out the shelf. Toss anything past its expiration or with a rusted cap. Keep an emergency spill kit on hand: baking soda, sand, or kitty litter works for most small spills. Never wash chemicals down drains or toss them in the trash without checking local disposal rules.
Training shouldn’t be reserved for workplaces. Every home relies on cleaners, fuels, and pest control products that can cause harm. Digital guides, short safety workshops, or even a simple chat in the family group can raise awareness. Educators say real-life examples stick better than long safety sheets, and personal stories often convince more than warning signs alone.
Taking the time to respect chemicals protects people, pets, and property. Common sense, a few good habits, and basic information draw the line between safe work and preventable disaster. The difference between disaster and routine really does come down to attention, not equipment.
Bis(4-Chlorobenzoyl) Peroxide shows up in a range of manufacturing settings, mostly as an initiator in the production of polymers and certain resins. The name probably won’t ring bells for most folks, but those working in chemical plants, labs, and quality control definitely know its quirks—and risks. For someone who’s spent years near the sharp end of a lab bench, understanding what’s in the air, on your gloves, or riding on your coveralls becomes more than routine—it’s survival.
Let’s get real. This is a peroxide—the chemical group famous for power-packed oxidizing strength. The first clue about hazard comes straight from experience: power means reactivity. Bis(4-Chlorobenzoyl) Peroxide doesn’t play nice if it heats up, gets contaminated, or hangs around with flammable materials. Old stories from factory floors—white dusts going up in smoke, surprised engineers blowing fire extinguishers—keep folks alert.
Direct exposure brings its own mess: rashes from skin contact, red eyes, wheezing or shortness of breath for those who catch a whiff, especially in spaces without enough fresh air. The product’s Safety Data Sheet points to skin and eye irritation and flags a moderate inhalation risk. No fun. Where I used to work, someone always had a bottle of saline and a shower ready in the corridor. Once, a rookie forgot to close a lid and spent the rest of the week under the watchful eye of our plant nurse, learning what it means to respect the rules.
Concentration matters. Below 77%, this substance becomes less twitchy—less likely to kick off a runaway fire or explosion. Still, it’s a chemical you never call “safe” on a whim. Storage has to be cool and away from sunlight, heat, or random debris. Every year, I’ve seen inspectors double-check stock rooms for the right labeling, segregated spaces, and working fire suppression measures. Sloppy habits—like tossing containers near exits—can turn an ordinary day into a full-blown emergency. Nobody forgets the lessons learned when someone gets burned.
Offsite, the risks continue. Imagine workers carrying powder on their clothes or tools. Wash stations and strict “clean in, clean out” routines limit the spread. Good ventilation stands between a healthy workforce and a string of respiratory complaints. More than once, packing tape and plastic sheeting saved the day when the extractor fan died—until the maintenance crew fixed the system for good.
Plenty of research papers—some I’ve pored over during long shifts—call for gloves, goggles, and lab coats as the baseline defense. Respirators come out if dusts go airborne. But tools can’t stand in for sound habits. Regular safety drills, real-world incident reviews, and honest reporting build a culture where nobody takes shortcuts. After one minor incident years ago, our team set up informal “five-minute check-in” meetings every morning, swapping stories and tips to stay safe without sounding like robots reciting a manual.
Clear labeling, good record-keeping, and strong communication with every layer of staff, from janitors to supervisors, cut risks sharply. Outsiders—contractors, delivery crews—need proper induction too. The point isn’t just to tick boxes; it’s to go home at the end of the shift with nothing worse than a tired back. Nothing beats that peace of mind.
Bis(4-Chlorobenzoyl) Peroxide can’t be ignored in modern manufacturing, but healthy respect, up-to-date training, and real vigilance keep its health hazards in check. Companies that invest in better equipment, smarter workplaces, and open conversations about risk will find fewer injuries and better morale. That’s an investment worth every penny.
Each day, I notice trash bins filling up with all manner of packaging, electronics, and old gadgets. Most folks give these items a quick look before dropping them in whichever bin feels convenient. I see shampoo bottles, batteries, and takeout containers sharing the same space. From my own experience, the guilt kicks in only after remembering just how much waste winds up in landfills, and how awkward it feels to realize I contributed to it.
Much of this confusion comes from unclear product labels. Some products sport tiny recycling symbols or vague text like "check locally," leaving people guessing. Out of habit or convenience, many just toss things in the trash, not thinking much beyond that moment.
Throwing away certain products without a second thought doesn't just waste resources—sometimes it harms our health. Tossing old batteries or phones in the garbage can let toxic metals seep into the soil and water. I remember the day my town’s dump closed its gates after a contamination scare. Kids’ playgrounds nearby had to close, and neighbors grew nervous about what was drifting out of the site. That’s when a lot of us started reading disposal guidelines more closely.
Food packaging, even cardboard types, often comes coated with plastics and chemicals that don’t break down properly. Single-use plastics clog waterways, creating more clean-up costs for cities and even higher grocery bills when fisheries and farms need to test for new pollutants. Every time we pick the easy route, the planet picks up the tab.
Sorting waste sounds complicated, but small changes help. For electronics, local recycling drives and drop-off points exist in most cities. I’ve learned to keep a pile of spent batteries and old chargers near the front door, dropping them at the hardware store collection box once a month. Through habit, the burden shrinks, and more devices actually get stripped for usable metals.
For plastics and packaging, rinsing items before tossing them in the recycling bin goes a long way. Leftover food ruins batches, sending the whole mess to a landfill. Paper products carrying grease or food—pizza boxes, coffee cups—often belong in the trash instead.
Hazardous products like paint, pesticides, and cleaning chemicals call for extra caution. My city publishes a disposal calendar, and I’ve seen lines of neighbors waiting their turn. Nobody gets it perfect every time, but steps in the right direction add up fast.
Clearer labels on everyday products would put less pressure on individuals to guess. Statewide initiatives tying deposit fees to returns (like the bottle bill in Michigan) bring incentives for returning containers. When enough people pitch in, recycling and waste diversion rates rise measurably.
Households gain from community education campaigns—workshops, local webinars, or even flyers do wonders for improving habits. I’ve learned more from chatting with my local sanitation workers than any website. Listening to their advice helps decisions at home stick: set up separate bins, don’t bag recyclables, save hazardous items for special pickups.
By thinking beyond convenience, respecting local guidelines, and supporting better product labeling, everyone takes part in slowing pollution and keeping neighborhoods healthy. Small steps each week shift the cycle away from the landfill and toward a world where products don’t just vanish after that final toss—they get a real chance at a second life.
Bis(4-Chlorobenzoyl) Peroxide grabs a spot on the shelf as an organic peroxide valued for its ability to kickstart reactions. Labs and manufacturers call on it for polymerization and other chemical processes. Before anyone stores a drum of this material, it makes sense to talk about real-world stability, especially since peroxides can turn unpredictable without the right handling.
With content up to 77%, the concentration raises risk. High content organic peroxides like this do not play nice with heat and friction. Once the percentage passes 50%, the wealth of reactive oxygen means even a small slip-up might trigger decomposition or worse. Thinking back to years spent in labs, I’ve seen how easy it is to forget about a sample pushed to the back of a bench. Even with Bis(4-Chlorobenzoyl) Peroxide, these risks do not vanish until the material is used up or disposed of.
Most peroxides, including this one, prefer it cool and dry. Storage above 25°C (77°F) edges the odds towards runaway decomposition. Many manufacturers even insist on refrigeration, believing that temperature swings alone can start trouble. In practical terms, air conditioning and temperature loggers become important, not afterthoughts. Failing to control storage conditions has caused accidents big enough to change industry rules.
The package matters. Metal drums may sound tough, but peroxides like Bis(4-Chlorobenzoyl) Peroxide need plastic or tightly-sealed glass containers. Clean, dry, and free of contamination: that’s the gold standard for storage. Sometimes just a few drops of a different chemical or a bit of moisture will set off a reaction. Labels need to be clear—mix-ups have led to emergencies more than once, as anyone in hazardous materials response can tell you.
Peroxides and contaminants form a dangerous mix. From personal experience, a trace of acid or base can set off a chain reaction, so separate storage by class is no joke. Mixing strong oxidizers or reductants into the pile—accidentally or not—pushes things closer to a thermal event. The National Fire Protection Association ranks organic peroxides in the hazard zone for good reason.
A few years ago, an incident involving similar peroxides forced an entire research building to evacuate. No one expected that material, thought stable at room temperature, to start reacting in the back of a supply cabinet. Investigation found poor ventilation, forgotten stock, and a container left open for a day—factors that sound small, until something goes wrong.
Routine checks make all the difference. Inventory audits, regular disposal, and training keep surprise decompositions off the table. Regulatory agencies—OSHA, EPA, and their peers abroad—publish clear advice: treat any high-content organic peroxide with the respect it demands. Safety Data Sheets are not just for posterity. Anyone working with Bis(4-Chlorobenzoyl) Peroxide reads the documentation, follows the exposure limits, and uses safety controls like ventilation and fire suppression.
Labs, factories, and even universities find that small changes in storage, training, and process control pay off. The value of Bis(4-Chlorobenzoyl) Peroxide means little if it destabilizes before it lands in the reactor. Respect for chemistry and routine safety checks form the foundation for long-term stability—and peace of mind for everyone involved.
| Names | |
| Preferred IUPAC name | Bis(4-chlorobenzoyl) peroxide |
| Other names |
Peroxybis(4-chlorobenzoyl) 4-Chlorobenzoyl peroxide 4-Chlorobenzoyl peroxyde Bis(4-chlorobenzoyl) peroxide 4-Chlorobenzoyl peroxide, ≤77% |
| Pronunciation | /ˈbɪs fɔːr ˈklɔːrəˌbɛnˈzoɪl pəˈrɒksaɪd/ |
| Identifiers | |
| CAS Number | [2212-81-9] |
| Beilstein Reference | 139873 |
| ChEBI | CHEBI:87157 |
| ChEMBL | CHEMBL185198 |
| ChemSpider | 14725 |
| DrugBank | DB11315 |
| ECHA InfoCard | 03b8f2f0-8e68-4e5e-8147-c46d9e43934a |
| EC Number | '211-599-0' |
| Gmelin Reference | Gmellin 239784 |
| KEGG | C19673 |
| MeSH | D004209 |
| PubChem CID | 7097 |
| RTECS number | TC6300000 |
| UNII | 1L88FGL8CS |
| UN number | 3104 |
| Properties | |
| Chemical formula | C14H6Cl4O4 |
| Molar mass | Molar mass: 348.57 g/mol |
| Appearance | White or pale yellow crystalline powder |
| Odor | Odorless |
| Density | 1.38 g/cm3 |
| Solubility in water | insoluble |
| log P | 3.89 |
| Vapor pressure | < 0.1 mmHg (20 °C) |
| Acidity (pKa) | 11.2 |
| Basicity (pKb) | pKb > 7 (at 25 °C) |
| Magnetic susceptibility (χ) | -6.22E-6 |
| Refractive index (nD) | 1.623 |
| Viscosity | 16 mPa.s (25 °C) |
| Dipole moment | 3.98 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 316.4 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -288.7 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -1788 kJ mol⁻¹ |
| Pharmacology | |
| ATC code | D10AE01 |
| Hazards | |
| GHS labelling | GHS02, GHS07, GHS08, GHS09 |
| Pictograms | GHS02,GHS07,GHS05 |
| Signal word | Danger |
| Hazard statements | Hazard statements: H242, H302, H317, H319, H332, H335 |
| Precautionary statements | P210, P220, P234, P235, P240, P241, P242, P243, P261, P264, P270, P271, P280, P321, P362+P364, P370+P378, P403+P235, P405, P410+P403, P501 |
| NFPA 704 (fire diamond) | 3-2-4-OX |
| Flash point | > 75°C |
| Autoignition temperature | Unknown |
| Lethal dose or concentration | LD50 Oral Rat: > 2000 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral, Rat: >5000 mg/kg |
| NIOSH | DDC |
| PEL (Permissible) | PEL: Not Established |
| REL (Recommended) | 0.2 mg/m³ |
| IDLH (Immediate danger) | Unknown |
| Related compounds | |
| Related compounds |
Benzoyl peroxide Dicumyl peroxide Tert-butyl peroxybenzoate 4-Chlorobenzoyl chloride Acetyl peroxide |
