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Chemistry loves to take long routes to get where it’s going. The story of Di-N-Butyl Peroxydicarbonate stretches back to the early days of polymer chemistry in the twentieth century, a time when researchers pushed the boundaries of what organic molecules could do. During these years, the demand for better initiators to drive the synthesis of plastics, elastomers, and advanced materials led scientists to tinker with all sorts of peroxides. Many failed due to short shelf lives or explosive tendencies. Di-N-Butyl Peroxydicarbonate emerged from this period, offering a new route for folks seeking room-temperature activity paired with better handling safety. I remember thumbing through an old chemistry compendium and coming across early patents describing this class of initiator, reflecting a period of real innovation as companies and universities both raced to roll out plastics at scale. The molecule gets its modern spotlight because it helps bridge safety and reactivity—something industrial chemists care about a lot once benches and glassware give way to drums and reactors.
Most people outside chemical manufacturing have never heard the name, but those working with PVC or acrylics know Di-N-Butyl Peroxydicarbonate by reputation. Found sold as a stable frozen dispersion in water, generally with content capped at 42 percent, this material finds a home in plants across the world. It doesn’t command headlines, but it does find its way into coatings, adhesives, and anything built from polymers needing free-radical initiation at lower temperatures. It’s not flashy, but it provides exactly what’s asked—predictable reactivity and a user-friendly handling profile, especially in locations where high ambient temperatures threaten more sensitive options.
Di-N-Butyl Peroxydicarbonate takes the form of a colorless to slightly yellow oily liquid, frozen solid in its standard dispersion. In terms of smell, there’s a faint odor, a bit like other peroxides, but not overwhelming. It stays stable when properly cooled and handled in dispersion, but once free from its frozen shell, it's only a matter of time before it starts decomposing, generating free radicals vital for its key uses. The molecule dissolves in various organic solvents but finds much less solubility in water, hence the frozen dispersion approach. From my time handling peroxides, chilling and quick movement remain essential—let it get above -10°C for too long, and you risk unplanned reactions, something no one wants behind a loading dock.
Chemical products must wear their credentials clearly. With Di-N-Butyl Peroxydicarbonate, labels usually stress both the percentage of active ingredient and the importance of freezing. Packages often display hazard warnings about oxidizing properties, alongside the UN number for shipping peroxides. Plus, the labeling provides handling instructions in every language needed where it’s shipped. No manufacturer wants ambiguity here—mishaps born of poor labeling cost companies much more than paint spills or spoiled batches. Much of the effort goes into making it easy for warehouse workers to check the temperature, rotate inventory, and make sure everything moves along to production safely.
Making this compound relies on classic organic chemistry, with a reaction involving n-butanol, phosgene, and hydrogen peroxide (handled with care). The process calls for solid control, especially temperature and exclusion of metal contaminants, both to improve yield and suppress unwanted byproducts. During college, my lab work never reached this scale, but I did learn early how fast peroxides can get out of hand even with tiny spills. Industrial chemists talk often about phased additions and vigorous scrubbing of evolved gases. Effluent treatment stays at the front of everyone’s minds, since both phosgene and peroxide breakdowns create real risks to air and water.
At its heart, Di-N-Butyl Peroxydicarbonate acts as a free-radical initiator—meaning it starts reactions that would otherwise need either high heat or more hazardous alternatives. Drop it into the right monomer soup, and it kicks off polymerization, creating long chains that turn liquid chemicals into hard plastics or flexible films depending on what’s mixed in. Tweaking the substituent groups on the core molecule can shift temperature sensitivity, storage life, or reactivity, helping tailor the molecule to specific industrial needs. Over the years, researchers have searched for greener ways to modify the molecule, reducing hazardous byproducts and extending shelf life—making the end product safer for everyone involved, from lab technician to factory operator.
Chemists rarely call a compound by just one name. In catalogs and scientific articles, you’ll find Di-N-Butyl Peroxydicarbonate listed alongside synonyms like Peroxydicarbonic acid, dibutyl ester, or simply DNBPDC. On barrels, brand names pop up from every corner of the globe, each with their own histories and markets. When reaching for a chemical, always match the CAS number and read the labels—the biggest accidents happen when someone confuses a cousin compound for the real deal.
Handling peroxides demands respect. Di-N-Butyl Peroxydicarbonate avoids some risks linked to more temperamental initiators, but lab coats, face shields, and gloves still make up the daily dress code where it’s involved. Precoolers and insulated transport lines line up along production floors, while safety officers check logs and monitor freezers constantly. During my years working for a chemical distributor, we trained every new worker to recognize the warning signs—cracking containers, odd smells, sweating drums—because one small foul-up could ruin a shift or send someone to the hospital. Regulatory agencies worldwide love paperwork, but their focus on proper packaging, clear hazard communication, and regular site audits really makes a difference with energetic compounds like this.
Plastic production drives demand for Di-N-Butyl Peroxydicarbonate. The molecule gets its main use as a polymerization initiator, especially in vinyl chloride, acrylics, and some specialty elastomers. I’ve seen factories transform tanker trucks filled with monomers into thousands of tons of pellets, all starting from a few liters of frozen initiator. Outside plastics, its unique stability profile earns a spot in laboratories exploring new low-temperature reactions, and sometimes in pharmaceuticals as a specialized reagent. While most consumers never touch or hear about this compound, it quietly shapes the products that show up on store shelves every day.
Researchers never stop searching for better methods, higher yields, and safer handling. New work looks at swapping out phosgene, a toxic legacy ingredient, with greener alternatives—something green chemistry folks push for strongly. Automation and remote monitoring get more attention, reducing worker exposure and tracking freezer temps from a phone app. Alternative solvents, more sustainable raw materials, and engineered catalysts promise improvements in both environmental footprint and product quality. Conferences and journals now regularly feature papers on peroxide safety mechanisms, aiming to prevent not just accidents but also minimize waste. The lab-to-plant pipeline may look slow, but the steady trickle of innovations shows real commitment to building a safer, cleaner future for industrial chemistry.
No compound used at industrial scale escapes scrutiny, and Di-N-Butyl Peroxydicarbonate earns its share. Toxicology studies focus on skin and respiratory sensitization, acute oral and dermal toxicity, environmental persistence, and breakdown products once released. Case reports from factories and transportation mishaps help build better safety guidelines. Thankfully, its stable aqueous form prevents many worst-case scenarios, though the need remains for robust spill response drills and careful waste handling. My own experience dealing with cleanup kits reminds me that mistakes happen—training and good habits, not paperwork, keep accidents from becoming disasters. Research continues into whether breakdown products present risks to aquatic life or crop soil, helping companies and regulators draw clear lines in plant design and waste treatment. Regulators, especially in Europe and parts of Asia, keep tightening limits and mandating transparent reporting.
As manufacturing demands more sustainable and safe chemistry, compounds like Di-N-Butyl Peroxydicarbonate face both challenges and open doors. The industry presses for even safer molecules, friendlier to both worker and ecosystem, often at lower cost. Digital process control and new production technologies could reduce human involvement along dangerous steps, leading to fewer accidents. Recyclable packaging and improved formulations for transport might extend shelf life, cut waste, and serve smaller markets. Universities and start-ups search for radical new initiators, but today’s proven molecules won’t vanish overnight—too many production lines and too much infrastructure rely on their steadiness. Ultimately, a combination of tighter safety protocols, smarter design, and relentless innovation will keep compounds like this one relevant in the coming decades.
Di-N-Butyl Peroxydicarbonate usually flies under the radar. It isn’t exactly a household name, but if you look at modern manufacturing, it pops up more often than you’d expect. I got curious about this compound after a conversation with a friend in the plastics industry. They explained that this stuff drives one key step in making certain plastics—acting as an initiator in the polymerization of vinyl chloride. Without it, imagine how different everyday life would look, from pipes to siding or even credit cards.
This chemical doesn’t just end up in factories churning out bulk PVC, though. In the lab, scientists rely on it to kick off polymerization for a bunch of specialty materials. Folks who work in coatings or adhesives count on the way it helps form reliable, flexible films. For example, manufacturers use it to fine-tune properties like clarity and strength in their product lines. There’s a certain satisfaction in seeing how each stage of the production process, powered by the right ingredient, changes the final product in your hands.
Peroxides often get a sketchy reputation because of their reactivity. I’ve seen the nervous glances when someone pulls one out in a college chemistry lab—even seasoned researchers double-check safety gear. By keeping the concentration at 42% or lower and presenting it as a stable dispersion in water (and shipping it frozen), manufacturers cut potential hazards significantly. That’s not just about following rules—there’s real peace of mind for workers moving barrels across a busy facility floor or technicians preparing a batch for research.
Workplace safety statistics, especially in chemical plants and distribution centers, show a decline in peroxide-related accidents thanks to better formulations like this. Stringent shipping guidelines now mean fewer unexpected emergencies—freezing the compound can curb thermal decomposition that would otherwise get dangerous fast. It’s not glamorous, but lives often depend on extra steps like these.
The flip side of these benefits includes real sustainability challenges. Every sector using these initiators has to wrestle with proper disposal and emissions. Water-based dispersions help by reducing the use of organic solvents, cutting VOC emissions—a win for air quality around the production plant. I remember a time volunteering for a community group near an industrial area, chasing down odd smells on warm days. The difference after stricter controls got introduced and water-based initiators became common was night and day.
Responsibility doesn’t stop at cleaner air. There’s an urgent discussion happening about lifecycle management for these chemicals. Tight controls on process wastewater and improved training go hand-in-hand with solutions, so these products add value without long-term environmental headaches.
There’s an interesting balance here between chemistry that fuels progress and the humans behind each step. The drive for stable, more manageable versions of tricky compounds like Di-N-Butyl Peroxydicarbonate keeps people safer and production lines humming. Supporting ongoing education means every new employee—from the warehouse to the quality control lab—knows where the risks lie and how to manage them.
It becomes easy to take specialty chemicals for granted, never stopping to think about the chain of invention, safety checks, and environmental care behind every batch. Producers who really invest in transparency—sharing safety data, traceability, and environmental impact—lead the way forward. That transparency helps the public trust industries that handle powerful tools like these.
Di-N-Butyl Peroxydicarbonate stands out as a specialty chemical with a reputation for being both useful and hazardous. My first encounter with this substance involved a tense conversation with a warehouse foreman after an unexpected temperature spike in our storage room. I remember the tension—nobody wants to be the one who overlooks safe handling.
Peroxydicarbonate compounds act as powerful oxidizers, which gives them a dual personality: impressive for the polymer industry, demanding for those working nearby. The water-based, frozen dispersion type feels less frightening than pure forms, but don’t let your guard down. Accidents usually strike when routines slip, not when everyone is on high alert.
We never stored this stuff with general-use chemicals, let alone on a shelf next to acids or fuels. Oxygen-rich chemicals and flammable products create a recipe for trouble once they mingle.
Cold storage keeps risks low. Regular freezers won’t cut it—I’ve seen colleagues try to make old equipment work and wind up with spoiled batches or worse. A dedicated walk-in freezer holding below minus 20°C made a difference. It is not just about extending shelf life; lower temperatures dampen the threat of decomposition or an unexpected reaction.
Store these chemicals in insulated, tightly sealed containers. Specialist suppliers use polyethylene or similar materials for good reason: glass cracks with temperature shifts, metal can corrode or even catalyze unwanted reactions. Containers need a clear label—not just for compliance, but for the next shift who hasn’t memorized every drum’s content. I learned early that mixed-up labeling caused confusion and nearly sent an intern to the hospital from a mistaken splash while doing an unscheduled inventory.
Rooms storing peroxydicarbonates can’t be forgotten, even temporarily. Good ventilation lets any off-gassed vapors dissipate. Once, the smell from slow decomposition triggered our alarms—ventilation proved its worth in avoiding a bigger mess.
Segregate this chemical far from incompatible substances and strong sunlight. UV rays speed decomposition and raise the risk of fire. Even with frozen storage, direct light starts that reaction faster than people realize. I recall a batch sitting near a window one winter: condensation and diffuse sunlight together started a chain of trouble we caught just in time.
Workers need training and clear safety instructions. Part of our routine included reviewing handling SOPs at least once a month. I came across stories—some tragic—of places that skipped this step. It’s much easier to review an emergency plan at your own pace than to fumble with it during a spill or worse, a fire.
The right personal protective equipment saved a coworker from chemical burns more than once. Face shields, cold-resistant gloves, and long sleeves weren’t negotiable. A casual attitude about PPE never lasted long—chloroform byproducts leave nasty burns, and these stories travel fast through any plant.
Secondary containment trays absorb drips and block water from reaching storage containers. Water plus most peroxides never adds up to anything good, even in a “safe” formulation. Neutralizing agents should always be close at hand. Once, after a shipment leak, we managed to prevent damage by responding in under a minute because our spill kit was nearby.
Disposal must follow local hazardous waste rules. Too often, someone dumps leftovers down a drain, thinking it’s diluted enough to avoid harm. I watched a municipal system choke and backflow once, teaching a sharp lesson—cleanup costs far outweigh a few minutes of proper disposal.
Open communication makes all the difference. Staff meetings where everyone shares recent incidents, near-misses, or odd findings mean problems get solved before they grow. Culture matters. I saw teams with open conversations own up to mistakes faster and grow safer over time.
Automation and better temperature monitoring give peace of mind. Investing in alarms and remote data loggers means sleep doesn’t get interrupted by a power outage you didn’t catch until morning. The price of prevention barely shows up on a balance sheet compared to emergency cleanup.
Handling chemicals like Di-N-Butyl Peroxydicarbonate never loses its importance, no matter your role or experience. For me, a bit of worry means I’m treating the risks with the respect they deserve—and reinforcing a safe environment for everyone at work.
Di-N-Butyl Peroxydicarbonate shows up in the chemical world as a pretty serious operator. It’s known to speed up polymerization, so industries use it to make plastics and resins. Even though it stays frozen and mixed in water to calm things down, this chemical still carries some heavy baggage as far as safety goes.
The most obvious worry comes from what happens if people get it on their skin or in their lungs. Studies in places handling peroxide chemicals show skin contact might lead to burns or rashes. This chemical combination does not belong in anyone’s eyes; splashes might bring severe irritation, and direct exposure risks actual damage. If it goes airborne—maybe through a spill or when not kept cold—it can irritate the nose and throat, sometimes causing headaches or trouble breathing.
Some folks take chemical dangers lightly, thinking they’ll just “wash off.” But there’s real history in plant environments: workers have ended up with chronic skin and respiratory problems thanks to repeated exposure. That’s not a scare tactic—it’s built up from decades of job records in chemical manufacturing.
It’s the instability that really stands out with this chemical, even in a stable frozen mix. Di-N-Butyl Peroxydicarbonate likes things cold. If the temperature nudges up, decomposition kicks in and things heat up further. This snowball effect sweeps fast: heat brings more decomposition, which brings more heat. All that pressure sometimes leads to violent rupture or even an explosion. Some tragic real-world examples in smaller manufacturing setups involved just a single broken freezer, and the fallout injured workers nearby.
Mixing this peroxide with other chemicals—especially acids, bases, or flammable materials—raises the odds of an unexpected reaction. This isn’t limited to big manufacturers. Even a small leak or poor storage conditions in a university lab or small factory might mean serious trouble.
Leaks or spills from storage or containers get into drains and pollute water systems. This chemical does not belong in any ecosystem. It doesn’t stick around forever, but while present, it does real harm to fish and aquatic bugs. Cleanup involves more than a mop—trained emergency teams work to keep waterways clear. The U.S. Environmental Protection Agency lists organic peroxides among high-hazard substances, and local authorities keep tight controls for good reason.
Personal protection works. Workers should use gloves and face protection, and businesses have to plan for emergencies. Ventilation makes a difference, too. Keeping the stuff frozen and far from heat sources must sit right at the center of storage rules. Never underestimate the value of safety drills. One factory I toured went a step beyond: every worker could spot early warning signs of decomposition, and their top supervisor insisted on regular reviews.
Switching to less hazardous chemicals in the process where possible cuts risks. Where substitution isn’t realistic, tighter monitoring with sensors and alarms, as well as robust emergency plans, stand as solid lines of defense. Trace amounts or small leaks may look minor—past incidents prove how fast a minor slip-up snowballs into a crisis.
There’s no shortage of rules for handling chemicals like this one—OSHA, EPA, and international bodies track its movement and storage. Fines follow slip-ups, but real motivation goes past fines. No one wants a headline about workplace injury or contaminated rivers on their watch. The smartest managers see this risk up close and budget for prevention far more than cleanup.
Good information, honest training, and commitment from every level of a shop or lab mean fewer accidents. Too often, rushed jobs or skipped steps cause harm that could vanish with just a little added care.
Many people, even those who work with chemicals regularly, sometimes don’t think much about the risks certain containers can pose. Di-N-Butyl Peroxydicarbonate, especially as a 42% dispersion in frozen water, deserves respect. This chemical, lurking in some laboratories and manufacturing plants, carries a hefty punch. If warmed up, shaken, or stored with the wrong stuff, it can go from harmless to dangerous without much warning. I remember a close call in a research lab: a coworker set an old, forgotten container of peroxide on top of a fridge, thinking it would be fine for a week. The following Monday, a mess—thankfully not an explosion, but enough to keep folks on high alert after that.
Most people just want hazardous chemicals gone, out of the building, off their list. Dumping it down the drain or mixing it with regular trash invites trouble nobody wants. This isn’t fear-mongering; stats from the EPA and OSHA point to several preventable injuries every year from improper chemical disposal and mixing. Water-reactive, shock-sensitive, and oxidizing chemicals have special needs—ignoring those can cause explosions, toxic clouds, even fires. Even in small amounts, peroxidic compounds like this one set the stage for a disaster if carelessly handled.
OSHA, the EPA, and local hazardous waste authorities lay down rules for a reason. Di-N-Butyl Peroxydicarbonate counts as a “reactive hazardous waste” by the US EPA’s definition. That means it should never mingle with general trash or regular water systems. Most chemical safety sheets repeat it—send unused or expired peroxide to a licensed hazardous waste handler. These disposal firms use trained personnel, gear, and procedures built around safety. They neutralize reactive substances under controlled conditions, separate them from incompatible items, and log every step so nothing vanishes or ends up in a river, landfill, or air vent.
Folks in small labs, schools, or startup companies face different pressures—they might not have full-time EHS (Environmental Health and Safety) staff to walk them through every regulation. It’s tempting to forget about a bottle of something as long as it’s sitting quietly in a freezer or on a shelf. That approach only works until it leaks or someone moves it without the right precautions. Taking the time to keep an up-to-date inventory, label everything clearly, and call in hazardous waste experts saves lives—and millions of dollars in fines or cleanup bills. It’s not theory—I’ve seen organizations catch mistakes early because someone noticed an odd label or an outdated bottle in a cold room and flagged it for proper disposal.
Educating everyone from the top down pays off. Training new hires, reminding veterans, bringing in outside consultants when needed—these steps prevent accidents and protect the environment. Leaning on government resources, such as the EPA’s and OSHA’s guidelines, means nobody has to work through this alone. More labs now partner with hazardous material disposal services that pick up, log, neutralize, and document everything. Taking those steps not only clears space but builds a culture of safety and environmental care that sticks with everyone well after they move on to new jobs or projects.
Handling Di-N-Butyl Peroxydicarbonate, even as a stable water dispersion, calls for some real care. This isn’t just another chemical stored in the backroom. Ask anyone from a production plant or research lab who’s mixed up organic peroxides, and you’ll hear stories about surprising reactivity and random decomposition events. Peroxides keep emergency rooms in business more than we’d all like. This compound comes with risks: flammability, sensitivity to heat or shock, and skin or respiratory irritation. As the ice keeping it stable begins to thaw, vigilance means more than simply following the rules—it prevents disasters.
No one forgets the first time a splash lands on skin or, worse, hits the eyes. Standard lab coats do little against organic peroxide solutions that creep under cuffs and collars. Most people working with these dispersions reach for chemical-resistant gloves—nitrile, often layered for confidence. Thick, old leather gloves don’t cut it; they soak up chemicals and trap the danger against your skin. Face shields or splash goggles block the worst, especially during transfer or weighing out smaller amounts. A regular pair of safety glasses does nothing if mist or aerosol escapes while handling frozen or thawing material.
If you’ve ever caught a whiff of peroxide vapors, your lungs remember. Reliance on a well-ventilated fume hood isn’t optional, particularly after thawing. Respirators rated for organic vapor cartridges step in if there’s any leak, accident, or if the hood loses its draw. Airborne particles, even microscopic, don’t announce themselves. Workers trust their gear and keep backup cartridges handy—that’s experience talking, not paranoia.
Clothing selection matters too. Loose sleeves and synthetic fabrics spell disaster if peroxide decomposes on them—melting shirts stick to skin, compounding the damage. Professionals working with peroxides skip the polyester: they wear cotton or flame-retardant lab coats and stick to long sleeves, minimizing exposure at every inch.
Ask a veteran why they wear chemical-resistant boots instead of open shoes or regular sneakers. Spilled peroxides roll off the workbench, land on floors, and seek out any inch of exposed skin. Protective foot coverings and closed-toe shoes without absorbent fabric close the safety loop.
No set of gloves, goggles, or coats makes up for sloppy habits. In my time supervising labs, I’ve seen strong PPE standards weaved right into daily routines. Teams that discuss last week’s near-misses build habits that help catch mistakes before they snowball. Regular retraining on chemical hazards reminds everyone why protocols exist—not to please inspectors, but to bring each person home safely at the end of the day.
Routine inspection of gear never feels glamorous, but it pays. Cracked goggles and thin gloves prove useless in the moment you need them. Real safety comes from a combination of good habits and well-chosen PPE. Talking candidly about risks, sharing mistakes, and using strong gear create a work environment where people look out for each other—not just themselves.
I see too many workplaces treating chemical PPE as a simple checklist. Ask the tough questions: Is my gear right for the specific risk at hand? What happens if something spills or decomposes? Would I trust this setup to protect me in a real accident? When teams dig for those answers, injuries go down, and everyone gets a little closer to going home in the same shape they showed up.
| Names | |
| Preferred IUPAC name | Peroxy(din-butylcarbonate) |
| Other names |
Peroxydicarbonic acid, dibutyl ester, mixture with water (≤42% active ingredient, frozen) Di-n-butyl peroxydicarbonate, wet (≤42%) Peroxydicarbonic acid, dibutyl ester, water-wet, frozen |
| Pronunciation | /daɪ-ɛn-bjuːˈtɪl pəˌrɒk.sɪd.aɪˈkɑː.bə.neɪt/ |
| Identifiers | |
| CAS Number | 13940-32-4 |
| Beilstein Reference | 1721163 |
| ChEBI | CHEBI:9456 |
| ChEMBL | CHEMBL1702067 |
| ChemSpider | 21468069 |
| DrugBank | DB14674 |
| ECHA InfoCard | 100_113_7 |
| EC Number | 226-885-3 |
| Gmelin Reference | 1468816 |
| KEGG | C18604 |
| MeSH | Di-N-Butyl Peroxydicarbonate |
| PubChem CID | 155270707 |
| RTECS number | EF8905000 |
| UNII | 8GHG851K1T |
| UN number | UN3112 |
| Properties | |
| Chemical formula | C10H18O6 |
| Molar mass | 266.32 g/mol |
| Appearance | White frozen mass |
| Odor | Odorless |
| Density | Density: 1.1 g/cm³ |
| Solubility in water | Insoluble |
| log P | 3.87 |
| Vapor pressure | 0.27 kPa (20°C) |
| Basicity (pKb) | > 3.5 |
| Magnetic susceptibility (χ) | -7.8E-6 |
| Refractive index (nD) | 1.4200 |
| Viscosity | 10 mPa·s (20°C) |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 510.2 J·mol⁻¹·K⁻¹ |
| Std enthalpy of combustion (ΔcH⦵298) | -9026 kJ/mol |
| Hazards | |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS02,GHS05,GHS07,GHS09 |
| Signal word | Danger |
| Hazard statements | H242, H302, H317, H332, H400 |
| Precautionary statements | P210, P220, P234, P280, P302+P335+P334, P305+P351+P338, P411+P235, P420 |
| NFPA 704 (fire diamond) | 2-4-3-W |
| Flash point | -20°C |
| Autoignition temperature | > 71°C |
| Explosive limits | Upper limit: 6.3%, Lower limit: 3.6% |
| Lethal dose or concentration | LD50 (Oral, Rat): 5000 mg/kg |
| LD50 (median dose) | LD50 (median dose): Rat 300mg/kg |
| NIOSH | UN3106 |
| PEL (Permissible) | 1 mg/m³ |
| REL (Recommended) | 5 kg |
| IDLH (Immediate danger) | IDLH: 5 ppm |
| Related compounds | |
| Related compounds |
Bis(2-ethylhexyl) peroxydicarbonate Di-sec-butyl peroxydicarbonate Diisopropyl peroxydicarbonate Dicyclohexyl peroxydicarbonate |
