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Chemistry often surprises those who dig into it, and diisopropyl peroxydicarbonate tells one of those understated stories. This compound didn’t get its start on the front pages. Instead, it appeared as chemists probed deeper into organic peroxides in the decades that followed the industrial revolution. Factories in Europe, hunting for new ways to kick-start polymerization, stumbled across the possibilities in peroxydicarbonates. Since then, the name diisopropyl peroxydicarbonate, or DIPP as many chemists know it, has settled into the quiet but important corners of industrial chemistry. In labs, the compound became almost a household name among those working on radical initiators, as the need for controlled, predictable chemical starts drove innovation. Stories passed around about early batch reactors blowing up, their pressure gauges rattling because the chemists didn’t respect the explosive nature of peroxides, show how experience shaped safer practices for handling DIPP. That past still sits behind every caution sign taped to peroxide storage rooms.
At its core, DIPP is made up of two isopropyl groups attached through oxygen linkages to a central peroxydicarbonate unit. The commercial product contains at most 32% DIPP, with at least 68% being a type A diluent, usually a phlegmatizer that tempers the reactivity and prevents accidents before they start. It has a bit of a reputation for being tricky to handle but does the job when asked. With a low decomposition temperature, it fits the niche of starting reactions that need a gentle push instead of a hard shove. The structure isn’t complicated compared to some specialty chemicals, but its reactivity demands respect. Anyone who’s ever unscrewed a bottle of DIPP for the first time knows to treat it with a steady hand and a clear mind.
DIPP lives as a colorless or pale liquid, easily mistaken at first glance for hundreds of similar compounds. You quickly learn to recognize the faint, almost sharp smell that signals peroxides. The boiling point drags far below room temperature, and the compound breaks down well before it can get hot. Heat, friction, or even shocks can cause sudden decomposition—no one needs reminding that organic peroxides earned their fearful reputation through such behaviors. Left exposed to air, it loses potency. Lab veterans often recall early mistakes, like warming a plastic pipette unknowingly, resulting in fizzing or even explosion. Chemically, DIPP initiates free radical reactions, splitting under mild conditions to give radicals that launch chain-reactions during polymer formation. The diluted formulation supplied commercially tames this wilder side but never removes it.
Industry and regulation both demand clear technical information for anything as volatile as DIPP. Commercial labels, mandated by local and international standards, offer sharp, direct warnings. Bottles arrive clearly stamped with concentration, diluent type and percentage, batch number, and hazard pictograms impossible to miss. Handlers get no leeway to misinterpret the risks, and transportation regulations treat every package with the suspicion reserved for explosives. Storage means cool, dark rooms, vigilantly tracked and often inspected. From my years working near chemical storage, I can’t count the times I saw newer colleagues trained rigidly on peroxide labeling practices, everyone knowing the consequences of carelessness.
Preparing DIPP starts with isopropyl alcohol and phosgene, under controlled settings that make any casual visitor look twice. The synthesis runs as a two-phase reaction, typically at low temperatures, with exacting amounts of sodium hydroxide used to scavenge unwanted acid byproducts. The oxygen source, usually hydrogen peroxide or similar, comes in slowly to avoid runaway reactions. As the process plays out, experienced chemists keep constant watch, because peroxide manufacturing gives no room for error. The mixture then receives a phlegmatizing agent, often dialkyl phthalate or a similar solvent, to create the familiar diluted concentrate. Every step is measured, every vessel checked, and any odd noise puts everyone on edge. Chemical manufacture of peroxides ranks among the jobs where nerves of steel and attention to detail spell the difference between success and disaster.
DIPP forms the backbone for radical polymerization, breaking into isopropoxy and carbonate radicals under modest heat. Its decomposition props up vinyl chloride and similar monomers, creating long polymer chains for plastics or specialty materials. Chemists often modify DIPP by shifting the diluent or adding stabilizers tailored to the end-use, adjusting shelf life or reactivity. In my own research, tweaking the reaction temperature shaved precious minutes off slow polymerizations, sometimes at the cost of increased side reactions. Tuning DIPP’s formulation lets industries tailor production for everything from PVC pipes to more technical polymer films. Every alteration, though, brings trade-offs—often in terms of purity, reactivity, or risk profile.
Anyone hunting through catalogues or safety manuals finds DIPP listed under several names, depending on geography or supplier. You may encounter entries like “Isopropyl Peroxydicarbonate,” “Peroxydicarbonic acid, bis(1-methylethyl) ester,” and various abbreviations. Multilingual manuals complicate matters, sometimes tossing in local dialects or historical labels. This confusion often crops up during procurement for international projects, where matching chemicals by structure or registration numbers saves more headaches than it should. In research settings, clarity in naming avoids disasters in ordering, especially when peroxides so easily confuse.
Safety takes on real urgency in environments where DIPP gets handled. Standard operating procedures combine personal protective gear, explosion-proof equipment, and strict inventory controls. No one stores DIPP near direct sunlight or in places subject to temperature swings, and air circulation prevents the buildup of dangerous vapors. Training new lab members leans heavily on stories of near-misses and actual accidents from past decades—stories that still feel fresh for those who lost colleagues or almost got caught in the wrong place at the wrong time. Inspections come with sharp eyes, security seals, and strict paperwork trails. Even at the shipping dock, handlers know to treat DIPP packages with the same respect given firearms or explosives. The best-run facilities bring new faces up to speed on these rules before any bottle gets touched, let alone opened.
The big uses for DIPP cluster around the plastics and composites sector, especially in the production of polyvinyl chloride (PVC) and allied polymers. It makes high-purity, clear plastics possible, thanks to efficient initiation at low temperatures. Electrical insulation, medical devices, packaging materials, and construction supplies all owe something to DIPP-driven chemistry. In these industries, reliability matters more than flash, and DIPP’s predictable behavior earns it repeat orders. I’ve seen whole factories run on three-shift rotations, with batch timings selected to match DIPP’s activity curve against the daily temperature cycle. Anyone working around these supply chains soon learns how central DIPP is, even if its name rarely appears outside technical instructions.
Modern R&D teams dig into DIPP mainly to improve safety, environmental profile, and polymerization performance. Ongoing projects aim to replace the type A diluents with safer or greener alternatives. Others look into stabilizing additives or new synthesis pathways that produce less waste or avoid chloroform. Over the last two decades, advances in process monitoring, continuous flow reactors, and automation have shrunk incident rates, but accidents still lurk for those who forget the underlying hazards. Cutting-edge polymer scientists experiment with DIPP-like initiators for novel plastics, including materials with special electrical or optical properties. The push for greener manufacturing keeps the pressure on chemists to find solutions that keep DIPP potent but less risky. Research journals often highlight incremental improvements, sometimes with as much focus on avoiding accidents as on boosting yields.
DIPP’s toxicity profile keeps health and safety officers alert. Direct contact causes skin and eye irritation, and inhalation of vapors brings headaches, dizziness, or worse. Chronic exposure links to longer-term respiratory problems, though data remain incomplete, partly because incidents are thankfully rare. Studies in lab animals show potential organ impacts at high doses, with unclear crossover to humans. For emergency personnel, DIPP’s potential to detonate or release hazardous fumes makes it no ordinary chemical spill—every incident receives full hazmat protocol. The wider field of peroxides has seen a decline in serious incidents, largely thanks to improved training and stricter controls. Still, anecdotal evidence from older workers—those who spent years handling DIPP before modern protocols—reminds everyone that the risks, though tamed, never vanish.
Looking out across the coming years, DIPP finds itself navigating tighter regulations, shifting environmental expectations, and ongoing demand from manufacturing. The search for native replacements continues, but new polymers often require the same radical chemistry that DIPP provides so reliably. Engineers at startup labs hope to engineer safer peroxides or find alternatives that shed the need for volatile side-ingredients. Automation shows promise in limiting human exposure, but process design standards will probably stay strict for decades. For now, unless a breakthrough sweeps through chemical engineering, DIPP keeps its niche—quietly backing industries that depend on quality plastics, all while quietly demanding absolute respect from those who handle it. If my own experience says anything, it’s that DIPP will stick around as long as there are chemists who appreciate the power and risk locked into a simple, transparent liquid. The onus sits on the current and next wave of researchers and plant operators to keep pushing for safer, better ways to use it, without losing sight of the hard lessons already written in the field’s long, sometimes hazardous history.
Diisopropyl Peroxydicarbonate shows up most often in the world of plastics. Its biggest role lands in the manufacturing and processing of polymers. Companies working with vinyl chloride lean on it to kickstart polymerization, the process that takes small molecules and turns them into the plastics used all over modern life. What’s important here is its ability to help polymer chains grow under controlled, often lower, temperatures. Many traditional polymerization initiators need more heat, running the risk of unwanted by-products or degradation. Workers in the plant can keep things cooler, which improves the quality of finished PVC and similar plastics. Those finer products end up in everything from medical tubing to electrical insulation, two areas where failures just can’t happen.
Some jobs need a steady hand and a careful approach. In the world of chemical synthesis, especially in pharmaceutical manufacturing, this peroxydicarbonate helps form specialty polymers and intermediates that go into advanced materials and drug delivery systems. Its segmented breakdown means it can provide free radicals reliably without the combustion or volatility risks seen in some other peroxide-based options. Drug makers trust consistent results—nobody wants a tainted batch making its way downstream—and this chemical delivers.
Paints, coatings, and adhesives demand consistency and control. Manufacturers rely on emulsion polymerization to achieve the kinds of particle size and distribution that translate into smooth finishes and strong bonds. The ingredient in question leads to more efficiently built-up polymers, keeping reaction times reasonable and energy costs contained. For instance, many water-based latex paints depend on polyvinyl chloride or vinyl acetate copolymers made reliably through these chemical tools. The result? Clean application, durable coatings, and, over the years, fewer environmental drawbacks.
Diisopropyl Peroxydicarbonate doesn’t act alone. The product comes diluted with a Type A diluent, making transport, storage, and dosing a lot safer. This blend reduces its sensitivity to heat and strong knocks, which helps prevent accidental reaction in the warehouse or on the factory floor. Having worked in plants with strict safety training, I’ve seen that easier handling reduces not only the chance of incidents but also the time spent on specialized procedures and storage controls. More predictable reactivity lessens both liability and downtime, which are two things every production manager tracks closely.
Demand for tighter environmental controls and lower emissions grows every year. Products like this that function well at lower temperatures help keep energy needs in check. These chemicals also release fewer unwanted side-products in many cases, which aligns with tighter regulations seen in countries leading the charge on chemical safety. Some research groups push for “greener” peroxide alternatives, but for now, production teams stick to these blended peroxydicarbonates for balance in throughput, safety, and quality. Professionals in plastics, coatings, and pharmaceuticals still count on them to meet targets and keep the supply chain humming.
I’ve spent years around chemical storage rooms—places humming with the quiet risk of unstable compounds tucked behind safety doors. Few chemicals grab as much respect from lab veterans as diisopropyl peroxydicarbonate. Its name can trip up the tongue as easily as its vapors can set off a headache. I’ve heard too many stories of close calls to treat this compound lightly.
Let’s talk straight: diisopropyl peroxydicarbonate reacts quickly, and it breaks down dangerously if you mess up the storage. It rarely forgives ignorance or shortcuts. So, there’s no place for guesswork.
This compound breaks apart if the temperature creeps up, releasing gases and heat that nobody wants in a lab or warehouse. I once saw a minor incident where temperature logging failed over a weekend—by Monday, the staff came in to a sharp, sour odor and the rush to vent the room. Fortunately, they caught it before an accident happened, but not everyone gets that lucky.
Stay under 10°C. A dedicated refrigerator with solid temperature monitoring saves trouble. Every scientist or worker entering the storage area needs to know the thermometer means as much as the hazard signs on the container. Regular checks, not just at start-of-day but throughout, reduce the odds of an unexpected breakdown.
Moisture, sun, sparks—each can make this chemical unstable. I keep my containers sealed tight, away from drains, windows, or HVAC vents. No sunlight, no heat, no water near the stash. Lighting should stay cool and remote. Even static electricity can do damage.
I ran into one facility keeping their chemicals near old, dusty light fixtures, thinking a little extra heat kept things pleasant for workers in the winter. They didn’t consider that one crack in insulation could spell disaster. Open shelving, crowded placement, or loosely capped vials only stack the odds against safety.
The right storage means secondary containment: spill trays, sturdy shelves, and cabinets that lock. I once came across a cracked tray soaked through after a minor bottle leak—it caught the spill instead of letting it pool onto the floor. Fire extinguishers, eye wash stations, emergency showers—every basic tool helps, but only if workers feel comfortable using them and trust their training.
Labeling saves lives. Every bottle needs big, clear warning labels—or color codes everyone recognizes instantly, no room for confusion. Signs with storage temperatures, emergency numbers, and chemical hazard information go up as daily reminders.
Mistakes happen when training stops after orientation. Every team member, from new hires to veteran chemists, signs off on updated safety procedures at least every year. Practicing emergency drills builds muscle memory—for fires, leaks, or accidental exposure. Open conversations about “What could go wrong today?” catch risks before they turn into headlines.
If things do go south despite planning, a quick, calm response keeps damage down. With the right habits and respect for what this chemical can do, staff and students go home safe at the end of every shift.
Storing diisopropyl peroxydicarbonate safely isn’t simply about checking boxes for an audit. Every step, from keeping it cold to keeping an eye on containers, comes from a place of knowing what’s at stake—everybody’s health and peace of mind.
Bleach lines the shelves in almost every supermarket and sits in countless homes for good reason: germs, mildew, and tough stains don’t stand a chance against it. While bleach works wonders for cleaning, it brings a set of serious hazards that can’t be brushed aside. Most folks know about the sharp smell, but few stop to consider what that really means—the fumes aren’t just unpleasant, they can irritate the lungs and eyes, even triggering asthma or coughing fits. I’ve seen it myself, trying to scrub a bathroom with windows shut tight; the air gets harsh and heavy fast. People with breathing trouble can feel the sting much sooner, and young kids or the elderly face even greater risks.
Direct contact on the skin stings, sometimes causing burns or rashes, especially during longer jobs or with splashes. A drop in the eye? That means a painful flush with water and a hasty trip to the doctor. Spilling or mixing bleach with ammonia or acidic cleaners ramps things up to a new level of danger—poisonous chloramine gases can fill the room in minutes. Reports from the CDC routinely warn about accidental poisonings, with thousands of cases each year involving mix-ups with cleaning products.
Reading warning labels looks like a chore, but past experience with accidental bleach stains helped me appreciate their value. Bleach doesn’t just wipe out germs; it strips color from clothing, furniture, and even damages floor finishes. That surprise splash can ruin a favorite shirt, but more importantly, accidental contact with food surfaces means health risks climb, especially for children who can touch and taste everything.
In busy homes, diluted bleach left in unmarked spray bottles can mean real trouble. Kids sometimes mistake cloudy liquids for something else, which leads to accidental ingestion—a true emergency. The National Capital Poison Center notes that swallowing even diluted bleach can cause burns to the mouth, throat, and stomach. Vigilance around storage and labeling often makes the difference between clean living spaces and dangerous accidents.
A few changes in how bleach gets handled can limit its risks without sacrificing the disinfecting power people rely on. Gloves make the most obvious difference—hands stay free from irritation, and it’s easier to avoid absentminded face touching. Opening a window or flipping on a fan stirs up good air flow, cutting down on irritating fumes. For surfaces, using just enough diluted bleach gets the job done without soaking everything in chemicals. I’ve learned to mark spray bottles clearly and stash them someplace high or locked up, out of reach from curious hands.
Never combining bleach with anything else ranks at the top of practical tips. Most disasters start with the urge to clean faster or stronger, but no sticky sink justifies mixing products. If bleach does get on the skin or in the eyes, quick action with cool running water helps—a lesson learned the hard way is one not soon forgotten.
On cleanup days, keeping a close eye on children and pets brings real peace of mind. They don’t spot hazards the way grown-ups do, so a bit of patience goes a long way in keeping everyone safer. For anyone wanting to skip bleach but not lose cleaning strength, hydrogen peroxide or soap and hot water offer proven, less risky alternatives.
At the heart of it, respecting bleach’s power—treating it as a tool, not a casual fix—leads to better, safer cleaning habits and keeps households healthier in the long run.
Nobody expects to tip a bottle and watch bright liquid race across the floor, but it happens even in the neatest workplaces. I remember once, at my first job in a garden center, a colleague toppled a jug of concentrated weedkiller. Lesson learned fast: people rarely panic if the group works like a team and keeps clear instructions handy. Fast forward, now spills could involve harsher stuff—cleaners, solvents, something that can harm skin or lungs instead of just grass.
With chemical products, acting on the spot matters. Fact sheets and Safety Data Sheets do not just take up space on a shelf; they break down what’s in the product, exactly how risky it is, and what to do if it spreads somewhere it shouldn't go. I always urge people to read these before getting close to the stuff, not after a spill soaks a rag. Too many people would rather rely on intuition than grab a document.
I learned the importance of air and distance the hard way. In an old paint shop, someone sprayed lacquer and left the door closed. Not fun. If a spill happens, open windows and turn on fans. Avoid breathing in fumes, and stop others from wandering close—this isn’t curiosity hour. Take off any dirty gloves, jackets or shoes and place them out of reach of others. You want to stop the product from following you home, literally or on your shoes. If the spill hits skin or eyes, rinse with plenty of water right away. At many factories, big yellow showers and eye-wash stations stand by for only these emergencies.
Make sure every worksite has an emergency clean-up kit ready. This means gloves made of the right stuff (some solvents laugh at regular disposable gloves), absorbent towels or powders, and tough trash bags. Read the label: some chemicals want different absorbents, and some will react with the wrong powder. Dispose of soaked towels or clean-up powders as hazardous waste, not regular trash. Cities often set up drop-off days for dangerous waste—skipping this leads to bigger headaches for garbage workers and the neighborhood.
I never believed in crossing my fingers and hoping for the best. Workplaces need real training, not a half-hearted safety video. Run drills. Ask people—could they find the chemical's first-aid directions with their eyes closed? Would they spot a warning sign if it changed color or smell? Only experience drills like these stick in memory. Even in homes, a YouTube video on product safety beats a shrug, and kids pick things up fast.
Communication makes all the difference. Hang up laminated step-by-step instructions wherever products are kept or used. Encourage people—kids and adults—to call a poison center in case of confusion. It’s better to ask for professional advice than scroll through random forums or rely on folk knowledge. The American Association of Poison Control Centers takes over two million calls a year, and most get resolved with no trip to the ER. Thinking ahead pulls its weight.
Respecting these products means owning the responsibility for the messes they can cause. Whether you work in a warehouse, clean apartments for a living, or tinker at home, never treat accidental exposures like “just another task.” Lives and safety depend on a fast, informed, and cautious response. Clean up isn’t glamorous, but it’s the real work of looking after each other and the planet.
Few folks spend their days thinking about Diisopropyl Peroxydicarbonate, but in labs and chemical plants, this compound carries risk. It’s a strong oxidizer. It turns dangerous when handled carelessly or stored without attention to detail. Chemical burns, toxic fumes, and the possibility for sudden combustion come straight to mind. Having watched seasoned chemists and newcomers alike, I’ve seen respect for proper protective gear develop the hard way—nobody wants to learn from a near miss.
Diisopropyl Peroxydicarbonate splits apart easily, releasing carbon dioxide and isopropanol. That’s chemistry talk for “things can go wrong fast.” Just a little contamination, friction, or jump in temperature turns a routine task into an emergency. There’s no bragging when you’re treated for inhalation or a flash burn. The right equipment offers a real barrier between you and the chemical—no cutting corners.
A splash on bare skin leaves a mark. The best approach: wear a lab coat or chemical-resistant suit that covers you from neck to ankles. Cotton loves to catch fire, so synthetic, flame-resistant materials offer a safer bet. In a facility using Diisopropyl Peroxydicarbonate, I once saw someone trade a loose, well-worn tee for a crisp Tyvek suit before opening a drum. Nobody laughed. Everyone respected the choice.
Standard latex tears or degrades after exposure to strong oxidizers. Nitrile or neoprene gloves stay strong. It pays to check them for holes before every use—just slide in a hand and flex each finger—and toss them by the end of the shift. A double-glove method, with one layer under a thicker, chemical-resistant pair, reduces the chance for leaks. Friends working in chemical production have told me that spending a bit extra on sturdy gloves often prevents hours of discomfort or worse.
A splash guard or goggles do more than keep dust out. That foggy rush on your glasses can mean exposure to reactive vapors. For Diisopropyl Peroxydicarbonate, goggles with side shields block sideways sprays, and a face shield provides a second layer during large transfers. An experienced supervisor explained that losing sight, even for a few days, changes a person’s view on “it’ll never happen to me.” There’s never a smart reason to skip eye protection in this environment.
Some procedures create vapors that harm lungs over time or all at once. Respirators with organic vapor cartridges or supplied air lines give real peace of mind. This isn’t just a rule—it’s something enforced for everyone. Checking fit and seal before use takes a minute, but that minute matters, especially for folks like me with asthma or allergies. Trust gets built not just through compliance, but through direct experience—nobody wants a coworker gasping in pain.
A sharp storage area, well-marked and ventilated, lessens the hazard. Emergency rinses—eyewash and showers—always close by, never stacked behind boxes. Regular training isn’t busywork. Updates about better gloves or new goggles make a difference. As the saying goes around most facilities I’ve visited, safety grows not from fear, but from routine, practiced care. Every worker, no matter how new or seasoned, has a stake in getting home with all their senses intact. Diisopropyl Peroxydicarbonate doesn’t forgive a lapse, but the right gear gives everyone a fighting chance.
| Names | |
| Preferred IUPAC name | Bis(1-methylethyl) peroxydicarbonate |
| Other names |
Peroxydicarbonic acid, bis(1-methylethyl) ester, mixture with dialkyl peroxydicarbonate Peroxydicarbonic acid, bis(propan-2-yl) ester, mixture with dialkyl peroxydicarbonate Diisopropyl peroxydicarbonate, mixture with dialkyl peroxydicarbonate |
| Pronunciation | /ˌdaɪ.aɪˈsɒ.prə.pɪl pəˌrɒk.si.daɪˈkɑː.bə.neɪt/ |
| Identifiers | |
| CAS Number | ["105-64-6"] |
| Beilstein Reference | 127873 |
| ChEBI | CHEBI:87701 |
| ChEMBL | CHEMBL1707922 |
| ChemSpider | 13666704 |
| DrugBank | DB11234 |
| ECHA InfoCard | ECHA InfoCard: 01-2119951482-36-0000 |
| EC Number | 221-109-1 |
| Gmelin Reference | 1391197 |
| KEGG | C19145 |
| MeSH | Ester Peroxides |
| PubChem CID | 11521 |
| RTECS number | UX8575000 |
| UNII | FCB12L361H |
| UN number | UN3108 |
| Properties | |
| Chemical formula | C10H18O6 |
| Molar mass | 234.25 g/mol |
| Appearance | Colorless liquid |
| Odor | Faint, pleasant |
| Density | 0.975 g/cm3 at 20 °C |
| Solubility in water | Insoluble |
| log P | 0.05 |
| Vapor pressure | 0.1 kPa (20 °C) |
| Magnetic susceptibility (χ) | -9.6e-6 |
| Refractive index (nD) | 1.398 |
| Viscosity | 2.54 mPa·s at 20°C |
| Dipole moment | 0.00 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 290 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -616.7 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -7411 kJ/mol |
| Pharmacology | |
| ATC code | D08AX |
| Hazards | |
| GHS labelling | GHS02, GHS07, GHS05, GHS08 |
| Pictograms | GHS02, GHS07, GHS08 |
| Signal word | Danger |
| Hazard statements | H242, H302, H317, H319, H332, H335, H400 |
| Precautionary statements | P210, P220, P234, P235, P280, P234+P410, P370+P378, P403+P235, P411+P235, P420, P501 |
| NFPA 704 (fire diamond) | 1-4-4-OX |
| Flash point | 40 °C (104 °F) |
| Autoignition temperature | 50°C |
| Explosive limits | Explosive limits: 2.9%–8.5% |
| Lethal dose or concentration | Lethal dose or concentration: LD₅₀ (oral, rat): > 5000 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral (rat): > 5,000 mg/kg |
| NIOSH | UN3107 |
| PEL (Permissible) | 300 mg/m³ |
| REL (Recommended) | 40 mg/m³ |
| IDLH (Immediate danger) | Unknown |
| Related compounds | |
| Related compounds |
Diethyl peroxydicarbonate Dibenzyl peroxydicarbonate Di-n-propyl peroxydicarbonate Di-sec-butyl peroxydicarbonate Di-tert-butyl peroxydicarbonate |
