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Looking back, Dinonanoyl Peroxide has grown from obscure roots. Chemistry has a knack for producing simple compounds with big personalities, and this peroxide sets a clear example. In the early 20th century, organic peroxides started gaining attention for their potential in industrial chemistry. Dinonanoyl Peroxide owes its discovery to the push for new initiators in polymer science. Early researchers, keen on tinkering with carbon chains and looking for better ways to spark reactions in plastics, crossed paths with longer-chain peroxides. Once this compound showed up in labs, the push shifted from curiosity to utility. Over decades, as demand for specialty chemicals rose, so did the recipe for making and handling this peroxide. Each wave of research, whether focused on process safety or cost reduction, added new bricks to the foundation we stand on now. Improvements in organic synthesis, better understanding of peroxide stability, and industrial-scale production all play into today’s relationship with Dinonanoyl Peroxide.
People familiar with organic peroxides soon learn there’s no such thing as a “one-size-fits-all” compound. Dinonanoyl Peroxide carves out its niche as a specialty initiator in free-radical chemistry. Known for kicking off reactions at moderate temperatures, it holds a place in the chemist’s toolbox that bridges the gap between low-volatile options and those that run too hot for comfort. Its solid form—generally a fine, flaky powder—calls for respect but not fear. Anyone who’s spent time in an industrial lab knows that handing off a canister of this stuff means treating it with the sort of seriousness you reserve for a loaded mousetrap.
Dinonanoyl Peroxide stands apart from relatives like benzoyl peroxide and lauroyl peroxide based on the length of its carbon tail. This subtle feature nudges a whole list of its traits. The compound typically appears as a white to pale yellow solid, barely soluble in water but ready to mix with organic liquids. It cracks apart at a lower temperature than some shorter-chain cousins, setting off free radicals just as the heat rises past normal room temperature. The smell, as with many organic peroxides, hints at fatty acids. Everyone who’s tried preparing a batch in the lab probably remembers both the aroma and the caution that goes with strong oxidizers. Chemically, this peroxide doesn’t greet metals with open arms; it prefers the company of other organic compounds, making it effective in controlled reaction environments.
Nobody walks away from a conversation about peroxides without talking safety. Labels for Dinonanoyl Peroxide should get checked before every use, not just during audits. From percentage purity to grain size and recommended storage temperature, these details matter. Labs and factories both count on precise measurements—99% purity isn’t a guess, it’s a requirement to avoid unwanted reaction surprises. Keeping this compound cool, usually below 30°C, shields users from its touchy side. Labels spell out “oxidizer,” and for good reason, reminding everyone to skip matches and heat sources. Proper storage—dry, away from direct sun—writes the first line of defense against shelf-life disappointments or, worse, accidents.
Making Dinonanoyl Peroxide takes a steady hand and a well-ventilated fume hood. Most syntheses leverage a reaction between nonanoic acid and hydrogen peroxide under acidic conditions. Acids like sulfuric or p-toluenesulfonic help catalyze the reaction, forming the peroxy bridge that defines the whole molecule. Step out of line for just a moment—wrong temperature, slip with the acid, overdosed peroxide—and things spiral quickly. Chemists respect peroxides for their sensitivity, and this respect translates into regular checks, slow addition, and lots of ice water. Once formed, the solid needs to dry safely, often on glass sheets, in small smears to avoid too much mass building up in one place. Every step, from mixing to drying, demands vigilance. Anyone who’s heard peroxide stories knows why the old safety manuals overflowed with “never scale up without a plan.”
Dinonanoyl Peroxide bases its value on its ability to break cleanly into free radicals, setting off polymerizations and crosslinking reactions in plastics, resins, and specialty coatings. Unlike more famous peroxides, its radical breakdown produces fragments with just enough punch to drive forward reactions without scorching delicate systems. People have tried tailoring its breakdown rate by adding co-initiators or tweaking reaction temperatures, and data support real gains in process control. Other experiments swap the nonanoic acid for related fatty acids, customizing reactivity and shelf stability. Modifications often walk a narrow path between improved handling and lost potency; the chemistry rewards those who understand just how easy it is to tip from “useful” to “reluctant” or “dangerous.”
Like nearly every organic peroxide, Dinonanoyl Peroxide often hides behind alternate names in catalogs and research papers. Some chemists call it nonanoic acid peroxide. Others refer to its more formal systematic name, peroxydinonanoic acid anhydride, or abbreviate it in laboratory shorthand. This web of names sometimes confuses newcomers, but each tag ties back to the same handful of key chemical principles. No matter which name lands on the bottle, experienced researchers know to double-check the CAS number before assuming anything about safety or compatibility.
Diving into a tub of Dinonanoyl Peroxide without clear safety habits is a stunt destined for regret. The peroxide class always comes with a risk of spontaneous breakdown and fire. Safe handling never gets casual; every movement—opening, weighing, dissolving—deserves careful attention. Gloves, face shields, and flame-retardant lab coats stand between lab workers and chemical burns or eye injuries. Storage away from heat sources, acids, and reducing agents counts as more than advice; it’s a rule set by past accidents and preserved in photos of scorched benches. Procedures built on lessons from old mishaps keep everyone on the safe side, and regular drills on spill response and fire suppression prove their worth every year.
Outside the research lab, Dinonanoyl Peroxide finds its strongest support among polymer manufacturers and specialty plastics makers. Its knack for controlled, moderate-temperature radical generation supports production of optical fibers, adhesives, and flexible plastics. By launching the polymerization process smoothly, it helps producers lock in desirable texture or chemical resistance in their final product. It steps aside from the blunt approach of older peroxides, letting manufacturers fine-tune their processes for new blends or stricter safety standards. I’ve seen plant chemists explain how swapping to this initiator can shave rework hours or win tighter regulatory approval simply by lowering residual monomer counts in finished goods. In more niche corners, it shows up in specialty resins and some coatings that demand just the right balance between speed and temperature sensitivity. Even though it doesn’t make the news like more volatile cousins, it carries its share of the load in modern materials science.
Chemists and chemical engineers keep pushing boundaries. Current studies keep tabs on Dinonanoyl Peroxide’s role as a greener or safer alternative. Researchers compare its reactivity with that of other peroxides, hunting for the lowest possible footprint and highest yield. Analytical methods improve almost every year, with better ways to detect trace impurities and study radical generation under real-world conditions. Some groups run life-cycle assessments, asking how much of the peroxide ends up in waste streams, what happens under recycling conditions, and where breakdown products go in the environment. Others focus on tweaking its molecular structure, putting faith in minor substitutions to unlock lower volatility or even broader application ranges. Every advance in understanding tends to filter outwards, helping regulatory agencies write smarter rules and giving plant chemists new tricks.
Safety extends from process controls out into questions of human health. Toxicity studies on peroxides rarely paint them in a soft glow. Animal and in vitro tests show that like its relatives, Dinonanoyl Peroxide poses risks if inhaled or absorbed through the skin. Strong irritant reactions stand as the biggest danger in poor ventilation, and repeated exposure can sensitize skin or lungs. Acute toxicity usually comes down to the dose; the chemical itself isn’t wildly different from better-known peroxides in hazard level, but its handling in bulk increases risk. Toxicity data drive rigorous workplace limits and insist on physical barriers. The conversation keeps evolving—each new paper adds a data point to guidelines shaping PPE requirements, medical monitoring, and spill response practices in both manufacturing and research settings.
Predicting where Dinonanoyl Peroxide points next brings up questions tied to green chemistry and innovation. On one side, industrial users demand tighter control, both for safety reasons and for cutting raw material costs. On the other, environmental concerns push for cleaner breakdown and reduced waste. With regulatory eyes shifting toward microplastics, peroxides that help polymer manufacturers switch to biodegradable or recyclable resins will earn more attention. Research pushes for broader use in composite materials and 3D printable resins. Each new bit of insight—better shelf-life, more convenient dosing, customized temperature triggers—brings the field closer to safer, more efficient materials. As someone who’s spent time on both research and production floors, I see opportunity here: partners across disciplines sharing data openly, asking hard questions, and focusing on improvements that don’t just pencil out on a spreadsheet but make a real difference at the drum, in the product, and for the people handling these chemicals every day.
Walk into any hardware store and shelves brim with plastic containers and tools. Each one, at some point, owed its solid shape to a chemical called a polymer. Dinonanoyl peroxide pushes the process forward, turning a thick soup of raw materials into tough, usable products. Technically, this compound works as a radical initiator, sparking those chain reactions in the lab so polyester resins can harden. Acrylate-based glues and fancy insulation foams both rely on it. Without compounds like dinonanoyl peroxide, shaping things like auto parts, shoe soles, or circuit boards would drag on forever or fall flat altogether.
Think about rolling a car tire or bouncing a rubber ball. Inside both, there’s a complicated tangle of molecular links holding things together. Rubber needs a careful dance between flexibility and strength, so it doesn't melt in summer or crack in winter. Dinonanoyl peroxide steps into that zone, where heat and pressure transform crumbly rubber into hospital seals, floor tiles, and weatherproof gaskets. Compared to other cross-linking agents, this compound throws less smoke, doesn’t leave behind weird odors, and helps mix in color or fillers cleanly. In all my years reading safety sheets and talking to seasoned engineers, it’s always clear that strong but flexible rubber depends on tight process control, and dinonanoyl peroxide makes that easier.
Many folks worry about what goes into plastics and rubbers. Regulations push manufacturers to reduce risky side products and embrace compounds that won’t trash the environment. Dinonanoyl peroxide stands out for its performance at moderate temperatures. Factories don’t need to crank up the burners as much, cutting both energy costs and emissions. Waste management doesn’t spiral out of control, either. In an age where every manufacturer faces pressure to explain their chemicals, using a steady, well-understood initiator matters. From REACH guidelines in Europe to U.S. EPA oversight, companies recognize that the old wild-west approach to chemical processing no longer flies.
No one should downplay the risks. Dinonanoyl peroxide, like its cousins, stores mighty energy in its bonds. Mishandling leads to fires or worse. That’s why training matters as much as infrastructure. Every plant that stores or handles these peroxides must use reinforced containers, fire suppression systems, and tight procedural controls. Plant managers invest in cooled storage rooms, regular inspections, and up-to-the-minute accident drills. In community meetings, people want honest talk about risks and how companies prepare for the rare emergency. I remember once sitting through a long Q&A with local firefighters at a site using organic peroxides; strong programs build trust, while shortcuts cost reputations in a hurry.
Engineers chase two things: more efficient outputs and greener chemistry. Some start-ups and university teams look at alternative radical sources, maybe enzymes or photoinitiators. For now, dinonanoyl peroxide’s clear performance history and steady handling still win over major manufacturers. I’ve seen research labs push the boundaries by tweaking mixtures and fine-tuning catalysts, but the old standbys rarely fall out of favor overnight. As long as demand for durable plastics and advanced rubber products continues, products like dinonanoyl peroxide will keep their place in the supply chain. The challenge lies not only in improving the chemistry but also in broadening worker training and transparency with communities.
Diving into lab chemicals brings new faces like dinonanoyl peroxide. Handling unknown materials sparks old memories of tight gloves and cautious respect, especially if there’s a whiff of peroxide in their name. This particular compound falls into the category of organic peroxides. Anyone who’s cracked open a textbook or got chemical splatter on their shoe knows this type of chemical doesn’t belong in casual, bare-handed routines.
Most people have heard nightmares about peroxides that explode out of nowhere, and those stories don’t come from nowhere. Dinonanoyl peroxide breaks down easily under heat, friction, or even when it gets poked by incompatible chemicals. The breakdown releases oxygen fast and sometimes, with a lot of force—imagine the energy packed in a stretched rubber band. It can ignite nearly everything in sight. In many accidents, the problem started with someone thinking a small bottle looked harmless, or that quick contact with skin wouldn't do much.
The National Institute for Occupational Safety and Health treats organic peroxides as chemicals with special handling needs for a reason. Chemistry journals point to peroxide accidents that left behind burns and destroyed benches. Most organic peroxides, especially those that reach content near 100%, count as high explosives. Dinonanoyl peroxide sits in this group. If the label says “Content ≤ 100%”, treat it as if it’s loaded to the brim, ready to react the moment a mistake happens.
Eyes and skin injuries happen easily with peroxides. Even small amounts irritate skin, and fumes can leave people coughing or worse. Breathing in dust, even accidentally, puts the lungs at risk. In the fire department’s hazmat training, we learned to worry not just about flames but about the invisible risk: old, partly crystallized organic peroxides can go off with just a knock on the bottle.
Every safe chemist I’ve met keeps their workspace cold and dry for peroxide storage. Heat puts stress on the chemical bonds. Good ventilation matters—organic peroxide fumes don’t belong in your lungs, and a strong breeze carries them away. Never open peroxides near open flames or sparks. Even static electricity from a sweater can spell disaster.
No dispenser can replace vigilance. Eyeshields, face masks, and double gloves become second nature when working with peroxides. Setting up a sturdy shield between myself and any transfer lets me breathe easier. Disposal means treating leftover material as hazardous waste, labeled and sealed, then handed off to professionals who specialize in chemical destruction.
Best practice involves only using as much dinonanoyl peroxide as the experiment calls for. Above all, avoid stockpiling. Strict inventory logs keep track of how long each bottle has been open; older containers run a higher risk of decomposition. Replace containers routinely and err on the side of caution—mother nature and chemical suppliers can always make more, but there’s no replacement for safety.
Schools, universities, and factories working with anything like dinonanoyl peroxide owe it to everyone under their roof to run proper safety drills. Knowing what to do in an emergency, from chemical showers to eye rinse stations, changes panic into action. History doesn’t have much sympathy for people who cut corners in chemistry. Dinonanoyl peroxide deserves the same care as its more famous cousins, not because it’s especially rare, but because even a routine day can turn dangerous if respect slips.
Dinoanoyl peroxide falls into the category of organic peroxides—compounds built for tough jobs, often found in plastic production or similar fields where molecules need breaking down or binding up. Yet, this chemical is no everyday household peroxide. It’s powerful and, under certain conditions, can turn unpredictable fast. Sitting on a shelf, it looks harmless. In practice, it holds serious potential for combustion or even explosions. Stories from chemical storage mishaps always leave a mark—so many start with someone forgetting just how unforgiving these peroxides can be.
Dinoanoyl peroxide hates warm temperatures. Temperatures above 30°C can send this compound into instability. Once experienced a situation where storage room cooling broke down over a weekend, which caused anxiety for the team handling benzoyl peroxide. Same caution applies here. Refrigerated spaces—think 2-8°C and no direct sunlight—make a huge difference. Heat means higher risk, so cool rooms and good ventilation set the foundation for safe storage.
Organic peroxides and moisture don’t mix. A damp storeroom leads to clumping or slow breakdown, undermining safety. Silica gel packets or dehumidifiers are handy tools for this job. Palletizing drums off the floor also keeps material away from accidental spills, leaks, or rising moisture during wet months.
It’s not just about the immediate risks. Dinoanoyl peroxide must stay well away from acids, bases, reducing agents, and flammable liquids. Closed shelving, designated chemical lockers, and clear labelling help avoid accidental contact. The walls of chemical supply rooms often display lists of incompatible materials—an obvious, but critical step rooted in tough lessons from the past. The fewer the distractions and shortcuts, the safer everyone remains.
A buddy who works in industrial supply tells a familiar story: A tiny spark becomes something bigger when storage areas lack proper airflow. Good ventilation isn’t about comfort; it’s about safety. Peroxides can release gases over time, and build-up in stagnant air pushes the environment closer to disaster.
Everyone from lab techs to warehouse staff benefits from simple, regular training around these chemicals. Inspect packages for leaks, discoloration, or swelling—never ignore anything odd. Even with the best containers, time can work against the stability of organic peroxides. Changing out old stock and rotating inventory beats waiting for trouble.
Accidents happen, no matter the precautions. Easy access to fire extinguishers (class D for oxidizers), emergency showers, and eye stations buys time in those first critical moments. Clear walkways and posted emergency procedures reduce the panic when seconds count. The job doesn’t end with safe storage; it continues with readiness for the unexpected.
Paperwork matters—SDS files, local and federal environmental rules—but real safety comes from hands-on experience and attention to detail. Regulators want proof that storage doesn’t drift into carelessness, so keeping logs and digital temperature records backs up the effort. It’s a challenge for busy teams, yet cutting corners just isn’t worth it.
Diving straight into the disposal of Dinonanoyl Peroxide, there’s no room for error. Anyone who’s handled organic peroxides knows how jumpy these chemicals get, even when sitting in a lab fridge. Mishandling or skipping steps isn’t just a minor slip—it can mean accidental fires or unexpected, dangerous reactions. Those of us who worked in labs or chemical plants have vivid memories of tightly checking all the hazard warnings on peroxide-based materials. The explosions that make headlines almost always come from someone cutting corners.
No one gets to ignore the strict regulations around these chemicals. The EPA and OSHA treat peroxides like Dinonanoyl as real threats. If someone gets caught pouring leftovers down the drain or into a regular dumpster, hefty fines land fast. Besides legal risk, lives remain at stake. Official guidelines exist for a reason—companies found violating those rules end up in court and on the news.
Plenty of folks think they can improvise, but with Dinonanoyl Peroxide, there’s too much heat generated during breakdown for home-brewed solutions. It’s best handed off to licensed hazardous waste contractors. They use neutralization or controlled incineration in reactors designed to catch any runaway reactions. In my earlier years, I once watched a chemical waste facility run a mock drill for a peroxide spill. Their gear looked almost military, with layers of fire retardant and blast shields working as standard kit.
Many manufacturers offer take-back programs, letting customers ship back unused compounds. This keeps the risks in the hands of engineers who know the material. At the very least, unused peroxide should sit in its original container, labeled clearly, with a secure lid, far from heat or sunlight until picked up by certified professionals. Never try to dilute or neutralize organic peroxides with household chemicals—these reactions often go sideways, producing heat, gas, or worse.
Not every chemical user works in a multi-million-dollar plant. University labs and smaller makers need better access to clear instructions and affordable disposal services. Many burn out dealing with mounting costs and paperwork. In my early days, no one taught a dedicated class on chemical waste—almost everything came down to learning from others’ close calls.
Institutions can step up. Sharing resources, centralizing drop-off days, and pooling waste for collective pick-up save money and keep dangerous leftovers away from landfill and sewer systems. Online reporting helps, but face-to-face training gives people a better sense of just how dangerous these materials get as they age. Anyone left guessing at disposal risks needs better support.
Nobody enjoys the extra steps that hazardous waste creates, but everyone working around Dinonanoyl Peroxide owes it to their colleagues and community to avoid shortcuts. Ignoring safe practices lets tragedy walk right in the door. Accidents don’t care if you meant well or were “just trying to get it done.” Years of handling reactive chemicals taught me this truth again and again: one moment of carelessness erases all the safe days that came before.
Safe disposal comes from respect—not just for the rules, but for the unpredictable energy packed into every bottle of peroxide. Spreading the word, backing up young techs with real training, and treating every handoff like it could be the one that goes wrong—these steps truly matter. Every safe handover, every disposal handled the right way, keeps workplaces quieter and neighborhoods safer. That’s worth taking seriously.
My early experience working in labs made me respect substances like peroxides on a practical level. Dinonanoyl Peroxide brings risks you notice the moment it comes out of storage. This organic peroxide can decompose rapidly under heat or shock, releasing gases and energy with almost no warning. During one training exercise, a faulty seal led to a chain reaction that set off a loud pop in our fume hood. We didn’t see flames, but the lesson landed hard—these peroxides don’t forgive mistakes. Several chemical safety databases list this compound among the materials that, even in small quantities, have touched off lab fires or explosions.
Skin and lungs count as silent entry points for danger. Any contact with Dinonanoyl Peroxide can cause burns or inflammation. Friends in chemical manufacturing once described how even brief exposure led to persistent skin irritation. Working unmasked with organic peroxides increases the chance of inhaling particles or vapors, and respiratory symptoms usually follow soon after. Researchers have seen allergy-like reactions among people exposed over time. I always make sure proper gloves and goggles are standard, not just recommendations, because symptoms can show up fast and unexpectedly.
Poor storage only multiplies the dangers. Dinonanoyl Peroxide breaks down at higher temperatures, and common solvents can make things worse. A misplaced container near a heat source or direct sunlight brings immediate danger. Many warehouses use dedicated cold rooms for peroxides, and I have seen audits that flag even minor deviations from temperature guidelines. Fire codes and workplace rules often make organic peroxide storage a top priority. I’ve seen containers kept in locked metal cabinets, away from other chemicals, to reduce temptation for anyone unfamiliar with their quirks.
Tossing Dinonanoyl Peroxide into ordinary waste starts a chain of risks that keeps environmental teams up at night. Organic peroxides react unpredictably with many disposal agents, and landfill disposal doesn’t cut it. We once spent hours packaging small vials in water-filled containers for transport to hazardous waste sites. Regulatory frameworks from OSHA and the EPA have grown strict for good reason. Disposal firms need special licenses and those handling the material have to document every step.
Training probably saves more lives than any material safety sheet. I’ve watched new staff memorize peroxide protocols before they touch anything, and mock spill drills always feel serious. Engineering controls like good ventilation and explosion-proof refrigerators make a difference, but staff discipline—double-checking labels, logging temperatures, scanning for leaks—closes much of the risk gap. Real safety comes from culture, not just rules. Workers who know the hazards take real steps to keep themselves and colleagues safe, day in and day out.
People working around Dinonanoyl Peroxide need real stories and examples, not just chemical formulas. Sharing near-misses and best practices transforms abstract warnings into personal responsibility. Industry groups and regulators use case studies to spread awareness. My own circle of colleagues often trades tips and reminders about staying safe, especially after news of an accident somewhere else. For some chemicals, vigilance never quite goes out of style. Dinonanoyl Peroxide fits squarely in that category.
| Names | |
| Preferred IUPAC name | bis(nonanoyl peroxide) |
| Other names |
Bis(3,7-dinonylperoxy)nonanedioate Peroxynonanoyl peroxide |
| Pronunciation | /daɪˌnoʊˈneɪ.nɔɪl pəˈrɑk.saɪd/ |
| Identifiers | |
| CAS Number | [601-90-9] |
| Beilstein Reference | 82696 |
| ChEBI | CHEBI:9459 |
| ChEMBL | CHEMBL4144745 |
| ChemSpider | 2297621 |
| DrugBank | DB11371 |
| ECHA InfoCard | 03d2651e-ff7e-4ae7-a736-d7aeb5e629a6 |
| EC Number | 208-733-6 |
| Gmelin Reference | 22571 |
| KEGG | C18607 |
| MeSH | D015090 |
| PubChem CID | 139517601 |
| RTECS number | OU6725000 |
| UNII | 7W0F5U76RK |
| UN number | UN3108 |
| Properties | |
| Chemical formula | C18H34O4 |
| Molar mass | 458.66 g/mol |
| Appearance | White powder |
| Odor | Odorless |
| Density | 1.1 g/cm3 |
| Solubility in water | Insoluble |
| log P | 4.62 |
| Vapor pressure | Negligible |
| Magnetic susceptibility (χ) | \( \chi = -9.5 \times 10^{-6} \) |
| Refractive index (nD) | 1.4600 ~ 1.4700 |
| Viscosity | Viscous liquid |
| Dipole moment | 4.81 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 519.9 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -523 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -6208.7 kJ/mol |
| Pharmacology | |
| ATC code | D10AE01 |
| Hazards | |
| Main hazards | Oxidizer, explosive, harmful if swallowed, causes skin and eye irritation. |
| GHS labelling | GHS02, GHS07, GHS05, GHS08 |
| Pictograms | flame, exclamation mark |
| Signal word | Warning |
| Hazard statements | Hazard statements: H242, H302, H317, H332, H335, H410 |
| Precautionary statements | P210, P220, P234, P234+P410, P280, P281, P302+P352, P305+P351+P338, P370+P378, P411+P235, P420, P501 |
| NFPA 704 (fire diamond) | 2-4-4-OX |
| Flash point | > 60 °C |
| Autoignition temperature | >120 °C (DIN 51794) |
| Explosive limits | Explosive limits: 2.5–91% |
| Lethal dose or concentration | LD₅₀ oral (rat): >5000 mg/kg |
| LD50 (median dose) | LD50 (median dose): Rat oral > 5000 mg/kg |
| NIOSH | Not established |
| PEL (Permissible) | PEL (Permissible Exposure Limit): Not established |
| REL (Recommended) | 1.5 mg/m³ |
| IDLH (Immediate danger) | Unknown |
| Related compounds | |
| Related compounds |
Nonanoic acid Nonyl alcohol Decanoyl peroxide |
