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A walk through the history of Di-Tert-Butylcumyl Hydroperoxide brings up the energy and curiosity that has driven chemical innovation over the past century. Some chemicals change industries overnight; others quietly stretch their influence in countless compounds and processes. This hydroperoxide, which falls in the range of 42% to 100% content with up to 57% inert solids, showed up in scientific papers and patents as a niche initiator. Its character snuck into applications wherever consistent but vigorous oxidation was called for. Early research barely imagined the sheer reach this molecule would achieve, especially when synthetic rubbers, plastics, and specialty polymers built up demand for more reliable initiators than old standbys.
Lab memories from graduate school — late nights, glassware etched by trace acids, tempers running short — remind me how unpredictable early peroxide work could get. Folks spent as much time scrubbing safety goggles as tracking product yields. Di-Tert-Butylcumyl Hydroperoxide, though, soon became a household name in research spaces dedicated to controlled polymer formation or targeted oxidation, mainly because its performance stood up under thermal, chemical, and logistical strain. Over time, the methods for synthesizing and purifying the stuff grew repeatable, reducing much of the risk that haunted its earliest days.
A bottle of Di-Tert-Butylcumyl Hydroperoxide wears its personality on its sleeve. Colorless to faint yellow, this liquid shouts caution with its strong acrid odor; it’s no friend to delicate noses or careless skin. You can often pick up hints of its volatility long before any spill triggers alarms. Chemists keep a wary distance, respecting a flash point that demands careful storage — usually away from heat, sparks, and sunlight. Its high oxygen content and unstable O–O bonds mean it wants to break apart, driving the chemical initiations that underpin its main uses. The substance finds itself riding the line between a tool of creation and a hazard that punishes lapses. Its density, solubility, and viscosity challenge handlers to know their way around pumps, containers, and temperature controls. Techniques for detecting and quantifying impurities improved over the years, giving producers new ways to cut down on side reactions and enhance shelf life.
Most of the time, the blend includes solid carriers to help manage the liquid’s energy. Blending with inert materials lessens the risk of runaway reactions that, in less regulated setups, could make headlines for all the wrong reasons. Chemists learned to rely on detailed labels, up-to-date safety charts, and plain old experience for each batch, since small formulation differences can tip the balance between safe handling and a laboratory incident. As more data rolled in from factory floors and application sites, it became clear that no shortcut replaces deep training in chemical handling.
The technical hoops around Di-Tert-Butylcumyl Hydroperoxide make it a textbook example of chemistry creeping into everyday life, unseen by most. Regulators insist on tight labeling rules, with concentration, carrier type, hazard classes, risk phrases, and batch data spelled out for anyone opening a drum or canister. It takes discipline to stick to these protocols; cutting corners isn’t an option. Thoughtful labeling doesn't just tick regulatory boxes — it keeps people safe who may never have studied organic chemistry. Supporting documents usually include a full breakdown of impurities, storage advice, stability predictions, exposure limits in ppm or mg/m³, and immediate emergency protocols. Modern standards call for regular recalibration of measurement devices, so readings remain trustworthy. Failing to keep up would turn an everyday chemical into a workplace headline.
I remember a plant manager who once quipped: “The bottle's fine if you respect it. Slack off and it’ll bite you.” Strict technical specs shape how warehouses stack and shift inventory, how shipping companies route deliveries, and even how R&D staff plan new product trials. In practice, this all plays out far from the lab benches, translated into workplace rules and daily checklists.
The manufacturing path for this hydroperoxide draws together classic batch chemistry with newer, safer approaches. Early on, the process called for controlling air flow, strict cooling, and exact catalyst choices to get the oxygen atoms arranged just so. Small mistakes produced waste, or worse, accidents, so new process controls — including real-time temperature sensors and closed-loop systems — went from luxury to necessity. Later, plants introduced continuous production designs, reducing exposure and giving tighter end-point control. Real-world experience showed that switching solvents or tweaking reactant ratios had a bigger effect than textbooks predicted. Teams rebuilt workflows to cut down on off-gassing and improve capture of trace byproducts, minimizing the risk of both product contamination and air pollution.
The chemistry behind modifications showcases old-school ingenuity. Adding to or changing the hydrocarbon backbone alters the reactivity of the peroxide group, giving polymer chemists the freedom to adjust cure rates or restrict side reactions. This has big implications for every industry that depends on well-timed polymerization, from car tires to insulation foam. Chemical engineers have picked up on new catalyst formulations and blending tricks to reduce instability and waste, but these advances always circle back to safety checks — a lesson chewed in through a century of trial and error.
On paper, a single compound often picks up a dozen names. Labs and factories stuck to naming conventions like ‘Cumene, α,α,4-triisopropyl-4-hydroperoxide’ or ‘DTBCH’ to avoid confusion in orders and batch releases. Scientific publications rely on International Union of Pure and Applied Chemistry (IUPAC) nomenclature, but warehouses might list versions like ‘Peroxide, Di-tert-butylcumyl’ or other trade names connected to region or manufacturer. Whatever the alias, the chemical’s signature effects travel with it. Mislabeling shows up in root-cause analyses after close calls or accidents, fueling better database management for chemical stocks everywhere. Accurate naming doesn’t just help scientists; it keeps the whole distribution chain running smoothly and safely.
My own trials with peroxides brought home that safety never grows automatic. Gloves degrade, fume hoods clog, signs fade. The key is cultivating habits — not just checking the box, but really thinking about what could go wrong. Facilities that handle Di-Tert-Butylcumyl Hydroperoxide put their trust in repeat training, spot audits, and backup systems. Eye washes and emergency showers sit close at hand, maintained on strict schedules, and no one argues when someone calls for a safety drill. Chemical storage separates incompatible families, and manifest logs keep a real-time record of usage. Ventilation systems undergo regular testing, and accidental release protocols often include both remote venting and blanket isolation to buy time for first responders.
Regulations pile up from every angle, but real-world compliance blooms from a shared sense of what’s at stake. Peer-to-peer instruction beats out endless paperwork. Teams that prioritize clear communication and regular upskilling tend to post the fewest near misses. Beyond regulatory fines and company reputation, these practices build the kind of workplace confidence that carries into every project, big or small.
Few chemicals leap between so many industries without skipping a beat. Di-Tert-Butylcumyl Hydroperoxide drives the polymerization reactions at the heart of modern plastics, helping to set the properties manufacturers rely on for strength, flexibility, and resistance to heat or chemicals. In rubber curing, its reliability stands out compared to legacy initiators, reducing batch failures and boosting production uptime. Crosslinking agents like this also find their way into coatings, adhesives, and elastomers. The shift toward green chemistry and resource-sensitive manufacturing spurred a wave of investigations into reducing the environmental footprint of initiators, with Di-Tert-Butylcumyl Hydroperoxide often sitting at the center of those debates — a reminder that even “invisible” chemicals ripple out through the supply chain, policy, and sustainability metrics.
On the research side, scientists chase ways to harness this compound for novel oxidative procedures, aiming for milder, cleaner reactions that can trim away hazardous byproducts. Plenty of patents now describe tweaks to old recipes, trying to squeeze out gains in efficiency or drop the overall environmental impact a notch further. I’ve followed some startups turning to this class of hydroperoxides for next-gen solar cell encapsulants or bioinspired materials, though the bridge from lab prototype to factory floor remains daunting.
It’s no exaggeration to say that the long-term prospects for using Di-Tert-Butylcumyl Hydroperoxide depend on what toxicology keeps finding. Early suspicions attached to most peroxides, as few of them offer much leeway for careless exposure. Eye and skin contact can bring quick, sharp injuries; inhalation at high concentrations pushes symptoms from mild eye redness to severe respiratory effects. The last few decades poured more resources into testing metabolite profiles, decay products, and chronic toxicity markers. Though acute toxicity generally ranges lower than some of its nastier relatives, the risk of systemic damage from repeated or accidental exposure drives ongoing reassessment by agencies and industrial hygienists.
Developments in workplace monitoring plugged gaps where exposure checks once lagged. Portable detectors, badge-based personal monitors, and air sampling replaced guesswork with real-time numbers. Risk profiles got sharper, which in turn allowed for more targeted training and investment in safer production lines. Calls for green substitutes reflect not just regulatory tightening but an effort to keep long-term workplace morbidity near zero.
The path ahead for Di-Tert-Butylcumyl Hydroperoxide hinges on a mix of practical innovation and regulatory due diligence. Scientists keep hunting for cleaner, safer synthesis methods, eyeing both resource consumption and waste streams. Manufacturers invest in closed-loop systems and digital monitoring, hoping to shave costs and shrink their environmental footprint. There’s growing pressure to find biodegradable or less persistent alternatives for select applications, especially in consumer-driven sectors, but no easy answer has appeared. My strongest memory from industry seminars comes from heated debate over how much risk modern society should bear for materials that enable its comforts. Some wanted faster swaps to new initiators, others warned about trading one hazard for another.
Trust, at the end of the day, comes from relentless commitment to transparency, independent review, and a clear chain of accountability from the supplier through to the end user. The compound’s historical successes and future prospects rest as much on culture as they do on chemistry — a blend of competence, curiosity, and respect for unseen consequences. We owe that not just to workers and scientists, but to every community touched by the processes that begin in flasks and beakers and end in the real world.
Working in chemical manufacturing for over a decade taught me something: small changes in process additives can transform the final product. Di-Tert-Butylcumyl Hydroperoxide, or DTBCHP, might sound like an obscure compound, but this chemical quietly drives progress behind the scenes in the plastics and rubber industries. Even folks outside the lab would recognize its impact in the goods they use daily.
Factories pushing out plastics and synthetic rubbers rely on crisp, controlled chemical reactions. Take polymerization. DTBCHP steps in as a catalyst, specifically a free-radical initiator. What does that mean in real words? It sparks the chain reactions that turn loose monomers into strong, useful polymers. Without reliable initiators like this one, the whole process slows down or veers off course. Manufacturers of polyethylene, polypropylene, and polystyrene keep DTBCHP on hand to ensure production charges ahead smoothly.
From an operator’s perspective, precise initiator blends mean fewer headaches. Shoddy mixes cost time, create safety risks, and eat into profit margins. Factories want consistent melt flow, reliable product strengths, and dependable yields. By providing strong, predictable performance at moderate temperatures, DTBCHP chapters out some of the hassle found with less stable or weaker initiators.
Step into the world of automotive and construction materials. Crosslinked polymers carry high strength, durability, and better resistance to wear or high heat. Crosslinking needs something to start the reactions—here, DTBCHP comes into play again. In the manufacture of crosslinked polyethylene (PEX) tubing or insulation foams, this hydroperoxide becomes the go-to initiator for the crosslinking step. Finished goods come out tougher and last longer, meeting real-world demands for reliability.
Down on the plant floor, efficiency outweighs excitement. Chemical teams want an initiator that delivers steady decomposition rates so temperatures don’t spike dangerously or dips slow production. DTBCHP proves out over time, shaving off unnecessary costs and lowering chances for spoiled batches.
If you’ve ever worked with adhesives, paints, or acrylic coatings, there’s a good chance DTBCHP played a hand somewhere upstream. Specialty resins and acrylics mean tight performance specs—clarity, curing speed, resistance to sunlight. This hydroperoxide helps control molecular weights, guiding everything towards that sweet spot in strength and flexibility. Even in composite manufacturing, which tests every chemical for reliability, DTBCHP repeatedly finds use as an initiator for unsaturated polyester resins.
Unlike some of the more reactive peroxides, DTBCHP balances reactivity with manageable safety. I remember walk-throughs in busy industrial parks, where operators appreciated stable, easy-to-meter additives that didn’t demand hour-by-hour TLC. Storing and transporting less volatile initiators cuts insurance and injury risks, a real financial and moral benefit for any business. At the end of each day, plants need to deliver quality products without trading away worker safety. Regulatory compliance also guides every major manufacturer’s decision, and DTBCHP earns a spot for its practical storage needs.
Companies everywhere face growing pressure to cut waste and reduce emissions. While DTBCHP itself isn't exactly green, process engineers continue to test dosing and recycling setups to maximize every gram. With better monitoring tools and stricter controls, more material stays in use and less gets wasted in the purge streams. Each step towards precision brings the industry closer to truly sustainable manufacturing, a goal that stands to benefit everyone in the supply chain.
Dealing with chemicals at concentrations greater than 42% changes the playing field completely. At these strengths, materials like hydrogen peroxide, hydrochloric acid, or sodium hydroxide won’t just cause a little irritation—they can burn right through skin or give off vapors that hurt the lungs and eyes. Years ago, I worked at a plating shop where caustic chemicals grew stronger with each process. I learned very quickly that a lapse in safety can mean a rushed trip to the ER. Having the product in hand, you don’t just worry about a little splash—strong solutions can sizzle right through normal work clothes and blind in seconds.
Most people picture gloves, but for high concentrations, gloves tell only part of the story. Thick nitrile or neoprene gloves stood between me and disaster more than once. A thin layer or a hole in the glove meant pain—burns, blisters, or worse. Eye protection mattered just as much. Goggles that fit snug, with no gaps, stopped stray drops that surprised me when pouring or mixing. In some shops, face shields made a big difference, especially if walking into a tight space where a splash might come from above or the side. Aprons, long sleeves, chemical-resistant shoes—the more barriers, the better. These weren’t suggestions. OSHA statistics show that skin exposure remains one of the biggest causes of chemical injuries, and reliable PPE greatly reduces this risk.
Strong vapors don’t stay put. I remember a day when someone swapped out the exhaust fan in the etching room for a quieter version. Mist hung in the air, and a few minutes later, blisters formed inside a co-worker’s nose. Proper fume hoods or local exhausts made the air clear again. Simply opening a window never did enough. Good ventilation pulls problem vapors away from people’s faces, making sure that one mistake doesn’t become a trip to the hospital. The CDC recommends engineering controls as the first line of defense, and experience backs that up.
High-strength chemicals chew through storage containers that would easily hold weaker stuff. We stored acids in dedicated acid cabinets, away from bases and anything flammable. Safe containers got checked for cracks or leaks every day, and new shipments never went in before a double check. Temperature swings made bottles expand or shrink, risking pressure build-up and leaks. Labels always faced outward, hazard signs stood large. It takes only seconds for a worker rushing to grab the wrong bottle to make a costly mistake. The Environmental Protection Agency provides strict guidelines for chemical storage, echoing lessons learned in every workplace incident I’ve seen.
No one likes thinking about accidents, but real practice beats panic every time. I saw folks freeze when someone else got splashed, not knowing if they should douse with water or use a neutralizer. We ran monthly drills, making sure everyone could find the nearest eyewash or shower blindfolded. Spills got cleaned immediately, with kits ready and tested. Material Safety Data Sheets were no dusty file—they stayed posted, easy to skim when seconds mattered. Preparedness removes guesswork and gets everyone home in one piece.
Training made all the difference. Before I handled any active chemical, someone more experienced walked me through the risks and the steps to control them. Safety culture grows as workers share what they’ve learned through mistakes and close calls. Fact-based policies, practical drills, and an attitude that no risk is “routine” save hands, eyes, and lives every year. Handling concentrated products isn’t just another part of the job—it demands respect, preparation, and the willingness to ask for help before something goes wrong.
Over the years, a handful of specialty chemicals have tested both patience and wits in the lab. Di-Tert-Butylcumyl Hydroperoxide happens to be one such compound—it’s known for strong oxidation and a knack for instability when handled carelessly. Stories of bottle seals trembling or crystalline clogs forming in cold storage rooms remind any chemist that safety isn’t a checklist, but a daily habit.
Substances like this bring a real sense of caution because their decomposition can go from harmless to dangerous without much warning. Hydroperoxides release oxygen; left unchecked, pressure can build up in a storage vessel. Under the wrong conditions, air and a dash of heat turn anxiety into real-world incidents. Finding the right spot and method for storage can make all the difference.
Direct sunlight or high ambient temperatures speed up decomposition. In my experience, setting the fridge between 2 and 8°C slows things down and reduces energy in the molecule. Bright lab lighting doesn’t help either; ambient UV can trigger a cascade nobody wants to witness. Let the chemical sit in an opaque or amber bottle and keep it away from windows. Not every utility fridge has room for chemicals, but carving out space for compounds like this never feels like wasted effort.
Gloved hands sometimes brush against bottles while searching crowded shelves. For hydroperoxides, glass makes a reliable ally, but I’ve leaned towards polyethylene liners for an added margin of safety. Strong screw caps keep vapors in and moisture out. Labels matter more than some think. Every bottle should show both date received and date opened. Knowing exactly how old the stuff is puts risk in perspective. An extra sticker reading “HEAT SENSITIVE—KEEP COOL” wouldn’t hurt if new staff cycle through the lab.
In tight storage rooms, dangerous neighbours create trouble. Never let acids, bases, reducing agents, or flammable solvents crowd out the shelf next to a hydroperoxide bottle. A spill, however minor, could spark a chain reaction. Locked cabinets or chemical safes fully dedicated to oxidizers help keep reactive families apart.
Fume hoods earn their keep not just for bench work, but as storage for small bottles of reactive chemicals. Strong ventilation draws away stray vapors and limits inhalation risks. In my lab, a simple checklist on the inside of the door reminds people to check for leaks, pressure build-up, or discoloration—signs things might be turning south.
Training remains the unsung hero in chemical safety. People who know what to do, and why, go home safer. Eye washes and spill kits stationed near storage areas offer a last line of defense. MSDS sheets don’t belong in cabinets; they should stand ready, printed, and clipped above emergency stations for quick action when seconds count.
Regular audits clear out forgotten stock and remind everyone about proper storage. Implementing a system where unused chemicals get returned for safe disposal saves headaches down the road. Investing in insulated cabinets and spill-proof shelving goes far beyond compliance checklists; it’s about creating a culture where people value their own safety and the safety of others.
Ask anyone who’s spent time near a chemical drum or scrubbed out a beaker in a school lab—chemicals have a knack for causing trouble fast. Even those labeled “safe” deserve respect. I remember an intern sneezing through a basic bleach solution cleanup. Eye protection ended up being the only thing between him and a painful ER visit. That's the thing about personal protective equipment: it acts as the last barrier, catching what slips past every other safety process.
Some folks rely on the basics—goggles, gloves, aprons. That’s only the start. Nitrile gloves keep a lot of solvents out, but acids like hydrofluoric eat right through. Every chemical needs its match, so the right glove material matters. Rubber gloves do little against aggressive organic chemicals. Contractors working with ammonia or bleach quickly learn vapor jumps through cotton coveralls, flooding skin and lungs with burning fumes.
Let’s talk eye and face protection. Cheap plastic goggles offer better protection than regular glasses in a pinch, but truly nasty chemicals require goggles with indirect vents. Splashing acids into an eye leaves damage that never fully heals. Full-face shields offer another line of defense when mixing high-risk liquids. I still remember a colleague who avoided a face full of splashed sodium hydroxide by trusting her shield.
Don’t skip over respiratory protection. Dust masks barely slow down most vapors, so cartridges must match the hazard. Chlorine gas, acidic mists, and toxic organics flood lungs without proper filters. Fit matters too; I’ve seen workers with loose masks complain about headaches and burning throats after short shifts. A respirator that gaps at the nose or jaw doesn’t count for much.
Suiting up means more than grabbing gloves and calling it safe. You have to check if everything is free from cracks, tears, and chemical stains. In hot weather, workers pull off goggles for relief, sweat quickly mixing with chemicals on their skin. The real world crowds safety out, so regular checks and training matter more than any poster on the wall. Daily routines turn into muscle memory that saves vision, protects lungs, and keeps skin from blistering.
Everyday talk in labs and factories circles back to three things: know the risks, match gear to the job, and fix hazards before slipping into routine. Safety data sheets prove their worth here. They spell out the minimums—what gloves shield skin, which respirator makes sense, and why that particular apron holds up better. Supervisors can double-check by running drills and replacing worn-out PPE faster than schedules suggest.
Companies spend money on the best PPE, but none of it pays off unless people wear it the right way, every time. Choices made in moments—like rinsing off gear after a splash or donning an extra layer before approaching a tank—build a safety culture that lasts long after inspections are over.
No single answer covers every chemical, but years of watching accidents teach that shortcuts never pay. Trusted brands and double checks help, but real safety grows from everyday habits—reading a label, reporting a tear, properly disposing of chemical-soaked gloves. Worker feedback on comfort and fit has real value, since uncomfortable gear lands unused on the nearest bench. The investment matters most when leaders listen and adapt, turning basic rules into daily protections that actually stick.
Dealing with waste that contains Di-Tert-Butylcumyl Hydroperoxide mixed with inert solids—at or below 57%—calls for real caution. This isn’t just about good housekeeping. The stuff comes with risks that you don’t shake off with a broom and a dustpan. Di-Tert-Butylcumyl Hydroperoxide is a strong organic peroxide. A spill or a misstep with disposal can mean fires, toxic fumes, or even explosions. This isn’t a distant danger; it’s a reality that’s led to workplace injuries and environmental citations. I’ve worked in labs where we handled hydroperoxides, and the level of respect this class of chemicals demands stays with you.
Rules from the EPA and local agencies exist for good reasons. They don’t just make for heavy reading; they mean you avoid fines, health hazards, and PR nightmares. The EPA places peroxides squarely in the hazardous waste camp. Waste with less than 70% active peroxide content, especially when mixed with other solids, still counts as hazardous unless specific exclusions apply. Transporting and dumping this type of waste in a regular landfill not only breaks the law but ups the risks for municipal workers and endangers groundwater supplies. The Resource Conservation and Recovery Act wants you to keep these dangers far from ordinary disposal channels.
The safest route I’ve seen involves treating anything with Di-Tert-Butylcumyl Hydroperoxide as hazardous from the moment it leaves the bench. This means storing the waste in certified, non-reactive containers with tight-fitting lids—never glass, since shock can shatter it and trigger trouble. Avoiding sparks and open flames in storage areas makes good sense, since organic peroxides can ignite without much provocation.
Marking the package with chemical names and concentration offers real help during emergencies. Unlabeled waste can turn a small accident into a nightmare for hazmat teams. Waste disposal companies familiar with organic peroxides become your best allies. I’ve seen how much safer things can run with trained handlers. These firms usually incinerate the waste at high temperatures in specialized facilities. This method destroys both the chemical and the organic part safely, minimizing the risk of byproducts escaping into the environment.
Staff need recurring safety training. Just once a year isn’t enough because high turnover and shifting duties can leave knowledge gaps. Training gives people the confidence to handle disposal steps and keeps mistakes rare. I’ve taken part in workshops where we drilled spill response and disposal protocols, and those hands-on sessions almost always beat plain classroom sessions in making safety stick. It’s not only about knowing the rules—it's about shaping smart habits under stress.
Working with an experienced waste contractor avoids pitfalls. They often offer audits, which spot unsafe storage or documentation slip-ups before regulators show up. Installing simple checklists in waste storage rooms cuts down on overlooked steps. Engineering controls like passively ventilated bins or temperature alarms can further reduce hazards. Some sites use peroxide-specific deactivation chemicals under controlled settings, but these practices demand a well-trained eye and strict adherence to tested protocols.
The safest course lines up respect for the chemical, keen awareness of legal obligations, and a team culture shaped around safety, not shortcuts. This blend leaves no room for luck and builds real protection for people and planet alike.
| Names | |
| Preferred IUPAC name | 2-(1,1-Dimethylethyl)-1,1-dimethylethylbenzene hydroperoxide |
| Other names |
Cumene, α,α-di(1,1-dimethylethyl)hydroperoxide Di-tert-butyl cumene hydroperoxide Cumene hydroperoxide, di-tert-butyl- DTBCH |
| Pronunciation | /daɪ-tɜrt-ˌbjuːtɪl-ˈkjuːmɪl haɪˈdrɒpəˌroʊˌksaɪd/ |
| Identifiers | |
| CAS Number | 124-40-3 |
| 3D model (JSmol) | `C(C)(C)(C)C1=CC(OO)(C(C)(C)C)C=C1` |
| Beilstein Reference | 1638734 |
| ChEBI | CHEBI:88231 |
| ChEMBL | CHEMBL1496982 |
| ChemSpider | 157462 |
| DrugBank | DB14329 |
| ECHA InfoCard | 03c80f17-64c6-4681-83f3-1b9e9126d2ba |
| EC Number | 202-650-3 |
| Gmelin Reference | 142858 |
| KEGG | C14072 |
| MeSH | D005923 |
| PubChem CID | 68597 |
| RTECS number | SAF178500 |
| UNII | 6Z9BV8P3NC |
| UN number | 3115 |
| Properties | |
| Chemical formula | C17H30O2 |
| Molar mass | 262.4 g/mol |
| Appearance | Colorless transparent liquid |
| Odor | No characteristic odor. |
| Density | 0.92 g/mL at 25 °C (lit.) |
| Solubility in water | insoluble |
| log P | 3.6 |
| Vapor pressure | < 0.1 hPa (20 °C) |
| Acidity (pKa) | ~13 |
| Magnetic susceptibility (χ) | -7.7e-6 cm³/mol |
| Refractive index (nD) | 1.501 |
| Viscosity | 15 mPa·s (25 °C) |
| Dipole moment | 3.06 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 497.42 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -551.1 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -1314 kJ/mol |
| Hazards | |
| GHS labelling | GHS02, GHS05, GHS06, GHS08 |
| Pictograms | GHS02,GHS05,GHS06,GHS08 |
| Signal word | Danger |
| Hazard statements | Hazard statements: H242, H302, H314, H332, H335, H411 |
| Precautionary statements | P210, P220, P221, P234, P260, P264, P270, P271, P280, P301+P310, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P308+P311, P311, P312, P321, P330, P337+P313, P363, P370+P378, P403+P235, P405, P501 |
| NFPA 704 (fire diamond) | 3-4-2-W |
| Flash point | 64°C |
| Autoignition temperature | 220 °C |
| Explosive limits | Explosive limits: 1.2 - 7 %(V) |
| Lethal dose or concentration | LD₅₀ Oral Rat: >2000 mg/kg |
| LD50 (median dose) | 307 mg/kg (rat, oral) |
| NIOSH | UN3109 |
| REL (Recommended) | 0.5 ppm |
| Related compounds | |
| Related compounds |
Cumene hydroperoxide tert-Butyl hydroperoxide Di-tert-butyl peroxide Dicumyl peroxide Methyl ethyl ketone peroxide |
