PRODUCTS

CALCIUM OXIDE

Calcium oxide, commonly known as lime, is a chemical compound with the formula CaO.
Calcium oxide, also known as quicklime, is an alkaline substance that has been in use since the medieval age.
Calcium oxide is believed that quicklime is one of the oldest chemicals known to the human race.
Calcium oxide can also be referred to as burnt lime or lime.

CAS Number: 1305-78-8
EC Number: 215-138-9
IUPAC Name: Calcium oxide
Chemical Formula: CaO

Other names: 1305-78-8, oxocalcium, Gebrannter kalk, Calcium monoxide, CALX, Calcium oxide (CaO), Lime [USP], Calcia, Calxyl, Lime (USP), Airlock, Chaux vive, Quick lime, Calx usta, Rhenosorb C, Rhenosorb F, Desical P, Lime, burned, Caloxal CPA, Caloxol W3, Vesta PP, Caloxol CP2, Calcia (CaO), Bell CML(E), Bell CML(P), Caswell No. 147A, Wapniowy tlenek, QC-X, Wapniowy tlenek [Polish], Oxyde de calcium, Oxyde de calcium [French], CCRIS 7496, CML 21, CML 31, CML 35, HSDB 1615, EINECS 215-138-9, UNII-C7X2M0VVNH, UN1910, EPA Pesticide Chemical Code 075604, Branntkalk, Kalziumoxid, Aetzkalk, Calcium oxide, CP, Calcium oxide, 98%, Calcium Oxide Dispersion, Calcium Oxide Nanopowder, Calcium oxide (JP17), EC 215-138-9, Calcium oxide, Reagent Grade, Tin(IV) selenide (SnSe2), Calcium oxide, p.a., 95.0%, AKOS015903966, FC07719, Lime, meets USP testing specifications, Calcium oxide, Vetec(TM) reagent grade, Calcium oxide [UN1910] [Corrosive], Calcium oxide, 99.995% trace metals basis, Calcium oxide, SAJ first grade, >=98.0%, Calcium oxide, SAJ special grade, >=98.0%, D01679, Q185006, Calcium oxide, ReagentPlus(R), 99.9% trace metals basis, Calcium oxide, anhydrous, powder, >=99.99% trace metals basis, Calcium oxide, nanopowder, <160 nm particle size (BET), 98%, Calcium oxide, puriss., meets analytical specification of FCC, 96-100.5% (ex ignited substance), powder (fine)

Calcium oxide has a medium viscosity and a high surface tension, plus a high to intermediate expansion and contraction rate.
This material isn’t volatile at ceramic temperatures.
Calcium oxide has a moderate effect on colour, except in large amounts when it may have a bleaching effect on iron oxide.
Calcium oxide also exists in the colour of kaki/tomato reds.

Preparation of Calcium Oxide
Calcium oxide can be produced by thermal decomposition of materials like limestone or seashells that contain calcium carbonate (CaCO3, mineral calcite) in a lime kiln.
The process that is used to prepare burnt lime is known as calcination.
Calcium oxide is a process that starts with thermally decomposing the reactants at high temperatures but ensuring that the temperature is kept well below the melting point.

Calcium carbonate undergoes calcination at temperatures ranging between 1070oC-1270oC.
These reactions are usually held in a rotary kiln.
The products formed as a result of the reaction are burnt lime and carbon dioxide.
The carbon dioxide that is formed is immediately removed so that the reaction is preceded until the completion of the process in accordance with Le-Chatelier’s principle.
CaCO3 → CaO + CO2

This reaction is reversible and exothermic in nature in the forward direction.

Structure of CaO Molecules
Calcium oxide molecules contain one calcium cation (which holds a charge of +2) and one oxygen anion (which holds a charge of -2).
The structure of calcium oxide is illustrated below.

Thus, it can be understood that calcium oxide is an ionic compound featuring an ionic bond between calcium and oxygen.

Lime Water Formula
The formula for lime water is Ca(OH)2 and the chemical name for lime water is calcium hydroxide.
When water is added to lime calcium hydroxide Ca(OH)2 is formed according to the following reaction.
CaO + H2O → Ca(OH)2

This reaction is strongly exothermic and takes place vigorously with the formation of clouds of steam.

What is the Difference Between Quicklime and Lime Water?
The chemical formula of lime or quicklime is CaO.
The chemical name of lime is calcium oxide.
On the other hand, the chemical formula of limewater is Ca(OH)2 and the chemical name of Calcium oxide is calcium hydroxide.

Properties of Calcium Oxide
Quick lime is an amorphous white solid with a high melting point of 2600°
Calcium oxide is a very stable compound and withstands high temperatures.
In the presence of water, it forms slaked lime.
This process is called the slaking of lime.
CaO+H2O → Ca (OH)2

Calcium oxide is an oxide that is basic in nature and forms salts when it comes in contact with an acid.
This compound crystallizes in a cubic crystal lattice.
The standard molar entropy associated with calcium oxide corresponds to 40 joules per mole kelvin.
This compound is known to emit an intense glow when it is heated to temperatures above 2400 degrees celsius.
CaO+H2SO4 → CaSO4+H2O

Uses of Calcium Oxide
Calcium oxide is extensively used for medicinal purposes and insecticides.
Calcium oxide finds its application in the manufacturing of cement, paper, and high-grade steel.
Lime is used as a reagent in laboratories for dehydration, precipitation reaction, etc.
Calcium oxide is the cheapest alkali available which is an important ingredient in the manufacturing of caustic soda.
Calcium is essential to animal life as the constituent of bones, shells, and teeth.
The most common of the calcium compounds are calcium carbonate which the potter uses as a source of calcium oxide for glazes.

Calcium oxide (CaO), commonly known as quicklime or burnt lime, is a widely used chemical compound.
Calcium oxide is a white, caustic, alkaline, crystalline solid at room temperature.
The broadly used term "lime" connotes calcium-containing inorganic materials, in which carbonates, oxides and hydroxides of calcium, silicon, magnesium, aluminium, and iron predominate.
By contrast, quicklime specifically applies to the single chemical compound calcium oxide.
Calcium oxide that survives processing without reacting in building products such as cement is called free lime.

Quicklime is relatively inexpensive.
Both it and a chemical derivative (calcium hydroxide, of which quicklime is the base anhydride) are important commodity chemicals.

Preparation
Calcium oxide is usually made by the thermal decomposition of materials, such as limestone or seashells, that contain calcium carbonate (CaCO3, mineral calcite) in a lime kiln.
This is accomplished by heating the material to above 825 °C (1,517 °F), a process called calcination or lime-burning, to liberate a molecule of carbon dioxide (CO2), leaving quicklime.
This is also one of the few chemical reactions known in prehistoric times.
CaCO3(s) → CaO(s) + CO2(g)

The quicklime is not stable and, when cooled, will spontaneously react with CO2 from the air until, after enough time, it will be completely converted back to calcium carbonate unless slaked with water to set as lime plaster or lime mortar.

Annual worldwide production of quicklime is around 283 million tonnes.
China is by far the world's largest producer, with a total of around 170 million tonnes per year.
The United States is the next largest, with around 20 million tonnes per year.

Approximately 1.8 t of limestone is required per 1.0 t of quicklime.
Quicklime has a high affinity for water and is a more efficient desiccant than silica gel.
The reaction of quicklime with water is associated with an increase in volume by a factor of at least 2.5.

Uses:
The major use of quicklime is in the basic oxygen steelmaking (BOS) process.
Its usage varies from about 30 to 50 kilograms (65–110 lb) per ton of steel.
The quicklime neutralizes the acidic oxides, SiO2, Al2O3, and Fe2O3, to produce a basic molten slag.
Ground quicklime is used in the production of aerated concrete blocks, with densities of ca. 0.6–1.0 g/cm3 (9.8–16.4 g/cu in).
Quicklime and hydrated lime can considerably increase the load carrying capacity of clay-containing soils.

They do this by reacting with finely divided silica and alumina to produce calcium silicates and aluminates, which possess cementing properties.
Small quantities of quicklime are used in other processes, e.g., the production of glass, calcium aluminate cement, and organic chemicals.
Heat: Quicklime releases thermal energy by the formation of the hydrate, calcium hydroxide, by the following equation:
CaO (s) + H2O (l) ⇌ Ca(OH)2 (aq) (ΔHr = −63.7 kJ/mol of CaO)

As it hydrates, an exothermic reaction results and the solid puffs up.
The hydrate can be reconverted to quicklime by removing the water by heating it to redness to reverse the hydration reaction.
One litre of water combines with approximately 3.1 kilograms (6.8 lb) of quicklime to give calcium hydroxide plus 3.54 MJ of energy.

This process can be used to provide a convenient portable source of heat, as for on-the-spot food warming in a self-heating can, cooking, and heating water without open flames.
Several companies sell cooking kits using this heating method.
Calcium oxide is known as a food additive to the FAO as an acidity regulator, a flour treatment agent and as a leavener.

Light: When quicklime is heated to 2,400 °C (4,350 °F), it emits an intense glow.
This form of illumination is known as a limelight, and was used broadly in theatrical productions before the invention of electric lighting.
Cement: Calcium oxide is a key ingredient for the process of making cement.

As a cheap and widely available alkali. About 50% of the total quicklime production is converted to calcium hydroxide before use.
Both quick- and hydrated lime are used in the treatment of drinking water.

Petroleum industry: Water detection pastes contain a mix of calcium oxide and phenolphthalein.
Should this paste come into contact with water in a fuel storage tank, the CaO reacts with the water to form calcium hydroxide.
Calcium hydroxide has a high enough pH to turn the phenolphthalein a vivid purplish-pink color, thus indicating the presence of water.

Paper: Calcium oxide is used to regenerate sodium hydroxide from sodium carbonate in the chemical recovery at Kraft pulp mills.

Plaster: There is archeological evidence that Pre-Pottery Neolithic B humans used limestone-based plaster for flooring and other uses.
Such Lime-ash floor remained in use until the late nineteenth century.

Chemical or power production: Solid sprays or slurries of calcium oxide can be used to remove sulfur dioxide from exhaust streams in a process called flue-gas desulfurization.

Mining: Compressed lime cartridges exploit the exothermic properties of quicklime to break rock.
A shot hole is drilled into the rock in the usual way and a sealed cartridge of quicklime is placed within and tamped.
A quantity of water is then injected into the cartridge and the resulting release of steam, together with the greater volume of the residual hydrated solid, breaks the rock apart.
The method does not work if the rock is particularly hard.

Disposal of corpses: Historically, it was mistakenly believed that quicklime was efficacious in accelerating the decomposition of corpses.
The application of quicklime can, in fact, promote preservation.
Quicklime can aid in eradicating the stench of decomposition, which may have led people to the erroneous conclusion.

Weapon
In 80 BC, the Roman general Sertorius deployed choking clouds of caustic lime powder to defeat the Characitani of Hispania, who had taken refuge in inaccessible caves.
A similar dust was used in China to quell an armed peasant revolt in 178 AD, when lime chariots equipped with bellows blew limestone powder into the crowds.
Quicklime is also thought to have been a component of Greek fire.
Upon contact with water, quicklime would increase its temperature above 150 °C (302 °F) and ignite the fuel.

David Hume, in his History of England, recounts that early in the reign of Henry III, the English Navy destroyed an invading French fleet by blinding the enemy fleet with quicklime.
Quicklime may have been used in medieval naval warfare – up to the use of "lime-mortars" to throw it at the enemy ships.

Substitutes
Limestone is a substitute for lime in many applications, which include agriculture, fluxing, and sulfur removal.
Limestone, which contains less reactive material, is slower to react and may have other disadvantages compared with lime, depending on the application, however, limestone is considerably less expensive than lime.
Calcined gypsum is an alternative material in industrial plasters and mortars.
Cement, cement kiln dust, fly ash, and lime kiln dust are potential substitutes for some construction uses of lime.
Magnesium hydroxide is a substitute for lime in pH control, and magnesium oxide is a substitute for dolomitic lime as a flux in steelmaking.

Physical Description HelpNew Window
Calcium oxide appears as an odorless, white or gray-white solid in the form of hard lumps.
A strong irritant to skin, eyes and mucous membranes. Used in insecticides and fertilizers.

Calcium oxide appears as an odorless, white or gray-white solid in the form of hard lumps.
A strong irritant to skin, eyes and mucous membranes. Used in insecticides and fertilizers.

Uses:
In construction applications incl finishing & masons lime, in metallurgy, principally as a flux in steel prodn, kraft paper pulp prodn, ammonia recovery in solvay process for sodium carbonate, treatment of sewage and trade waste, water purification and softening, misc applications
In bricks, plaster, mortar, stucco, building materials, manufacture of steel, aluminum, magnesium, and flotation of non-ferrous ores, manufacture of glass, paper, Na2CO3 (Solvay process), calcium salts and many other industrial chemicals, dehairing hides, clarification of cane and beet sugar juices, in fungicides, insecticides, drilling fluids, lubricants, in water and sewage treatment, in laboratory to absorb carbon dioxide (the combination with NaOH is known as soda-lime ...)

Industry Uses
Abrasives
Adhesives and sealant chemicals
Adsorbents and absorbents
Calcium oxide (CaO) used in the pulp manufacturing
Catalyst

Cement
Chemical is part of scrap metal/iron kish used in the manufacture of metal in an electric arc furnace.
Corrosion inhibitors and anti-scaling agents
Desiccant
Engineered fill for construction
Fillers

Graveling and road bed material.
Intermediates
Ion exchange agents
Lubricants and lubricant additives
Oxidizing/reducing agents

Paint additives and coating additives not described by other categories
Pigments
Process regulators
Processing aids, not otherwise listed
Raw Material Constituent

Reactant
Refractories
Refractory Materials
Regenerated white liquor from green liquor
Smelter feedstock production

Used by others in land application.
Used on-site for Calcium Hydroxide Production
Water treatment.
other industrial function
soil stabilization
sorbent for capture of sulfur dioxide in boiler

Consumer Uses
Abrasives
Adhesives and sealants
Air care products
Building/construction materials not covered elsewhere

Catalyst
Fuels and related products
High temperature refractories for furnace linings.
Metal products not covered elsewhere
Non-TSCA use

Paints and coatings
Paper products
Plastic and rubber products not covered elsewhere
Recycled material
Water treatment products
oxygen concentrators

General Manufacturing Information
Industry Processing Sectors
Adhesive manufacturing
Adhesives and Sealants.
Agriculture, forestry, fishing and hunting

All other basic inorganic chemical manufacturing
All other basic organic chemical manufacturing
All other chemical product and preparation manufacturing
All other petroleum and coal products manufacturing
Asphalt paving, roofing, and coating materials manufacturing

Construction
Food, beverage, and tobacco product manufacturing
Industrial gas manufacturing
Mining (except oil and gas) and support activities
Miscellaneous manufacturing

Nonmetallic mineral product manufacturing (includes clay, glass, cement, concrete, lime, gypsum, and other nonmetallic mineral product manufacturing.
Oil and gas drilling, extraction, and support activities
Paint and coating manufacturing
Paper manufacturing

Petrochemical manufacturing
Petroleum refineries
Pharmaceutical and medicine manufacturing
Primary metal manufacturing
Rubber product manufacturing

Services
Synthetic dye and pigment manufacturing
Synthetic rubber manufacturing
Utilities
Wholesale and retail trade

Chemical properties
Calcium oxide appears as white cubic crystalline powder.
Industrial products often contain magnesia, alumina and ferric oxide and other impurities so exhibit dark gray, light yellow or brown.
Calcium oxide is soluble in acid.

Uses:
Calcium oxide can be used in the manufacture of calcium carbide, soda ash, bleaching powder, used as building materials, refractoriness’, desiccant and soil conditioner and calcium fertilizer
Calcium oxide can be used as an analysis reagent and flux agent for manufacturing fluorescence powder.
Calcium oxide can be used in the manufacture of calcium carbide, soda ash, bleaching powder, also used for leather, waste water purification

Calcium oxide can be used as building materials, metallurgical flux agent and the major raw materials for the manufacturing of calcium hydroxide and a variety of calcium compounds.
Calcium oxide is also the inexpensive alkali in the chemical industry.
Calcium oxide is widely used in pesticides, paper, food, petrochemical, leather, waste water purification and so on.
Calcium oxide can also be used for the drying of the laboratory ammonia and alcohol dehydration.
Use as drug carriers.
Uses as analysis reagents; Calcium oxide can be applied to steel, pesticides, pharmaceuticals, non-ferrous metals, fertilizers, leather and manufacturing of calcium hydroxide, drying of laboratory ammonia, carbon dioxide absorbent and alcohol dehydration.

Calcium oxide is also known as lime, quick lime, burnt lime, or calx. Lime does not occur naturally since it reacts so readily with water (to form hydrated lime) and carbon dioxide (to form limestone).
Calcium oxide is produced from calcium carbonate, limestone, or oyster shells by calcination at temperatures of 1,700-2,450℃.
Calcium Oxide is a solid with a very high affinity for water - it will react with water in the air, or in your skin or anywhere it can and form calcium hydroxide.

This reaction is exothermic so it releases a lot of heat while it is reacting - there fore as well as being corrosive and causing significant skin irritation, calcium oxide's reaction with water can also cause burns. Calcium hydroxide is basically hydrated calcium oxide.
Calcium oxide is alkali so can be corrosive.
In solution it makes limewater.
CaO is not found pure in nature but rather is contained in various abundant minerals (i.e. calcite, aragonite, limestone, marble) but vary greatly in their purity (impurities usually include magnesia, iron, alumina, silica, sulfur).

Of these iron and sulfur are most troublesome (i.e. where clarity is important in glass).
Lime minerals vary in the degree of crystallization and cohesion of the crystalline mass and the homogeneity of the matrix.
Calcium oxide is the principle flux in medium and high temperature glazes, beginning its action (within the glaze) around 1100C.
Calcium oxide must be used with care in high-fire bodies because its active fluxing action can produce a body that is too volatile (melting if slightly overfired).

Lime, or calcium oxide, is a principle ingredient in the production of Portland cement, the basis for most mortars and concrete. Hydrated or ‘slaked’ lime is the chemical calcium hydroxide.
This chemical is also used in mortars.
Both types of lime are strong bases and are also used in food production (calcium hydroxide is commonly used in making corn tortillas), petroleum refining and sewage treatment.
In the household it is used by aquarium hobbyists to add bioavailable calcium to fish tanks.
Calcium oxide is also found in hair relaxers.

Chemical Properties
Calcium oxide, CaO, occurs as white or grayish-white lumps or granular powder.
The presence of iron gives it a yellowish or brownish tint.

Physical properties
Calcium oxide is a white caustic crystalline alkali substance that goes by the common name lime.
The term lime is used both generically for several calcium compounds and with adjectives to qualify different forms of lime. This entry equates lime, also called quicklime or burnt lime, with the compound calcium oxide.

Hydrated lime, made by combining lime with water, is calcium hydroxide and is often referred to as slaked lime (Ca(OH)2). Dolomite limes contain magnesium as well as calcium.
Limestone is the compound calcium carbonate.
The term lime comes from the Old English word for a sticky substance and denotes lime’s traditional use to produce mortar.
Calx was the Latin word for lime and was used to name the element calcium.

Uses
The major uses of lime are metallurgy, flue gas desulfurization, construction, mining, papermaking, and water treatment.
About one third of calcium oxide production in the United States is used for metallurgical processes, principally in the iron and steel industry.
Calcium oxide is used to remove impurities during the refining of iron ore.

Calcium oxide combines with compounds such as silicates, phosphates, and sulfates contained in iron ores to form slag.
Lime is also used for purification in other metal refining and to control pH in mining processes such as leaching and precipitation.
The calcium oxide is also used in remediation of mine wastes to recover cyanides and to neutralize acid mine drainage.

In bricks, plaster, mortar, stucco and other building and construction materials, manufacture of steel, aluminum, magnesium, and flotation of non-ferrous ores, manufacture of glass, paper, Na2CO3 (Solvay process), Ca salts and many other industrial chemicals; dehairing hides, clarification of cane and beet sugar juices, in fungicides, insecticides, drilling fluids, lubricants; water and sewage treatment, in laboratory to absorb CO2 (the combination with NaOH is known as soda-lime, q.v.).

Calcium Oxide is a general food additive consisting of white granules or powder of poor water solubility. it is obtained by heating limestone (calcium carbonate) in a furnace.
Calcium oxide is also termed lime or quicklime.
Calcium oxide is used as an anticaking agent, firming agent, and nutritive supple- ment in applications such as grain products and soft candy.

Agricultural Uses
Calcium oxide (CaO) is a white powder with a neutralizing value or calcium carbonate equivalent (CCE) of 179%, compared to 100% for calcium carbonate (CaCO3).
For quick results, either calcium oxide or calcium hydroxide [Ca(OH)2] is used.
Calcium oxide is also known as lime, unslaked lime, burned lime or quicklime.
Roasting CaCO3 in a furnace makes calcium oxide.
A complete mixing of calcium oxide with soil is difficult because it cakes due to absorption of water.

Industrial uses
Lime is the most widely used reagent in the mineral industry for flotation of sulfides and, in some cases, non-sulfide minerals.
The word “lime” is a general term used to describe any kind of calcareous material or finely divided form of limestone and dolomite.
In more strict chemical terms, lime is calcinated limestone known as calcium oxide (CaO), quicklime or unslaked lime.

The slaked or hydrated lime Ca(OH)2 is the form of lime primarily used in mineral flotation.
Production of high-calcium lime is based on calcination of limestone at a temperature of 1100–1300 °C in kilns.
CaCO3+heat--->CaO+CO2 For high-magnesium (dolomitic) limestone, the calcination reaction (at 1000–1200 °C) is CaCO3·MgCO3 (limestone) + heat--->CaOMgO (quicklime-2CO2)

Calcium oxide is registered under the REACH Regulation and is manufactured in and / or imported to the European Economic Area, at ≥ 10 000 000 tonnes per annum.
Calcium oxide is used by consumers, in articles, by professional workers (widespread uses), in formulation or re-packing, at industrial sites and in manufacturing.

Biocidal Uses
Calcium oxide is approved for use as a biocide in the EEA and/or Switzerland, for: disinfection, veterinary hygiene.

Consumer Uses
Calcium oxide is used in the following products: pH regulators and water treatment products, adsorbents, water treatment chemicals, fertilisers, cosmetics and personal care products, coating products and fillers, putties, plasters, modelling clay.
Other release to the environment of Calcium oxide is likely to occur from: indoor use (e.g. machine wash liquids/detergents, automotive care products, paints and coating or adhesives, fragrances and air fresheners) and outdoor use.

Release to the environment of Calcium oxide can occur from industrial use: formulation of mixtures, industrial abrasion processing with low release rate (e.g. cutting of textile, cutting, machining or grinding of metal) and industrial abrasion processing with high release rate (e.g. sanding operations or paint stripping by shot-blasting). Other release to the environment of Calcium oxide is likely to occur from: outdoor use, indoor use (e.g. machine wash liquids/detergents, automotive care products, paints and coating or adhesives, fragrances and air fresheners), outdoor use in long-life materials with low release rate (e.g. metal, wooden and plastic construction and building materials) and indoor use in long-life materials with low release rate (e.g. flooring, furniture, toys, construction materials, curtains, foot-wear, leather products, paper and cardboard products, electronic equipment).

Calcium oxide can be found in complex articles, with no release intended: vehicles, electrical batteries and accumulators and machinery, mechanical appliances and electrical/electronic products (e.g. computers, cameras, lamps, refrigerators, washing machines). Calcium oxide can be found in products with material based on: stone, plaster, cement, glass or ceramic (e.g. dishes, pots/pans, food storage containers, construction and isolation material), plastic (e.g. food packaging and storage, toys, mobile phones), metal (e.g. cutlery, pots, toys, jewellery), paper (e.g. tissues, feminine hygiene products, nappies, books, magazines, wallpaper), fabrics, textiles and apparel (e.g. clothing, mattress, curtains or carpets, textile toys), leather (e.g. gloves, shoes, purses, furniture), rubber (e.g. tyres, shoes, toys) and wood (e.g. floors, furniture, toys).

Widespread uses by professional workers
ECHA has no public registered data indicating whether or in which chemical products the substance might be used. Calcium oxide is used in the following areas: agriculture, forestry and fishing, building & construction work, municipal supply (e.g. electricity, steam, gas, water) and sewage treatment, printing and recorded media reproduction, health services, scientific research and development and formulation of mixtures and/or re-packaging.
Calcium oxide is used for the manufacture of: plastic products, mineral products (e.g. plasters, cement), machinery and vehicles, textile, leather or fur, wood and wood products, pulp, paper and paper products, rubber products, electrical, electronic and optical equipment and furniture.

Release to the environment of Calcium oxide can occur from industrial use: formulation of mixtures.
Other release to the environment of Calcium oxide is likely to occur from: indoor use (e.g. machine wash liquids/detergents, automotive care products, paints and coating or adhesives, fragrances and air fresheners) and outdoor use.

Release to the environment of Calcium oxide can occur from industrial use: formulation of mixtures, formulation in materials, manufacturing of the substance, in processing aids at industrial sites, as an intermediate step in further manufacturing of another substance (use of intermediates), as processing aid, as processing aid, industrial abrasion processing with low release rate (e.g. cutting of textile, cutting, machining or grinding of metal), in the production of articles, for thermoplastic manufacture, industrial abrasion processing with high release rate (e.g. sanding operations or paint stripping by shot-blasting) and of substances in closed systems with minimal release.

Other release to the environment of Calcium oxide is likely to occur from: outdoor use in long-life materials with low release rate (e.g. metal, wooden and plastic construction and building materials), indoor use in long-life materials with low release rate (e.g. flooring, furniture, toys, construction materials, curtains, foot-wear, leather products, paper and cardboard products, electronic equipment), outdoor use in long-life materials with high release rate (e.g. tyres, treated wooden products, treated textile and fabric, brake pads in trucks or cars, sanding of buildings (bridges, facades) or vehicles (ships)) and indoor use in long-life materials with high release rate (e.g. release from fabrics, textiles during washing, removal of indoor paints).

Uses at industry
Calcium oxide is used in the following areas: mining.
Calcium oxide is used for the manufacture of: chemicals.
Release to the environment of Calcium oxide can occur from industrial use: in processing aids at industrial sites, as an intermediate step in further manufacturing of another substance (use of intermediates), as processing aid, as processing aid, in the production of articles, for thermoplastic manufacture, of substances in closed systems with minimal release, manufacturing of the substance, formulation of mixtures, formulation in materials, industrial abrasion processing with low release rate (e.g. cutting of textile, cutting, machining or grinding of metal) and industrial abrasion processing with high release rate (e.g. sanding operations or paint stripping by shot-blasting).

Manufacture
Release to the environment of Calcium oxide can occur from industrial use: manufacturing of the substance, formulation of mixtures, formulation in materials, in processing aids at industrial sites, in the production of articles, as an intermediate step in further manufacturing of another substance (use of intermediates), as processing aid, for thermoplastic manufacture, as processing aid, industrial abrasion processing with low release rate (e.g. cutting of textile, cutting, machining or grinding of metal), industrial abrasion processing with high release rate (e.g. sanding operations or paint stripping by shot-blasting) and of substances in closed systems with minimal release.