Oxygen not included lime
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This type of preservation conserves high levels of detail, even down to the microscopic level. Most of the vertebrate fossils of the Two Medicine Formation-a geologic formation known for its duck-billed dinosaur eggs-are preserved by CaCO 3 permineralization. The carbonate compensation depth can range from 4,000 to 6,000 meters below sea level.Ĭalcium carbonate can preserve fossils through permineralization. Increasing pressure also increases the solubility of calcium carbonate. Calcium carbonate is unusual in that its solubility increases with decreasing temperature. Deep in the ocean, the temperature drops and pressure increases.
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The carbonate compensation depth (CCD) is the point in the ocean where the rate of precipitation of calcium carbonate is balanced by the rate of dissolution due to the conditions present. Under these conditions calcium carbonate decomposes to produce carbon dioxide which, along with other gases, give rise to explosive volcanic eruptions. Where the oceanic crust is subducted under a continental plate sediments will be carried down to warmer zones in the asthenosphere and lithosphere. The calcification processes are changed by ocean acidification.
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Cold-water carbonates do exist at higher latitudes but have a very slow growth rate. Calcium carbonate contributors, including plankton (such as coccoliths and planktic foraminifera), coralline algae, sponges, brachiopods, echinoderms, bryozoa and mollusks, are typically found in shallow water environments where sunlight and filterable food are more abundant. In warm, clear tropical waters corals are more abundant than towards the poles where the waters are cold. The carbonate minerals form the rock types: limestone, chalk, marble, travertine, tufa, and others. Calcium carbonate occurs as aragonite, calcite and dolomite as significant constituents of the calcium cycle. Surface precipitation of CaCO3 as tufa in Rubaksa, EthiopiaĬarbonate is found frequently in geologic settings and constitutes an enormous carbon reservoir. Magnesium carbonate (MgCO 3) has the calcite structure, whereas strontium carbonate and barium carbonate (SrCO 3 and BaCO 3) adopt the aragonite structure, reflecting their larger ionic radii. The vaterite structure is not fully understood. Calcite contains calcium atoms coordinated by six oxygen atoms in aragonite they are coordinated by nine oxygen atoms. The aragonite form can be prepared by precipitation at temperatures above 85 ☌ the vaterite form can be prepared by precipitation at 60 ☌. Other forms can be prepared, the denser (2.83 g/cm 3) orthorhombic λ-CaCO 3 (the mineral aragonite) and hexagonal μ-CaCO 3, occurring as the mineral vaterite. The thermodynamically stable form of CaCO 3 under normal conditions is hexagonal β-CaCO 3 (the mineral calcite). Water is added to give calcium hydroxide then carbon dioxide is passed through this solution to precipitate the desired calcium carbonate, referred to in the industry as precipitated calcium carbonate (PCC): CaO + H 2O → Ca(OH) 2 Ca(OH) 2 + CO 2 → CaCO 3↓ + H 2O Structure Pure calcium carbonate (such as for food or pharmaceutical use), can be produced from a pure quarried source (usually marble).Īlternatively, calcium carbonate is prepared from calcium oxide. The vast majority of calcium carbonate used in industry is extracted by mining or quarrying. This reaction is important in the erosion of carbonate rock, forming caverns, and leads to hard water in many regions.Īn unusual form of calcium carbonate is the hexahydrate, ikaite, CaCO 3♶H 2O. releases carbon dioxide upon heating, called a thermal decomposition reaction, or calcination (to above 840 ☌ in the case of CaCO 3), to form calcium oxide, commonly called quicklime, with reaction enthalpy 178 kJ/mol:Ĭalcium carbonate reacts with water that is saturated with carbon dioxide to form the soluble calcium bicarbonate.ĬaCO 3( s) + CO 2( g) + H 2O( l) → Ca(HCO 3) 2( aq).reacts with acids, releasing carbon dioxide (technically speaking, carbonic acid, but that disintegrates quickly to CO 2 and H 2O):ĬaCO 3( s) + 2 H +( aq) → Ca 2+( aq) + CO 2( g) + H 2O( l).8.3 Solubility in a strong or weak acid solutionĬalcium carbonate shares the typical properties of other carbonates.8.2 With varying pH, temperature and salinity: CaCO 3 scaling in swimming pools.