Calcium silicate: Difference between revisions
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'''Calcium silicate''' is the [[chemical compound]] Ca<sub>2</sub>SiO<sub>4</sub>, also known as calcium [[orthosilicate]] and is sometimes formulated as 2CaO·SiO<sub> |
'''Calcium silicate''' is the [[chemical compound]] Ca<sub>2</sub>SiO<sub>4</sub>, also known as calcium [[orthosilicate]] and is sometimes formulated as 2CaO·SiO<sub>2</sub>. It is also referred to by the shortened trade name Cal-Sil or Calsil. It occurs naturally as the mineral [[larnite]]. |
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==Properties== |
==Properties== |
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Revision as of 17:54, 17 August 2021
 | This article needs additional citations for verification. (July 2017) |
| Names | |
|---|---|
| Preferred IUPAC name
Calcium silicate | |
| Systematic IUPAC name
Dicalcium silicate | |
| Other names
Belite
Calcium monosilicate | |
| Identifiers | |
| |
3D model (JSmol)
|
|
| ChemSpider | |
| ECHA InfoCard | 100.014.282 |
| EC Number |
|
| E number | E552 (acidity regulators, ...) |
| KEGG | |
| MeSH | Calcium+silicate |
PubChem CID
|
|
| UNII |
|
CompTox Dashboard (EPA)
|
|
| |
| |
| Properties | |
| Ca2O4Si | |
| Molar mass | 172.237 g·mol−1 |
| Appearance | White crystals |
| Density | 2.9 g/cm3 (solid)[1] |
| Melting point | 2,130[2] °C (3,870 °F; 2,400 K) |
| 0.01% (20 °C)[1] | |
| Thermochemistry | |
Std molar
entropy (S⦵298) |
84 J/(mol·K)[3] |
Std enthalpy of
formation (ΔfH⦵298) |
−1630 kJ/mol[3] |
| Pharmacology | |
| A02AC02 (WHO) | |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards
|
Irritant |
| NFPA 704 (fire diamond) | |
| Flash point | Not applicable |
| NIOSH (US health exposure limits): | |
PEL (Permissible)
|
TWA 15 mg/m3 (total) TWA 5 mg/m3 (resp)[1] |
REL (Recommended)
|
TWA 10 mg/m3 (total) TWA 5 mg/m3 (resp)[1] |
IDLH (Immediate danger)
|
N.D.[1] |
| Safety data sheet (SDS) | [4] |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
| |
Calcium silicate is the chemical compound Ca2SiO4, also known as calcium orthosilicate and is sometimes formulated as 2CaO·SiO2. It is also referred to by the shortened trade name Cal-Sil or Calsil. It occurs naturally as the mineral larnite.
Properties
Calcium silicate is a white free-flowing powder. It can be derived from naturally occurring limestone and diatomaceous earth, a siliceous sedimentary rock.[citation needed] It is one of a group of compounds that can be produced by reacting calcium oxide and silica in various ratios[5] e.g. 3CaO·SiO2, Ca3SiO5; 2CaO·SiO2, Ca2SiO4; 3CaO·2SiO2, Ca3Si2O7 and CaO·SiO2, CaSiO3. It has a low bulk density and high physical water absorption.[citation needed]
Use
Calcium silicate is used as an anticaking agent in food preparation, including table salt[6] and as an antacid. It is approved by the United Nations' FAO and WHO bodies as a safe food additive in a large variety of products.[7] It has the E number reference E552.
High-temperature insulation
Calcium silicate is commonly used as a safe alternative to asbestos for high-temperature insulation materials. Industrial-grade piping and equipment insulation is often fabricated from calcium silicate. Its fabrication is a routine part of the curriculum for insulation apprentices. Calcium silicate competes in these realms against rockwool and proprietary insulation solids, such as perlite mixture and vermiculite bonded with sodium silicate. Although it is popularly considered an asbestos substitute, early uses of calcium silicate for insulation still made use of asbestos fibers.
Passive fire protection
It is used in passive fire protection and fireproofing as calcium silicate brick or in roof tiles. It is one of the most successful materials in fireproofing in Europe because of regulations and fire safety guidelines for commercial and residential building codes. Where North Americans use spray fireproofing plasters, Europeans are more likely to use cladding made of calcium silicate. [why?] High-performance calcium-silicate boards retain their excellent dimensional stability even in damp and humid conditions and can be installed at an early stage in the construction program, before wet trades are completed and the building is weather-tight. For sub-standard products, silicone-treated sheets are available to fabricators to mitigate potential harm from high humidity or general presence of water. Fabricators and installers of calcium silicate in passive fire protection often also install firestops.[citation needed]
While the best possible reaction to fire classifications are A1 (construction applications) and A1Fl (flooring applications) respectively, both of which mean "non-combustible" according to EN 13501-1: 2007, as classified by a notified laboratory in Europe, some calcium-silicate boards only come with fire classification of A2 (limited combustibility) or even lower classifications (or no classification), if they are tested at all.[citation needed]
Acid mine drainage remediation
Calcium silicate, also known as slag, is produced when molten iron is made from iron ore, silicon dioxide and calcium carbonate in a blast furnace. When this material is processed into a highly refined, re-purposed calcium silicate aggregate, it is used in the remediation of acid mine drainage (AMD) on active and passive mine sites.[8] Calcium silicate neutralizes active acidity in AMD systems by removing free hydrogen ions from the bulk solution, thereby increasing pH. As its silicate anion captures H+ ions (raising the pH), it forms monosilicic acid (H4SiO4), a neutral solute. Monosilicic acid remains in the bulk solution to play other important roles in correcting the adverse effects of acidic conditions. As opposed to limestone (a popular remediation material),[9] calcium silicate effectively precipitates heavy metals and does not armor over, prolonging its effectiveness in AMD systems.[8][10]
As a product of sealants
It is used as a sealant in roads or on the shells of fresh eggs: when sodium silicate is applied as a sealant to cured concrete or egg shells, it chemically reacts with calcium hydroxide or calcium carbonate to form calcium silicate hydrate, sealing micropores with a relatively impermeable material.[11][12]
As a component of cement
It also occurs in cements, where it is known as belite or in cement chemist notation C2S.[13]
Agriculture
Calcium silicate is often used in agriculture as a plant available source of silicon. It is "applied extensively to Everglades mucks and associated sands planted to sugarcane and rice" [14]
See also
References
- ^ a b c d e NIOSH Pocket Guide to Chemical Hazards. "#0094". National Institute for Occupational Safety and Health (NIOSH).
- ^ R. B. Heimann, Classic and Advanced Ceramics: From Fundamentals to Applications, Wiley, 2010 ISBN 352763018X
- ^ a b Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A21. ISBN 978-0-618-94690-7.
- ^ "SDS Sheet Library". BNZ Materials. Archived from the original on 2012-03-04. Retrieved 2017-07-19.
- ^ H. F. W. Taylor, Cement Chemistry, Academic Press, 1990, ISBN 0-12-683900-X, p. 33–34.
- ^ [1] Archived 2008-12-25 at the Wayback Machine
- ^ "Food Additive Details: Calcium silicate". Archived from the original on June 5, 2012. Retrieved July 28, 2013. Codex General Standard for Food Additives (GSFA) Online Database, FAO/WHO Food Standards Codex alimentarius, published by the Food and Agricultural Organization of the United Nations / World Health Organization, 2013.
- ^ a b Ziemkiewicz, Paul. "The Use of Steel Slag in Acid Mine Drainage Treatment and Control". Wvmdtaskforce.com. Archived from the original on 20 July 2011. Retrieved 25 April 2011.
- ^ Skousen, Jeff. "Chemicals". Overview of Acid Mine Drainage Treatment with Chemicals. West Virginia University Extension Service. Archived from the original on 24 May 2011. Retrieved 29 March 2011.
- ^ Hammarstrom, Jane M.; Philip L. Sibrell; Harvey E. Belkin. "Characterization of limestone reacted with acid-mine drainage" (PDF). Applied Geochemistry (18): 1710–1714. Archived from the original (PDF) on 5 June 2013. Retrieved 30 March 2011.
- ^ Giannaros, P.; Kanellopoulos, A.; Al-Tabbaa, A. (2016). "Sealing of cracks in cement using microencapsulated sodium silicate". Smart Materials and Structures. 25 (8): 8. Bibcode:2016SMaS...25h4005G. doi:10.1088/0964-1726/25/8/084005.
- ^ Passmore, S. M. (1975). "Preserving eggs". Nutrition & Food Science. 75 (4): 2–4. doi:10.1108/eb058634.
- ^ Dovál, M., Palou, M. & Mojumdar, S.C. J Therm Anal Calorim (2006) 86: 595. https://doi.org/10.1007/s10973-006-7713-0
- ^ Gascho, Gary J. (2001). "Chapter 12 Silicon sources for agriculture". Studies in Plant Science. 8 (8): 197–207. doi:10.1016/S0928-3420(01)80016-1. ISBN 9780444502629.