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Making of Barium oxide

• Definition •Processes •Preparation •Properties •Disadvantages •Uses/Application •Health Hazard •Fire Hazard Gonzaga, Gift Onah Zoe D. Making of Barium oxide.

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Making of Barium oxide

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  1. • Definition •Processes •Preparation •Properties •Disadvantages •Uses/Application •Health Hazard •Fire Hazard Gonzaga, Gift Onah Zoe D. Making of Barium oxide

  2. Is a white hygroscopiccompound formed by the burning of barium in oxygen, although it is often formed through the decomposition of other barium salts. • Processes 2Ba + O2 → 2BaO BaCO3 → BaO + CO2 BARIUM OXIDE

  3. Barium oxide is made by heating barium carbonate with coke, carbon black or tar. It may also be prepared by thermal decomposition ofbarium nitrate. Coke is a fuel with few impurities and a high carbon content, usually made from coal. It is the solid carbonaceous material derived fromdestructive distillation of low-ash, low-sulfur bituminous coal. Cokes made from coal are grey, hard, and porous. While coke can be formed naturally, the commonly used form is man-made. The form known aspetroleum coke, or pet coke, is derived from oil refinery coker units or other cracking processes. Preparation

  4. Molecular formula: BaO Molar mass: 153.326 g/mol Appearance: white solid Density: 5.72 g/cm3, solid Melting point: 1923 °C Boiling point: ~2000 °C Solubility inwater: 3.48 g/100 mL (20 °C)90.8 g/100 mL (100 °C) Solubility: soluble in ethanol, dilute mineral acids and alkalies insoluble in acetone and liquid ammonia Chemical Properties: white to cream powder Properties

  5. Barium oxide is an irritant. If it contacts the skin or the eyes or is inhaled it causes pain and redness. However, it is more dangerous when ingested. It can causenausea and diarrhea, muscle paralysis, cardiac arrhythmia, and can cause death. If ingested, medical attention should be sought immediately. Barium oxide should not be released environmentally; it is harmful to aquatic organisms. Disadvantages

  6. Used as a drying agent for gasoline and solvents. Barium oxide is used as a coating for hot cathodes, for example, those in cathode ray tubes. It replaced lead(II) oxide in the production of certain kinds of glass such as optical crown glass. While lead oxide raised the refractive index, it also raised the dispersive power, which barium oxide does not alter.[5] Barium oxide also has use as an ethoxylationcatalyst in the reaction of ethylene oxide and alcohols, which takes place between 150 and 200°C. Uses\Application

  7. Cathode ray tube Crown glass (optics) Images of Applications

  8. TOXIC; inhalation, ingestion or contact (skin, eyes) with vapors, dusts or substance may cause severe injury, burns or death. Reaction with water or moist air will release toxic, corrosive or flammable gases. Reaction with water may generate much heat that will increase the concentration of fumes in the air. Fire will produce irritating, corrosive and/or toxic gases. Runoff from fire control or dilution water may be corrosive and/or toxic and cause pollution. HEALTH HAZARD

  9. Non-combustible, substance itself does not burn but may decompose upon heating to produce corrosive and/or toxic fumes. Vapors may accumulate in confined areas (basement, tanks, hopper/tank cars etc.). Substance will react with water (some violently), releasing corrosive and/or toxic gases and runoff. Contact with metals may evolve flammable hydrogen gas. Containers may explode when heated or if contaminated with water. FIRE HAZARD

  10. Barium Oxide

  11. http://en.wikipedia.org/wiki/Barium_oxide ^Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. ISBN0-618-94690-X. Jump up^Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. ISBN0-618-94690-X. Jump up^"Compounds of barium: barium (II) oxide". Web Elements. The University of Sheffield. 2007-01-26. Retrieved 2007-02-22. Jump up^ S.C. Middleburgh, K.P.D. Lagerlof, R.W. Grimes - Accommodation of Excess Oxygen in Group II Oxides http://onlinelibrary.wiley.com/doi/10.1111/j.1551-2916.2012.05452.x/pdf Jump up^"Barium Oxide (chemical compound)". EncyclopædiaBritanica. EncyclopædiaBritanica. 2007. Retrieved 2007-02-19. Jump up^Nield, Gerald; Washecheck, Paul; Yang, Kang (05-04). "United States Patent 4210764". Retrieved 2007-02-20. Jump up^PradyotPatnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8 Jump up^"Barium Oxide (ICSC)". IPCS. October 1999. Archived from the original on 26 February 2007. Retrieved 2007-02-19. References

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