Difference between revisions of "Calcium oxide"
Jump to navigation
Jump to search
| (One intermediate revision by the same user not shown) | |||
| Line 14: | Line 14: | ||
== Physical and Chemical Properties == | == Physical and Chemical Properties == | ||
| − | Soluble in acid. Hygroscopic. Reacts with water to form calcium hydroxide with evolution of heat. | + | * Soluble in acid. |
| + | * Hygroscopic. | ||
| + | * Reacts with water to form calcium hydroxide with evolution of heat. | ||
{| class="wikitable" | {| class="wikitable" | ||
| Line 38: | Line 40: | ||
== Resources and Citations== | == Resources and Citations== | ||
| − | + | * Wikipedia: [https://en.wikipedia.org/wiki/Calcium_oxide Calcium oxide] Accessed July 2023 | |
* Richard S. Lewis, ''Hawley's Condensed Chemical Dictionary'', Van Nostrand Reinhold, New York, 10th ed., 1993 | * Richard S. Lewis, ''Hawley's Condensed Chemical Dictionary'', Van Nostrand Reinhold, New York, 10th ed., 1993 | ||
| − | |||
* Henry Hodges, ''Artifacts: An Introduction to Early Materials and Technology'', Ronald P. Frye, Kingston, Canada, 1988 | * Henry Hodges, ''Artifacts: An Introduction to Early Materials and Technology'', Ronald P. Frye, Kingston, Canada, 1988 | ||
| − | |||
* Random House, ''Webster's Encyclopedic Unabridged Dictionary of the English Language'', Grammercy Book, New York, 1997 | * Random House, ''Webster's Encyclopedic Unabridged Dictionary of the English Language'', Grammercy Book, New York, 1997 | ||
| − | |||
* ''The Merck Index'', Martha Windholz (ed.), Merck Research Labs, Rahway NJ, 10th edition, 1983 Comment: entry 1733 | * ''The Merck Index'', Martha Windholz (ed.), Merck Research Labs, Rahway NJ, 10th edition, 1983 Comment: entry 1733 | ||
Latest revision as of 13:02, 14 July 2023
Description
White, alkaline lumps obtained from the thermal decomposition of Limestone or seashells. Calcium oxide is a refractory solid that becomes incandescent at temperatures near its melting point (2500C). In 1816, prior to the development of electrical lights, calcium oxide was used for bright white illumination, called limelights. Calcium oxide is primarily used in the manufacture of slaked limes for mortar, plasters, and cements. It is also used as a refractory and flux in manufacturing Steel and Glass. Calcium oxide is added to Paper pulp for pH control and phosphate removal. The inexpensive, hygroscopic material is added to petroleum for water removal.
Synonyms and Related Terms
lime; quicklime; burnt lime; calx; unslaked lime; fluxing lime
Risks
- Skin contact causes irritation and burns.
- Fire risk in contact with organic materials.
- Fisher Scientific: SDS
Physical and Chemical Properties
- Soluble in acid.
- Hygroscopic.
- Reacts with water to form calcium hydroxide with evolution of heat.
| Composition | CaO |
|---|---|
| CAS | 1305-78-8 |
| Melting Point | 2570 C |
| Density | 3.40 g/ml |
| Molecular Weight | mol. wt. = 56.1 |
| Boiling Point | 2850 C |
Resources and Citations
- Wikipedia: Calcium oxide Accessed July 2023
- Richard S. Lewis, Hawley's Condensed Chemical Dictionary, Van Nostrand Reinhold, New York, 10th ed., 1993
- Henry Hodges, Artifacts: An Introduction to Early Materials and Technology, Ronald P. Frye, Kingston, Canada, 1988
- Random House, Webster's Encyclopedic Unabridged Dictionary of the English Language, Grammercy Book, New York, 1997
- The Merck Index, Martha Windholz (ed.), Merck Research Labs, Rahway NJ, 10th edition, 1983 Comment: entry 1733