Carbide Lamp

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Vintage Carbide Coal Miners HAT Brass Lamp Lantern Butterfly Trademark
$25.00
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VERY SMALL 3 1 2 JUST RITE MINERS CARBIDE HAT LAMP
$40.00
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$50.00
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c1918 SUN RAY DEWAR MANUFACTURING MINERS CARBIDE HAT LAMP CAST REFLECTOR
$80.00
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c1921 VICTOR MINERS CARBIDE CAP LAMP PATENTED TRADEMARK
$75.00
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SIMMONS S EXTRA CARBIDE BOTTOM CONTAINER FOR CAP LAMP NICKLE PLATED EXCELLEN
$40.00
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$45.00
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$55.00
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$10.00
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VINTAGE JUSTRITE NO2 810 CARBIDE MINERS LAMP COMPLETE IN BOX DIRECTIONS UNUSED
$158.95
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$32.00
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$45.00
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c1918 SMALL 3 1 4 SUN RAY DEWAR MANUFACTURING MINERS CARBIDE HAT LAMP
$75.00
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12 COAL MINE MINER MINING CARBIDE LAMP LANTERN LIGHT PARTS EAGLE P
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$28.50
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$44.99
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$20.00
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$23.00
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$40.00
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$26.50
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$40.00
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CARBIDE LAMP JUSTRITE MADE IN USA PATENED 1912
$9.99
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$19.99
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ANTIQUE JUSTRITE CARBIDE MINERS LAMP
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Vintage Coal Miners Cap Auto Lite Carbide Lamp 4 Tall 2 1 2 Reflector Used
$79.99
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Carbide Lamp

carbide lamp.wmv

Calcium Carbide—the Illuminating Chemical Compound

Just like with other calcium compounds that contains the suffix -ide in their names, calcium carbide is not also associated in the production of calcium-based supplements. It is commonly used on modern industrial applications as well. Read on the preceding contents of this article and learn more about calcium carbide.

Chemical Compound Reaction

Bearing the chemical formula CaC2, calcium carbide is produced through the process of electrostatic discharge by means of mixing carbon and lime at high temperature. When reacted with water, it produces acetylene. Such reaction is the principle behind the production of dissolved acetylene which is the only modern industrial use of calcium carbide.

Application

The most common application of calcium carbide is on so-called carbide lamps (also known as acetylene lamps) wherein it uses acetylene gas which is produced by means of combining the chemical compound and water. Such lamps were formerly used in mines.

Calcium carbide in this application takes the form of small pellets or chunks that is placed on the lower chamber of the lamp. Its upper chamber is filled with another reactant, which is water. There is a screw valve or similar mechanism which controls the drip rate of water to the lower chamber where the calcium carbide is stored. Such water drip rate control results to the production of acetylene gas. It results in control of the size of the flame as well as the quantity of light that it produces.

The reaction of water with calcium carbide generates enough quantity of heat apart from the flame. In cold cave conditions, the heat can be used to save someone from hypothermia.

After the entire quantity of calcium carbide is reacted with water, the lower chamber contains now a wet paste of calcium hydroxide or caustic lime which is emptied in order to be refilled for the next usage. The caustic lime is toxic on humans and animals and must be deposited on a place wherein no one will be affected.

The next application of calcium carbide is the flare which is a type of pyrotechnic that emits a brilliant light as well as intense heat without the occurrence of an explosion. It is commonly used as a signal and illumination (especially on small fishing boats) as well as defensive counter measures in military and civilian applications.

Calcium carbide is only handled within industrial production. Individuals who work with this chemical compound always take some precautionary measures to avoid any untoward incident that may happen due to mishandling of calcium carbide.

About the Author

This content is provided by Low Jeremy. It may be used only in its entirety with all links included. For more information on calcium, please visit http://calcium.articlekeep.com

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Carbide Lamp

Frequently Asked Questions...

Many years ago, bicycle lamps used to burn the gas eythene C2H2?

The gas was produced by allowing water to drip on to calcium carbide. the unbalanced equation for this reaction is
CaC2(s)+H2O(l)--->C2H2(g)+Ca(OH)2(s)

a) balance this equation
b) calculate the mass of calcium carbide which would be needed to produce 500cm^3 of eythne (at rtp)


Answer:

CaC2 + 2 H2O --> C2H2 + Ca(OH)2

22400 cc gas is formed from 1 mole = 64 g CaC2 at STP
500 cc gas will be formed from (64 x 500) / 22400 g CaC2

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