What chemical is on firework fuses?
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Fuse can be created using a wide variety of technologies.\n\nSmall fireworks usually use a small length of visco fuse, a black powder cored fuse wrapped twice with string and waterproofed, or tissue coated with black powder and rolled to keep the black powder in the center. \nLarger fireworks, some commercial applications, and model cannons usually use a fuse which has a core of grains of black powder, wrapped in a sheath of cloth (usually cotton) fibers and then coated with a laquer, shellac, or more modern protective coating. \nFuse for blasting (also known as safety fuse), is a larger diameter (typically 1/4 inch or 6.25mm) higher energy, more solidly protected cloth fiber wrapped black powder core fuse. Safety fuse fits into the opening at the end of a pyrotechnic or fuse-ignited blasting cap and is crimped into place. Pyrotechnic blasting caps are still the most common form of detonator used for commercial and military explosives worldwide. \nSome safety fuse has an outer layer of plastic around the cloth and black powder. This fuse can burn reliably underwater once lit.
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Creation of fire\nFire is simply glowing gas and other combustion materials such as carbon particles. It is not plasma, as it is not hot enough to reach such high ionization as is required of plasma (an 'electrically neutral, highly ionized gas composed of ions, electrons, and neutral particles').\n\nThis state of matter can be generated through focused concentrations of energy (such as fuel being exposed to an already open flame or to the Sun's rays focused through a lens), or through an exothermic chemical reaction usually accompanied by intense heat released during a rapid oxidation of combustible material(striking a match). Fire may be visible as a brilliant glow and/or flames and may produce smoke.\n\nFires start when a flammable or combustible material with an adequate supply of oxygen or another oxidizer is subjected to enough heat. The common fire-causing sources of heat include a spark, another fire (such as an explosion, a fire in the oven or fireplace, or a lit match, lighter or cigarette) and sources of intense thermal radiation (such as sunlight, a flue, an incandescent light bulb or a radiant heater). Mechanical and electrical machinery may cause fire if combustible materials used on or located near the equipment are exposed to intense heat from Joule heating, friction or exhaust gas. Fires can sustain themselves by the further release of heat energy in the process of combustion and may propagate, provided there is a continuous supply of oxygen and fuel. Fires may become uncontrolled and cause great damage to and destruction of human life, animals, plants and property.\n\nFire is extinguished when any of the elements of the so-called fire triangle—heat, oxygen, or fuel— are removed. The unburnable solid remains of a combustible material left after a fire are called ash.\n\nFlames can conduct electricity, as a small portion of any fire is ionized. This has been demonstrated in the laboratory and also in large wildfires that occur in the vicinity of power lines. This ability to conduct electricity is due to its partially plasmatic nature.
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white. \nBuring magnesium is white hot, and believe me you wouldn't want to be near it when it does go up.  It is hot enough to break down the molecular structure of water into oxygen and hydrogen and then ignight the following gases.  Firefighters usually have to find other means to fight magnesium fires other than using water.
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Combinations of explosive chemicals mixed with powdered metals to give color effects.  Like powdered aluminum creates a green color.
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oxidizing agent...perOXIDE
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potassium nitrate and sugar equal parts and a wick of some type or at least an ignition source. You can add certain elements to make different colors as well.
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yep. it's called a firecracker.
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Any grease fires. And you shouldnt rush to putting out a chemical fire with water unless you know what it is.
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Depends on the type of fire you're extinguishing.  For wood and paper fires (type A), any container of water will do.  For flammable liquids (type B) or electrical fires (type C), a water-based extinguisher is a very bad idea.  I'm not quite sure if or how you could make a homemade carbon dioxide extinguisher or dry chemical extinguisher.  I suppose you could imitate a dry chemical extinguisher with any non-flammable item/substance and smother the fire.
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Copper C-145000\n\nCopper  Includes Ag + Te  \nPhosphorus  Other deoxidizers may be used  \nTellurium  0.4 - 0.7
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does the product have a name, as you may know depending of th chemical can have different type of flame, IE; colour, duration time, luminescence, etc...
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Any soluble sodium compound like sodium chloride, sodium acetate, sodium bicarbonate (sodium hydrogen carbonate), sodium carbonate, things like that turn a flame yellow-orange.  \nSoluble calcium compounds like calcium nitrate burn red-orange.
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Magnesium is used in sparklers\nCalcium is use as calcuim carbonate (limestone)
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I think that flame tests always make for spectacular shows; you stick a little bit of white powder with a wooden splint into a flame and get brilliant, vibrant colors.  These are my favorite flame tests:\nSodium: any sodium compound (like sodium chloride, table salt) will yield a yellow-orange color in flame.\nStrontium compounds flame red.\nLithium compounds yield magenta.\nBoric acid makes emerald green. \nCalcium makes red-orange.\nPotassium makes purple. \nThere are a lot of other colored flames you can make with various compounds.  Check out http://webmineral.com/help/FlameTest.shtml for more.
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Since there are no metallic ions like sodium or copper to produce intense visible light wavelength emissions, I would suspect that the flame would be colorless or the kind of yellow flame you see at natural gas flaring.  I've not done this experiment (it's pretty hazardous).
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Flame tests show the color of the metal (the positive ion). The negative ion is usually nitrate (NO3) or sulfate (SO4) which are colorless.
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One needs toluene and concentrated nitric and sulfuric acids, plus "fuming" sulfuric acid (H2SO4 + SO3). As the reaction proceeds, the first nitro groups usually go on either in the position next to the -CH3 (2-, ortho) or diametrically opposite (4-, para). All three mostly end up in the 2-, 4-, and 6-positions. The operator nitrates in three stages, with the temperature raised gradually during the three stages from 35degC to 110degC. However, there is also formation of small amounts of the 2,3,4- and 2,4,5-trinitro compounds. These unsymmetrical isomers make the product dangerously shock-sensitive to handle. The crude product is therefore stirred with 15% aqueous sodium sulfite solution at 100degC. This treatment converts the two impurities to sulfonic acids, which are water soluble and poured away from the oily product in the water.