Potassium, chlorate chloride

Methyl orange III, P. 23 Nickel chloride XI Nitric acid, 6mormal Nitric acid, 16-normal Phenolphthalein P. 53 Phosphoric acid, ortho, 85% IV Potassium chlorate (chloride free) III Potassium ferricyanide III, IX, P. 73, Q. 73... 

Pyrotechnic mixtures may also contain additional components that are added to modify the bum rate, enhance the pyrotechnic effect, or serve as a binder to maintain the homogeneity of the blended mixture and provide mechanical strength when the composition is pressed or consoHdated into a tube or other container. These additional components may also function as oxidizers or fuels in the composition, and it can be anticipated that the heat output, bum rate, and ignition sensitivity may all be affected by the addition of another component to a pyrotechnic composition. An example of an additional component is the use of a catalyst, such as iron oxide, to enhance the decomposition rate of ammonium perchlorate. Diatomaceous earth or coarse sawdust may be used to slow up the bum rate of a composition, or magnesium carbonate (an acid neutralizer) may be added to help stabilize mixtures that contain an acid-sensitive component such as potassium chlorate. Binders include such materials as dextrin (partially hydrolyzed starch), various gums, and assorted polymers such as poly(vinyl alcohol), epoxies, and polyesters. Polybutadiene mbber binders are widely used as fuels and binders in the soHd propellant industry. The production of colored flames is enhanced by the presence of chlorine atoms in the pyrotechnic flame, so chlorine donors such as poly(vinyl chloride) or chlorinated mbber are often added to color-producing compositions, where they also serve as fuels. 

Manufacture. Most chlorate is manufactured by the electrolysis of sodium chloride solution in electrochemical cells without diaphragms. Potassium chloride can be electroly2ed for the direct production of potassium chlorate (35,36), but because sodium chlorate is so much more soluble (see Fig. 2), the production of the sodium salt is generally preferred. Potassium chlorate may be obtained from the sodium chlorate by a metathesis reaction with potassium chloride (37). 

The first large-scale use of chlorine was for bleaching paper and cotton textiles it also is widely used as a germicide for public water supplies. Presently it is used principally in production of the chemical compounds sulfur chloride, thionyl chloride, phosgene, aluminum chloride, iron(ni) chloride, titaniura(IV) chloride, tin(IV) chloride, and potassium chlorate. 

When potassium chlorate is burned, potassium chloride and oxygen are formed. 

If potassium chlorate, KCIO is heated gently, the crystals will melt. Further heating will decompose it to give oxygen gas and potassium chloride, KC1. 

Write the balanced chemical equation for (a) the thermal decomposition of potassium chlorate without a catalyst (b) the reaction of bromine with water (c) the reaction between sodium chloride and concentrated sulfuric acid, (d) Identify each reaction as a Bronsted acid—base, Lewis acid—base, or redox reaction. 

C03-0068. Write chemical formulas for these compounds (a) potassium chlorate (b) ammonium hydrogen carbonate (c) iron(II) phosphate (d) copper(II) nitrate hexahydrate (e) aluminum chloride (Q cadmium(II) chloride and (g) potassium oxide. 

C03-0110. The following pairs of substances are quite different despite having similar names. Write correct formulas for each, (a) sodium chloride and sodium hypochlorite (b) nitrogen oxide and nitrogen dioxide (c) potassium chlorate and potassium perchlorate and (d) ammonia and ammonium ion. 

C04-0012. When heated, potassium chlorate decomposes to potassium chloride and gaseous molecular oxygen 2 KCIO3 2KC1 + 3 O2 What is the theoretical yield of oxygen when 5.00 g of potassium chlorate decomposes Calculate the percent yield if a 5.00-g sample gives 1.84 g O2 on decomposition. Give possible reasons why the actual yield is less than the theoretical yield. 

Alkaline-earth sulfides react vigorously with chromyl chloride, lead dioxide, potassium chlorate (explodes lightly) and potassium nitrate (explodes violently). 

Alloxantin has been obtained by the oxidation of uric acid with nitric acid, followed by reduction with hydrogen sulfide 2 by oxidation of uric acid with potassium chlorate, followed by reduction with stannous chloride by condensation of alloxan with dialuric acid in aqueous solution and by oxidation of dialuric acid. ... 

Tin(IV) chloride Titanium Alkyl nitrates, ethylene oxide, K, Na turpentine Aluminum, boron trifluoride, carbon dioxide, CuO, halocarbons, halogens, PbO, nitric acid, potassium chlorate, potassium nitrate, potassium permanganate, steam at high temperatures, water... 

Other inorganic crystals studied by Mark and his collaborators, sometimes leading to complete structure determinations, include strontium chloride, zinc hydroxide, tin tetraiodide, potassium chlorate, potassium permanganage, and ammonium ferrocyanide. Minerals investigated by them include CaSO (anhydrite), BaSO (barite), PbSO, Fe2TiO[j (pseudobrookite), and three forms of Al2Si05 (cyanite, andalusite, and sillimanite). 

A sample containing 2/3 mole of potassium chlorate, KC103, is heated until it decomposes to potassium chloride and oxygen gas. The oxygen is collected in an inverted bottle through the displacement of water. Answer the following questions using this information. 

Oxygen (Gas), Carbon disulfide, Mercury, Anthracene, 4831 Oxygen (Liquid), Carbon, Iron(II) oxide, 4832 Oxygen difluoride, Hexafluoropropene, Oxygen, 4317 Potassium chlorate, Manganese dioxide, 4017 f Propionyl chloride, Diisopropyl ether, 1163 f Propylene oxide, Sodium hydroxide, 1225 Silver azide, 0023 Silver nitride, 0038 Sodium carbonate, 0552 Sodium peroxoborate, 0155 Tetrafluoroammonium tetrafluoroborate, 0133 Triallyl phosphate, 3184... 

Two of the substances on the head of a safety match are potassium chlorate and sulfur. When the match is struck, the potassium chlorate decomposes to give potassium chloride and oxygen. The sulfur then burns in the oxygen and ignites the wood of the match. 

It reacts violently with potassium chlorate forming phosphoryl chloride ... 

Potassium chlorate may be prepared by mixing concentrated solutions of sodium chlorate and potassium chloride. Potassium chlorate crystallizes when the solubility product [K+] [ClOs j is exceeded. 

Potassium chlorate decomposes on heating below its melting point and in the presence of a catalyst, forming potassium chloride and oxygen. The reaction is catalyzed by manganese dioxide and is used in laboratory preparation of oxygen ... 

Potassium Chlorate. .. Potassium Triiodo Mercurate(ll) Potassium Chloride Potassium Chlorate Potassium Chromate Potassium Cyanide Potassium Dichromate Potassium Ferricyanide Potassium Ferrocyanide Potassium Fluoride Potassium Formate Potassium Hydride Potassium Hydrogen Phthalate Potassium Hydroxide Potassium lodate... 

If this reaction occurs, the chance of spontaneous ignition of the mixture is likely. Therefore, any composition containing both a chlorate salt and an ammonium salt must be considered extremely hazardous. The shipping regulations of the United States Department of Transportation classify any such mixtures as "forbidden explosives" because of their instability [8]. However, compositions consisting of potassium chlorate, ammonium chloride, and organic fuels have been used, reportedly safely, for white smoke production [Ij. 

Finally, a product of a pyrotechnic reaction may vaporize from the reaction zone and subsequently condense as fine particles in air, creating a smoke. Potassium chloride (boiling point 1407°C) produces smoke in many potassium chlorate and potassium perchlorate compositions, although smoke is usually not a goal sought from these mixtures. 

One of the very best, and certainly the most controversial, of the common oxidizers is potassium chlorate, KCIO 3. It is a white, crystalline material of low hygroscopicity, with 39.2% oxygen by weight. It is prepared by electrolysis from the chloride salt. 

Potassium chlorate Potassium chloride, Bleach (Calcium hypochlorite) Low explosive, lED filler, Black powder weapon propellant, Oxidizer... 

Anhydrous hydrazine, Cyanogen bromide, Isopropyl alcohol, Sodium nitrite, Sodium bicarbonate, Copper nitrate cryohydrate Sodium nitrate, Sodium chloride. Sugar, Charcoal powder Potassium nitrate. Sodium chlorate. Sugar, Charcoal powder Potassium nitrate. Potassium chlorate. Sugar, Charcoal powder Sodium nitrate. Potassium chlorate. Sugar, Charcoal powder 3-Pyridol, Ethylmethylamine, Formaldehyde, Pyridine, Dimethylcarbamoyl chloride. Sodium carbonate. Chloroform, Sodium sulfate, 1,10-Dibromodecane, Acetone, Acetonitrile, Charcoal, Ethyl acetate... 

Potassium chloride. Bleach Red phosphorus. Potassium chlorate. Alcohol Quebrachitol, Nitric acid. Sulfuric acid. Sodium bicarbonate Hexamine, Nitric acid. Sodium nitrate PropionitrUe, Sulfuric acid, Trioxane, Nitric acid DAPT, Acetic acid. Ammonium nitrate. Nitric acid. Acetic anhydride... 

Monochloroacetic Acid Chloroacetyl Chloride Potassium Chlorate Potassium Chlorate Sodium Chlorate Chlordane Chlordane... 

The presence of a certain excess of base prevents the conversion of the hypochlorite into chlorate and chloride, whereas it is rapidly effected when the acid is in excess. It is therefore necessary to add the acid to the alkaline substance in quantity insufficient for saturation, and constantly to agitate the bottle immersed in cold water and not to reverse the operation by gradually saturating the acid with the base. By taking these precautions, cone. soln. of hypochlorous acid and potash may be used without precipitating potassium chlorate, notwithstanding the sparing solubility of this salt. This proves that u any chlorate is formed, the quantity is very small. 

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