"of the sooty flame produced by acetylene. A mining or caving lamp has calcium carbide placed in a lower chamber, the generator. The upper reservoir is then filled with water. A threaded valve or other mechanism is used to control the rate at which the water is allowed to drip into the chamber containing the calcium carbide. By controlling the rate of water flow, the production of acetylene gas is controlled. This, in turn, controls the flow rate of the gas and the size of the flame at the burner, and thus the amount of light it produces. This type"
"Carbonated water Carbonated water is water containing dissolved carbon dioxide gas, either artificially injected under pressure or occurring due to natural geologic processes. Carbonation causes small bubbles to form, giving the water an effervescent quality. Common forms include sparkling natural mineral water, club soda, and commercially produced sparkling water (also known “seltzer water” in the U.S.). Club soda, sparkling mineral water, and many other sparkling waters contain added or dissolved minerals such as potassium bicarbonate, sodium bicarbonate, sodium citrate, or potassium sulfate. These occur naturally in some mineral waters but are also commonly added artificially to man-made waters to mimic"
"Carbonatation Carbonatation is a chemical reaction in which calcium hydroxide reacts with carbon dioxide and forms insoluble calcium carbonate: The process of forming a carbonate is sometimes referred to as ""carbonation"", although this term usually refers to the process of dissolving carbon dioxide in water. Carbonatation is a slow process that occurs in concrete where lime (CaO, or Ca(OH)) in the cement reacts with carbon dioxide (CO) from the air and forms calcium carbonate. The water in the pores of Portland cement concrete is normally alkaline with a pH in the range of 12.5 to 13.5. This highly alkaline environment"
"it is produced by the action of acidified water on limestone or dolomite. The reaction between hydrochloric acid and calcium carbonate (limestone or chalk) is shown below: The carbonic acid () then decomposes to water and : Such reactions are accompanied by foaming or bubbling, or both, as the gas is released. They have widespread uses in industry because they can be used to neutralize waste acid streams. Carbon dioxide is a by-product of the fermentation of sugar in the brewing of beer, whisky and other alcoholic beverages and in the production of bioethanol. Yeast metabolizes sugar to produce and"
"Calcium bicarbonate Calcium bicarbonate, also called calcium hydrogen carbonate, has a chemical formula Ca(HCO). The term does not refer to a known solid compound; it exists only in aqueous solution containing the calcium (Ca), bicarbonate (), and carbonate () ions, together with dissolved carbon dioxide (CO). The relative concentrations of these carbon-containing species depend on the pH; bicarbonate predominates within the range 6.36–10.25 in fresh water. All waters in contact with the atmosphere absorb carbon dioxide, and as these waters come into contact with rocks and sediments they acquire metal ions, most commonly calcium and magnesium, so most natural waters"
"metals from corrosion such as iron and steel by passivation of their surface. Limewater turns milky in the presence of carbon dioxide due to formation of calcium carbonate, a process called carbonatation:for example lime water When heated to 512 °C, the partial pressure of water in equilibrium with calcium hydroxide reaches 101kPa (normal atmospheric pressure), which decomposes calcium hydroxide into calcium oxide and water. Calcium hydroxide adopts a polymeric structure, as do all metal hydroxides. The structure is identical to that of Mg(OH) (""brucite structure""); i.e., the cadmium iodide motif. Strong hydrogen bonds exist between the layers. Calcium hydroxide is"
"near land (as evidenced by fossilized driftwood, which is not uncommon). When seawater is warmed by the sun, its capacity to hold dissolved gas is reduced, consequently dissolved carbon dioxide (CO) is released into the atmosphere as a gas. Calcium and bicarbonate ions within the water are then able to combine, to form calcium carbonate (CaCO) as a precipitate. The process of lime scale build up in a kettle in hard water areas is similar. Calcium carbonate is the principal constituent of most limestones. Billions of minute crystals of precipitated calcium carbonate (called calcite) accumulated forming lime mud (called micrite)"
"added to water, it sublimes to carbon dioxide gas rapidly because the solution's temperature is warmer than the dry ice (-78.5 C° or -109.3 F°). This gas can be observed as bubbles or clouds above the solution. Since the temperature of the gas is so cold, the water vapor containing in the air above the water condenses into small water droplets or cloud suspending in the carbon dioxide gas. CO CO However, some of them reacts reversibly with water molecules to form acidic solution symbolized by the production of hydrogen ion. CO + HO HCO + H When acidic solution"
"the carbide chamber contains a wet paste of slaked lime (Ca(OH)) which can be used to make a cement. This is emptied into a waste bag and the chamber can be refilled. In 1892, Thomas Willson discovered an economically efficient process for creating calcium carbide in an electric arc furnace from a mixture of lime and coke. The arc furnace provides the high temperature required to drive the reaction. Manufacture of calcium carbide was an important part of the industrial revolution in chemistry, and was made possible in the US as a result of massive amounts of inexpensive hydroelectric power"
"as cosmic rays. It was announced in 1993 that solid carbonic acid had been created by a cryogenic reaction of potassium bicarbonate and HCl dissolved in methanol. Later work showed that in fact the methyl ester had been formed, but other methods were successful. Theoretical calculations showed that a single molecule of water can catalyze the decomposition of a gas-phase carbonic acid molecule to carbon dioxide and water. In the absence of water, the dissociation of gaseous carbonic acid has been predicted to be very slow, with a half-life of 180,000 years. This only applies if the molecules are few"
"dioxide from air can react with the calcium hydroxide in concrete to form calcium carbonate. This process is called carbonatation, which is essentially the reversal of the chemical process of calcination of lime taking place in a cement kiln. Carbonatation of concrete is a slow and continuous process progressing from the outer surface inward, but slows down with increasing diffusion depth. Carbonatation has two effects: it increases mechanical strength of concrete, but it also decreases alkalinity, which is essential for corrosion prevention of the reinforcement steel. Below a pH of 10, the steel's thin layer of surface passivation dissolves and"
"cements in concrete. Non-hydraulic cement, such as slaked lime (calcium oxide mixed with water), hardens by carbonation in the presence of carbon dioxide, which is naturally present in the air. First calcium oxide (lime) is produced from calcium carbonate (limestone or chalk) by calcination at temperatures above 825 °C (1,517 °F) for about 10 hours at atmospheric pressure: The calcium oxide is then ""spent"" (slaked) mixing it with water to make slaked lime (calcium hydroxide): Once the excess water is completely evaporated (this process is technically called ""setting""), the carbonation starts: This reaction takes time, because the partial pressure of"
"by either combustion (for organic samples) or the addition of hydrochloric acid (for shell material). The resulting gas was passed through hot copper oxide to convert any carbon monoxide to , and then dried to remove any water vapour. The gas was then condensed, and converted to calcium carbonate in order to allow the removal of any radon gas and any other combustion products such as oxides of nitrogen and sulphur. The calcium carbonate was then converted back to again, dried, and converted to carbon by passing it over heated magnesium. Hydrochloric acid was added to the resulting mixture of"
"fleet use in 1996 when it was suspected of releasing chemicals into the circuit. In larger environments, such as recompression chambers or submarines, a fan is used to maintain the flow of gas through the scrubbing canister. The overall reaction is: Each mole of CO (44 g) reacting with calcium hydroxide produces one mole of water (18 g). The reaction can be considered as a strong-base-catalysed, water-facilitated reaction. The reaction mechanism of carbon dioxide with soda lime can be decomposed in three elementary steps: This sequence of reactions explains the catalytic role played by sodium hydroxide in the system and"
"and groundwater contaminated with petroleum by the process of enhanced in-situ bioremediation. Calcium peroxide Calcium peroxide or calcium dioxide is the inorganic compound with the formula CaO. It is the peroxide (O) salt of Ca. Commercial samples can be yellowish, but the pure compound is white. It is almost insoluble in water. As a solid, it is relatively stable against decomposition. In contact with water however it hydrolyzes with release of oxygen. Upon treatment with acid, it forms hydrogen peroxide. Calcium peroxide is produced by combining calcium salts and hydrogen peroxide: The octahydrate precipitates upon the reaction of calcium hydroxide"
"of the carbon dioxide formed when carbon monoxide reacts with water. Water gas Water gas is a mixture of carbon monoxide and hydrogen produced from synthesis gas. Synthesis gas is a useful product, but requires careful handling due to its flammability and the risk of carbon monoxide poisoning. The water-gas shift reaction can be used to reduce the carbon monoxide while producing additional hydrogen, resulting in water gas. Synthesis gas is made by passing steam over a red-hot carbon fuel such as coke: The reaction is endothermic, so the fuel must be continually re-heated to keep the reaction going. In"
"generally matched to the diffusion scheme; juice from RT diffusers being processed by the RT carbonatation. The clear juice from carbonatation is generally known as ""thin juice"". it may undergo pH adjustment with soda ash and addition of sulfur (""sulfitation"") prior to the next stage which is concentration by multiple effect evaporation. The carbonatation reaction takes place during lime softening (Clark's process) in water softening. Carbonatation Carbonatation is a chemical reaction in which calcium hydroxide reacts with carbon dioxide and forms insoluble calcium carbonate: The process of forming a carbonate is sometimes referred to as ""carbonation"", although this term usually"
"to other Ca centres. When strongly heated in air, calcium bromide will react with oxygen to produce calcium oxide and bromine: In this reaction the oxygen oxidizes the bromide to bromine. It is mainly used as dense aqueous solutions for drilling fluids. It is also used in neuroses medication, freezing mixtures, food preservatives, photography and fire retardants. Calcium bromide Calcium bromide is the name for compounds with the chemical formula CaBr(HO). Individual compounds include the anhydrous material (x = 0), the hexahydrate (x = 6), and the rare dihydrate (x = 2). All are white powders that dissolve in water,"
"matter, in the formation of the caves themselves. As water containing carbon dioxide (including extra CO acquired from soil organisms) passes through limestone or other calcium carbonate-containing minerals, it dissolves part of the calcium carbonate, hence becomes richer in bicarbonate. As the groundwater enters the cave, the excess carbon dioxide is released from the solution of the bicarbonate, causing the much less soluble calcium carbonate to be deposited. In the reverse process, dissolved carbon dioxide (CO) in rainwater (HO) reacts with limestone calcium carbonate (CaCO) to form soluble calcium bicarbonate (Ca(HCO)). This soluble compound is then washed away with the"
"rainwater. This form of weathering is called carbonation. In medicine, calcium bicarbonate is sometimes administered intravenously to immediately correct the cardiac depressor effects of hypokalemia by increasing calcium concentration in serum, and at the same time, correcting the acid usually present. Calcium bicarbonate Calcium bicarbonate, also called calcium hydrogen carbonate, has a chemical formula Ca(HCO). The term does not refer to a known solid compound; it exists only in aqueous solution containing the calcium (Ca), bicarbonate (), and carbonate () ions, together with dissolved carbon dioxide (CO). The relative concentrations of these carbon-containing species depend on the pH; bicarbonate predominates"
"Carbonic acid Carbonic acid is a chemical compound with the chemical formula (equivalently OC(OH)). It is also a name sometimes given to solutions of carbon dioxide in water (carbonated water), because such solutions contain small amounts of HCO. In physiology, carbonic acid is described as ""volatile acid"" or ""respiratory acid"", because it is the only acid excreted as a gas by the lungs. It plays an important role in the bicarbonate buffer system to maintain acid–base homeostasis. Carbonic acid, which is a weak acid, forms two kinds of salts: the carbonates and the bicarbonates. In geology, carbonic acid causes limestone"
"example, nitrogen reacting with sodium and carbon according to the equation - 1.5N + 3Na + 3C → 3NaCN. Aluminium carbide forms in the potlining from the reaction of aluminium metal and carbon according to the equation – 4Al + 3C → AlC. Aluminium nitride forms from a number of reactions including the reaction of cryolite with nitrogen and sodium according to the equation - NaAlF + 0.5N + 3Na → AlN + 6NaF Gases are generated from reactions of water with compounds such as un-oxidised aluminium metal, un-oxidised sodium metal, aluminium carbide and aluminium nitride. Typical gases from the"
"reacts with water or even the moisture in air to give ammonia and calcium hydroxide: Like sodium oxide, calcium nitride absorbs hydrogen above 350 °C: Calcium nitride Calcium nitride is the inorganic compound with the chemical formula CaN. It exists in various forms (isomorphs), α-calcium nitride being more commonly encountered. α-Calcium nitride adopts an anti-bixbyite structure, similar to MnO, except that the positions of the ions are reversed: calcium (Ca) take the oxide (O) positions and nitride ions (N) the manganese (Mn). In this structure, Ca occupies tetrahedral sites, and the nitride centres occupy two different types of octahedral sites."
"Frank–Caro process The Frank–Caro process, also called cyanamide process, is the nitrogen fixation reaction of calcium carbide with nitrogen gas in a reactor vessel at about 1,000°C. The reaction is exothermic and self-sustaining once the reaction temperature is reached. Originally the reaction took place in large steel cylinders with an electrical resistance element providing initial heat to start the reaction. Modern production uses rotating ovens. The synthesis produces a solid mixture of calcium cyanamide (CaCN), also known as nitrolim, and carbon. The Frank–Caro process was the first commercial process that was used worldwide to fix atmospheric nitrogen. The product was"
"a lower heat of combustion than coal gas, so the calorific value was often boosted by passing the gas through a heated retort, into which oil was sprayed. The resulting mixed gas was called ""carburetted water gas"". ""Semi-water gas"" is a mixture of water gas and producer gas made by passing a mixture of air and steam through heated coke. The heat generated when producer gas is formed keeps the temperature of the coke high enough to allow water gas to be formed. Pure hydrogen can be obtained from water gas by using the water-gas shift reaction, after subsequent removal"
"reaction between carbon dioxide and water to form carbonic acid. This acid immediately dissociates into hydrogen and bicarbonate ions. The hydrogen ions leave the cell through H/K ATPase antiporter pumps. At the same time, sodium ions are actively reabsorbed. This means that the majority of secreted K and Na ions return to the cytoplasm. In the canaliculus, secreted hydrogen and chloride ions mix and are secreted into the lumen of the oxyntic gland. The highest concentration that gastric acid reaches in the stomach is 160 mM in the canaliculi. This is about 3 million times that of arterial blood, but"
"water arose from the observation by Richard Bewley, an 18th-century English chemist from Norfolk, that the addition of a little sodium carbonate to the water greatly facilitated the absorption of carbon dioxide. Modern carbonated water is made by injecting pressurized carbon dioxide into water. The pressure increases the solubility and allows more carbon dioxide to dissolve than would be possible under standard atmospheric pressure. When the bottle is opened, the pressure is released, allowing gas to exit the solution, forming the characteristic bubbles. In the United States, carbonated water was known as ""soda water"" until World War II, due to"
"may also be prepared by reacting liquid hydrocyanic acid with calcium carbide. Alternatively calcium cyanide may be prepared by reacting hydrocyanic acid gas with quicklime (CaO) at high temperatures around 400 °C. At higher temperatures around 600 °C calcium cyanimide is formed instead. The material prepared often is contaminated with polymeric derivatives of hydrogen cyanide, hence the black color. Calcium cyanide hydrolyzes readily to form hydrogen cyanide gas. The presence of acid accelerated evolution of hydrogen cyanide gas. It is reactive toward oxidizing agents. Calcium cyanide is also sometimes used to produce ammonium cyanide by reacting it with ammonium carbonate."
"sodium carbonate (""washing soda""), sodium bicarbonate (""baking soda""), or sodium hydroxide (""lye"", or ""caustic soda""). Any of these reactions produce sodium acetate and water. When a sodium and carbonate ion-containing compound is used as the reactant, the carbonate anion from sodium bicarbonate or carbonate, reacts with hydrogen from the carboxyl group (-COOH) in acetic acid, forming carbonic acid. Carbonic acid readily decomposes under normal conditions into gaseous carbon dioxide and water. This is the reaction taking place in the well-known ""volcano"" that occurs when the household products, baking soda and vinegar, are combined. Industrially, sodium acetate trihydrate is prepared by"
"as a component of rocket fuel by the Luftwaffe. Calcium permanganate Calcium permanganate is an oxidizing agent and chemical compound with the chemical formula Ca(MnO). It consists of the metal calcium and two permanganate ions. It is noncombustible, but, being a strong oxidizing agent, it will accelerate the burning of combustible material. If the combustible material is finely divided, the resulting mixture may be explosive. Contact with liquid combustible materials may result in spontaneous ignition. Contact with sulfuric acid may cause fires or explosions. Mixtures with acetic acid or acetic anhydride can explode if not kept cold. Explosions can occur"
"Calcium nitride Calcium nitride is the inorganic compound with the chemical formula CaN. It exists in various forms (isomorphs), α-calcium nitride being more commonly encountered. α-Calcium nitride adopts an anti-bixbyite structure, similar to MnO, except that the positions of the ions are reversed: calcium (Ca) take the oxide (O) positions and nitride ions (N) the manganese (Mn). In this structure, Ca occupies tetrahedral sites, and the nitride centres occupy two different types of octahedral sites. Calcium nitride is formed along with the oxide, CaO, when calcium burns in air. It can be produced by direct reaction of the elements: It"
"Water gas Water gas is a mixture of carbon monoxide and hydrogen produced from synthesis gas. Synthesis gas is a useful product, but requires careful handling due to its flammability and the risk of carbon monoxide poisoning. The water-gas shift reaction can be used to reduce the carbon monoxide while producing additional hydrogen, resulting in water gas. Synthesis gas is made by passing steam over a red-hot carbon fuel such as coke: The reaction is endothermic, so the fuel must be continually re-heated to keep the reaction going. In order to do this, an air stream, which alternates with the"
"for most terrestrial applications as it reacts quickly with atmospheric oxygen, its use as such in space has been considered. The chemistry of calcium is that of a typical heavy alkaline earth metal. For example, calcium spontaneously reacts with water more quickly than magnesium and less quickly than strontium to produce calcium hydroxide and hydrogen gas. It also reacts with the oxygen and nitrogen in the air to form a mixture of calcium oxide and calcium nitride. When finely divided, it spontaneously burns in air to produce the nitride. In bulk, calcium is less reactive: it quickly forms a hydration"