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Soda lime canister used in anaesthetic machines to act as a carbon dioxide scrubber. Soda lime, a mixture of sodium hydroxide (NaOH) and calcium oxide (CaO), is used in granular form within recirculating breathing environments like general anesthesia and its breathing circuit, submarines, rebreathers, and hyperbaric chambers and underwater habitats.
The standard Gibbs free energy of formation (G f °) of a compound is the change of Gibbs free energy that accompanies the formation of 1 mole of a substance in its standard state from its constituent elements in their standard states (the most stable form of the element at 1 bar of pressure and the specified temperature, usually 298.15 K or 25 °C).
Chemical or power production: Solid sprays or slurries of calcium oxide can be used to remove sulfur dioxide from exhaust streams in a process called flue-gas desulfurization. Carbon capture and storage: Calcium oxide can be used to capture carbon dioxide from flue gases in a process called calcium looping.
Its solubility product K sp of 5.02 × 10 −6 at 25 °C, [1] its dissociation in water is large enough that its solutions are basic according to the following dissolution reaction: Ca(OH) 2 → Ca 2+ + 2 OH −. The solubility is affected by the common-ion effect. Its solubility drastically decreases upon addition of hydroxide or calcium sources.
Gas C 716.67 Carbon dioxide: Gas CO 2: −393.509 Carbon disulfide: Liquid CS 2: 89.41 Carbon disulfide: Gas CS 2: 116.7 Carbon monoxide: Gas CO −110.525 Carbonyl chloride Gas COCl 2: −218.8 Carbon dioxide (un–ionized) Aqueous CO 2 (aq) −419.26 Bicarbonate ion Aqueous HCO 3 – −689.93 Carbonate ion Aqueous CO 3 2– −675.23 ...
Calcium peroxide or calcium dioxide is the inorganic compound with the formula CaO 2. It is the peroxide (O 2 2− ) salt of Ca 2+ . Commercial samples can be yellowish, but the pure compound is white.
The reaction of calcium carbide with water, producing acetylene and calcium hydroxide, [5] was discovered by Friedrich Wöhler in 1862. CaC 2 + 2 H 2 O → C 2 H 2 + Ca(OH) 2 . This reaction was the basis of the industrial manufacture of acetylene, and is the major industrial use of calcium carbide.
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 2) in rainwater (H 2 O) reacts with limestone calcium carbonate (CaCO 3) to form soluble calcium bicarbonate (Ca(HCO ...