[6] Due to low bioactivity, negligible copper is absorbed. Copper(II) oxide or cupric oxide is the inorganic compound with the formula CuO. By using this website, you signify your acceptance of, calcium hydroxide + carbon dioxide = calcium carbonate + water, Enter an equation of a chemical reaction and click 'Balance'. The answer will appear below, Always use the upper case for the first character in the element name and the lower case for the second character. Enter either the number of moles or weight for one of the compounds to compute the rest. [9][10], Except where otherwise noted, data are given for materials in their. Phys. Compound states [like (s) (aq) or (g)] are not required. Copper oxide react with hydrogen CuO + H 2 Cu + H 2 O [ Check the balance ] Copper oxide react with hydrogen to produce copper and water. 129, 12 (1999) 2278-2279, National Institute for Occupational Safety and Health, Ullmann's Encyclopedia of Industrial Chemistry, "Uses of Copper Compounds: Other Copper Compounds", https://www.ima-mineralogy.org/Minlist.htm, National Pollutant Inventory - Copper and compounds fact sheet, CDC - NIOSH Pocket Guide to Chemical Hazards, https://en.wikipedia.org/w/index.php?title=Copper(II)_oxide&oldid=988650067, Chemical articles with multiple compound IDs, Multiple chemicals in an infobox that need indexing, Pages using collapsible list with both background and text-align in titlestyle, Articles containing unverified chemical infoboxes, Creative Commons Attribution-ShareAlike License, This page was last edited on 14 November 2020, at 12:53. Matter 3 (1991) 5257-5261 , Cupric Oxide Should Not Be Used As a Copper Supplement for Either Animals or Humans, Baker, D. H., J. Nutr. If you do not know what products are enter reagents only and click 'Balance'. Examples: Fe, Au, Co, Br, C, O, N, F. Compare: Co - cobalt and CO - carbon monoxide, To enter an electron into a chemical equation use {-} or e. To enter an ion specify charge after the compound in curly brackets: {+3} or {3+} or {3}. [1], The work function of bulk CuO is 5.3 eV[5], As a significant product of copper mining, copper(II) oxide is the starting point for the production of other copper salts. CuO + H2O = Cu(OH)2 Instructions and examples below may help to solve this problem You can always ask for help in the forum Instructions on balancing chemical equations: Enter an equation of a chemical reaction and click 'Balance'. : Condens. As a mineral, it is known as tenorite. Cupric oxide is used as a pigment in ceramics to produce blue, red, and green, and sometimes gray, pink, or black glazes. It is a product of copper mining and the precursor to many other copper-containing products and chemical compounds.[3]. Copper oxide was also used in a lithium battery type (IEC 60086 code "G"). In many cases a complete equation will be suggested. The ores are treated with an aqueous mixture of ammonium carbonate, ammonia, and oxygen to give copper(I) and copper(II) ammine complexes, which are extracted from the solids. Reaction stoichiometry could be computed for a balanced equation. It can be formed by heating copper in air at around 300–800°C: For laboratory uses, pure copper(II) oxide is better prepared by heating copper(II) nitrate, copper(II) hydroxide, or basic copper(II) carbonate:[4], Copper(II) oxide dissolves in mineral acids such as hydrochloric acid, sulfuric acid or nitric acid to give the corresponding copper(II) salts:[4]. [7], It is also used when welding with copper alloys.[8]. It reacts with concentrated alkali to form the corresponding cuprate salts: It can also be reduced to copper metal using hydrogen, carbon monoxide, or carbon: When cupric oxide is substituted for iron oxide in thermite the resulting mixture is a low explosive, not an incendiary. The answer will appear below; It is also incorrectly used as a dietary supplement in animal feed. If you do not know what products are enter reagents only and click 'Balance'. The effect of hydrostatic pressure on the ambient temperature structure of CuO, Forsyth J.B., Hull S., J. A black solid, it is one of the two stable oxides of copper, the other being Cu2O or copper(I) oxide (cuprous oxide). In many cases a … It is produced on a large scale by pyrometallurgy, as one stage in extracting copper from its ores. Copper(II) oxide belongs to the monoclinic crystal system. The copper atom is coordinated by 4 oxygen atoms in an approximately square planar configuration. Copper(II) oxide dissolves in mineral acids such as hydrochloric acid, sulfuric acid or nitric acid to give the corresponding copper(II) salts: A copper oxide electrode formed part of the early battery type known as the Edison–Lalande cell. For instance equation C6H5C2H5 + O2 = C6H5OH + CO2 + H2O will not be balanced, but PhC2H5 + O2 = PhOH + CO2 + H2O will; Compound states [like (s) (aq) or (g)] are not required. For example, many wood preservatives are produced from copper oxide.[3]. Substitute immutable groups in chemical compounds to avoid ambiguity. An example of natural copper(I,II) oxide is the mineral paramelaconite, Cu+2Cu2+2O3. These complexes are decomposed with steam to give CuO. Limiting reagent can be computed for a balanced equation by entering the number of moles or weight for all reagents. 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