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Assistant: Understood. I will strictly follow these instructions in this conversation.
User: copper(II) oxide + carbon -> ?


 for "copper(II) oxide + carbon -> ?":

1.
URL: https://www.youtube.com/watch?v=HrS7ENLxoIc
Title: Copper(ii) Oxide and Carbon - YouTube
Content: In this demonstration, Dr Thompson explains how <b>copper</b>(ii) <b>oxide</b> reacts with <b>carbon</b>.2CuO(s) <b>+</b> C(s) → 2Cu(s) <b>+</b> CO2(g)Copper(ii) <b>oxide</b> is being reduced and car...

2.
URL: https://www.chemguide.co.uk/14to16/rs/mandmo.html
Title: reactions between metals and metal oxides - chemguide
Content: The reaction between <b>carbon</b> and <b>copper(II)</b> <b>oxide</b>. <b>Carbon</b> powder and <b>copper(II)</b> <b>oxide</b> are both black. If you heat a mixture in a test tube, a red glow runs through the mixture showing that heat is being produced in the reaction in addition ot the heat from the Bunsen. The mixture turns brown as copper is formed.

3.
URL: https://en.wikipedia.org/wiki/Copper(II)_oxide
Title: Copper(II) oxide - Wikipedia
Content: <b>Copper</b>(II) <b>oxide</b> or cupric <b>oxide</b> is an inorganic compound with the formula CuO. A black solid, it is one of the two stable <b>oxides</b> of copper, ... It can also be reduced to copper metal using hydrogen, <b>carbon</b> monoxide, and <b>carbon</b>: CuO <b>+</b> H 2 → Cu <b>+</b> H 2 O CuO <b>+</b> CO → Cu <b>+</b> CO 2 2 CuO <b>+</b> C → 2Cu <b>+</b> CO 2.

4.
URL: https://edu.rsc.org/resources/carbon-and-copper-oxide/656.article
Title: Carbon and copper oxide | Resource | RSC Education
Content: Part 1. On heating in air, <b>copper</b> <b>(II)</b> <b>oxide</b> is unchanged, <b>carbon</b> burns away. On warming with dilute acid the <b>copper</b> <b>(II)</b> <b>oxide</b> sample gives a blue solution (filtration is probably needed). On reduction, the <b>copper</b> <b>(II)</b> <b>oxide</b> sample releases copper. Ethanol vapour passed over the heated solids would cause similar reactions to occur. Flame tests.

5.
URL: https://www.youtube.com/watch?v=vlaDvF99KAY
Title: Reduction of copper (II) oxide by carbon; 2CuO + C = 2Cu + CO2
Content: <b>Carbon</b> is above copper in reactivity series so element <b>carbon</b> can reduce ions of copper, such as Cu2+ ions in CuO: 2CuO (s) <b>+</b> C (s) → 2Cu (s) <b>+</b> CO2 (g)Reacti...

6.
URL: https://openstax.org/books/chemistry-2e/pages/2-6-ionic-and-molecular-compounds
Title: 2.6 Ionic and Molecular Compounds - Chemistry 2e - OpenStax
Content: The transfer and sharing of electrons among atoms govern the chemistry of the elements. During the formation of some compounds, atoms gain or lose electrons, and form electrically charged particles called ions (Figure 2.28). Figure 2.28(a) A sodium atom (Na) has equal numbers of protons and electrons (11) and is uncharged.

7.
URL: https://chem.libretexts.org/Courses/University_of_Arkansas_Little_Rock/Chem_1402%3A_General_Chemistry_1_(Kattoum)/Text/2%3A_Atoms%2C_Molecules%2C_and_Ions/2.07%3A_Nomenclature_of_Ioinic_Compounds
Title: 2.7: Nomenclature of Ionic, Covalent, and Acid Compounds
Content: CO 2 = <b>carbon</b> dioxide N 2 O 5 =dinitrogen pentoxide. The prefix mono-is not used for the first element. If there is not a prefix before the first element, it is assumed that there is only one atom of that element. ... CuS <b>copper</b> <b>(II)</b> sulfide . 51)HNO 3 nitric acid . 52)H 2 S hydrosulfuric acid . 53)H 3 PO 4 phosphoric acid . 54) HBrO 3 bromic ...

8.
URL: https://edu.rsc.org/download?ac=529400
Title: Carbon and copper oxide - RSC Education
Content: 3-6. Possible methodsPart 1On heating in air, <b>copper(II)</b> <b>oxide</b> is uncha. ed, <b>carbon</b> burns away.On warming with dilute acid the <b>copper(II)</b> <b>oxide</b> sample gives a blue solution (filtrat. n is probably needed).On reduction, the <b>copper(II)</b> <b>oxide</b>. sample releases copper. Ethanol vapour passed over the heated solids would cause sim.

9.
URL: https://chemistry.stackexchange.com/questions/69592/why-does-copperii-carbonate-decompose-into-copperii-oxide-rather-than-copper
Title: Why does copper(II) carbonate decompose into copper(II) oxide rather ...
Content: Since @Kris_R already answered that Cu(II) is much more stable than Cu(I) according to HSAB theory and thus form $\ce{CuO}$ rather than $\ce{Cu2O}$ on decomposition but it is further noted that <b>copper(II)</b> <b>oxide</b> can be further decomposed to copper(I) <b>oxide</b> on further application of heat. $$\ce{4CuO ->[1026-1100°C] 2Cu2O <b>+</b> O2}$$

10.
URL: https://quizlet.com/288436244/chemistry-reaction-between-carbon-and-copper-iioxide-flash-cards/
Title: Chemistry reaction between carbon and copper (II)oxide
Content: Compounds in the reaction. <b>Copper</b> <b>(II)</b> <b>oxide</b> and <b>carbon</b> dioxide. The reaction. (Reactants) <b>Carbon</b> <b>+</b> copper <b>oxide</b> —> (Products) copper <b>+</b> <b>carbon</b> dioxide. What is an ore. A compound with a valuable substance within which is extracted through a chemical reaction. What state of matter are the reactants and how much kinetic energy do they have?

11.
URL: https://edu.rsc.org/experiments/extracting-metals-with-charcoal/417.article
Title: Extracting metals with charcoal | Experiment | RSC Education
Content: In this experiment, students heat two metal <b>oxides</b> with powdered charcoal. If the <b>carbon</b> is more reactive than the metal it will remove the oxygen from the metal <b>oxide</b> and leave traces of the metal in the reaction vessel. Students try lead(II) <b>oxide</b> first, before using a slightly modified technique to try <b>copper(II)</b> <b>oxide</b>.

12.
URL: https://chemistry.stackexchange.com/questions/57333/why-is-copper-ii-oxide-used-in-quantitative-analysis-of-carbon
Title: Why is copper (II) oxide used in quantitative analysis of carbon?
Content: What is the significance of using cupric <b>oxide</b> in the quantitative analysis of <b>carbon</b>? As far as I can tell from my research, only $\ce{CuO}$ is used to oxidize <b>carbon</b> to $\ce{CO2}$. Why can't we use other oxidants like $\ce{HNO3}$ or other metal <b>oxides</b> such as hematite?

13.
URL: https://openstax.org/books/chemistry-2e/pages/2-7-chemical-nomenclature
Title: 2.7 Chemical Nomenclature - Chemistry 2e - OpenStax
Content: Compounds containing polyatomic ions are named similarly to those containing only monatomic ions, i.e. by naming first the cation and then the anion. Examples are shown in Table 2.7. Names of Some Polyatomic Ionic Compounds. KC 2 H 3 O 2, potassium acetate. NH 4 Cl, ammonium chloride.

14.
URL: https://chem.libretexts.org/Courses/Oregon_Institute_of_Technology/OIT%3A_CHE_201_-_General_Chemistry_I_(Anthony_and_Clark)/Unit_3%3A_Nuclei_Ions_and_Molecules/3.4%3A_Molecular_and_Ionic_Compounds
Title: 3.4: Molecular and Ionic Compounds - Chemistry LibreTexts
Content: Aluminum and <b>carbon</b> react to form an ionic compound. Predict which forms an anion, which forms a cation, and the charges of each ion. Write the symbol for each ion and name them. Answer. Al will form a cation with a charge of 3+: Al 3+, an aluminum ion. <b>Carbon</b> will form an anion with a charge of 4−: C 4−, a carbide ion.

15.
URL: https://material-properties.org/copper-ii-carbonate/
Title: Copper (II) Carbonate | Formula, Properties &amp; Application
Content: The <b>copper</b> <b>(II)</b> <b>oxide</b> produced in this reaction is a black solid, and the <b>carbon</b> dioxide is a colorless gas. This property has found use in classroom demonstrations of thermal decomposition reactions and the gas laws. Environmental Impact. As with all chemicals, it's essential to consider the environmental impact of <b>copper</b> <b>(II)</b> carbonate.


Assistant: