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but PhC2H5 + O2 = PhOH + CO2 + H2O will; Compound states [like (s) (aq) or (g)] are not required. Aqueous Ammonia. Learn vocabulary, terms, and more with flashcards, games, and other study tools. CuO (s) + H2O (l) D. CuO (s) + H2SO4 (aq) ! Characteristic reactions of Cu²âº The +2 oxidation state is more common than the +1. Complete the following chemical reaction and classify into (a) hydrolysis, (b) redox and (c) hydration reactions. Copper(II) ion reacts with stoichiometric quantities of aqueous ammonia to precipitate light blue Cu(OH)2. … CuCO3 + 2NaCl + CuCl2 + 2H2O -> CuCl2 + H2O + CO2 + Cu(OH)2 + 2NaCl. In many cases a complete equation will be suggested. The 2NaCl on both sides cancel, and t6he H2O on the right cancels ONE of the 2H2O on the left. The net reaction for these two reactions is: CuCO3 + CuCl2 + H2O -> CuCl2 + CO2 + Cu(OH)2. decomposition AND acid-base c.) oxidation-reduction AND oxidation-reduction d.) acid-base AND oxidation-reduction Start studying [Cu(H2O)6]2+ reactions. CuSO4 (aq) + H2O (l) E. CuSO4 (aq) + Zn (s) ! Balanced half-reactions are well tabulated in handbooks and on the web in a 'Tables of standard electrode potentials'. If you add ammonia solution to a solution containing hexaaquacopper(II) ions, [Cu(H 2 O) 6] 2+, four of the water molecules are eventually replaced by ammonia molecules to give [Cu(NH 3) 4 (H 2 O) 2] 2+.This can be written as an equilibrium reaction to show the … View solution Justify that the reaction 2 C 2 O ( s ) + C u 2 S ( s ) → 6 C u ( s ) + S O 2 ( g ) is a redox reaction. Since no copper is added or removed between Reactions A and E, and since each reaction nearly goes to … Cu (s) + ZnSO4 (aq) This series of reactions begins and ends with copper metal. Replacing aqua ligands with ammine ligands. Identify the oxidizing and reducing agents in the equation. To make the oxidation reaction, simply reverse the reduction reaction and change the sign on the E 1/2 value. Reaction stoichiometry could be computed for a balanced equation. These tables, by convention, contain the half-cell potentials for reduction. identify the species oxidized , reduced , which acts s oxidation and which act as reductant. {eq}\rm CuO + H_2 \to Cu + H_2O {/eq} Now add reaction 3 to this one, etc. M n O 4 − ( a q ) + H 2 O 2 ( a q ) → View solution Which reaction does not represent auto redox or disproportionation reaction? Copper(II) is commonly found as the blue hydrated ion, \(\ce{[Cu(H2O)4]^{2+}}\). Balance the reaction of Cu + HNO3 = Cu(NO3)2 + NO + H2O using this chemical equation balancer! Determine what is oxidized and what is reduced. If you do not know what products are enter reagents only and click 'Balance'. Cu(OH)2 (s) + NaNO3 (aq) C. Cu(OH)2 (s) ! 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