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