Complete the following chemical reaction and classify into (a) hydrolysis, (b) redox and (c) hydration reactions. 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 … To make the oxidation reaction, simply reverse the reduction reaction and change the sign on the E 1/2 value. {eq}\rm CuO + H_2 \to Cu + H_2O {/eq} Cu (s) + ZnSO4 (aq) This series of reactions begins and ends with copper metal. Which reaction does not represent auto redox or disproportionation reaction? CuO (s) + H2O (l) D. CuO (s) + H2SO4 (aq) ! identify the species oxidized , reduced , which acts s oxidation and which act as reductant. Reaction stoichiometry could be computed for a balanced equation. CuSO4 (aq) + H2O (l) E. CuSO4 (aq) + Zn (s) ! The net reaction for these two reactions is: CuCO3 + CuCl2 + H2O -> CuCl2 + CO2 + Cu(OH)2. Balance the reaction of Cu + HNO3 = Cu(NO3)2 + NO + H2O using this chemical equation balancer! Since no copper is added or removed between Reactions A and E, and since each reaction nearly goes to … Replacing aqua ligands with ammine ligands. If you do not know what products are enter reagents only and click 'Balance'. Now add reaction 3 to this one, etc. These tables, by convention, contain the half-cell potentials for reduction. Cu(OH)2 (s) + NaNO3 (aq) C. Cu(OH)2 (s) ! Balanced half-reactions are well tabulated in handbooks and on the web in a 'Tables of standard electrode potentials'. oxidation-reduction AND recomposition b.) M n O 4 − ( a q ) + H 2 O 2 ( a q ) → View solution 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, \(\ce{[Cu(H2O)4]^{2+}}\). CuCO3 + 2NaCl + CuCl2 + 2H2O -> CuCl2 + H2O + CO2 + Cu(OH)2 + 2NaCl. decomposition AND acid-base c.) oxidation-reduction AND oxidation-reduction d.) acid-base AND oxidation-reduction Identify the oxidizing and reducing agents in the equation. 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. 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). Aqueous Ammonia. Learn vocabulary, terms, and more with flashcards, games, and other study tools. Determine what is oxidized and what is reduced. Copper(II) ion reacts with stoichiometric quantities of aqueous ammonia to precipitate light blue Cu(OH)2. … Start studying [Cu(H2O)6]2+ reactions. 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. 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