For the following reactions, determine the species being oxidized or reduced, the balanced half reactions, and the balanced equation.
Al(s)+Cu^2+(aq) -> Al^3+(aq)+CU(s)
For the following reactions, determine the species being oxidized or reduced, the balanced half reactions, and...
For the following reactions, determine the species being oxidized or reduced, the balanced half reactions, and the balanced equation. HCOOH+MnO4^- -> CO2+Mn^2+ in acidic solution
1. Identify the species being oxidized and reduced in each of the following reactions, and determine the number of electrons (in mol) involved in the reaction: a. Crt + Sn4+ -> Cr3+ + Sn2+ b. 3 Hg2+ + 2 Fe (s) -> 3 Hg2+ 2 Fe3+ c. 2 As (s) + 3 Cl2 (8) 2 AsCl3
4. In each of the following reactions, identify the elements being oxidized or reduced, a) 4 Fe (s) + 3 O2(g) 2 FeO3 (5) (Oxygen is in its natural state.) Element being oxidized: Element being reduced: b) CuCl2 (aq) + Zn (s) → ZnCl2 (aq) + Cu (s) (Zinc and Copper are in their natural states.) Element being oxidized: Element being reduced: 21
7. Balance the following reactions and identify the species that have been oxidized and the species that have been reduced Species reduced Species oxidized I lon) Clergo Reaction Cl2(g) + (aq) WO2(8) FH2(g) Ca(s) FH20(1) 4 Al(s) +(8) → 12(8) CI" (aq) → W(8) +H20(1) H2(g) + Ca(OH)2(s) A1,0,($) 8. Assuming that the following redox reactions are found to occur spontaneously, identify the more active metal in each reaction. More active metal Reaction 2Li(s) + Cu2+ (aq) — 2Li* (aq)...
5) Determine which element is oxidized and which element is reduced in the following redox reactions. (4) Fe2O3 + CO ® Fe + CO2 Element oxidized ____________________ Element reduced _________________ Cr2O72- + H2C2O4 ® Cr3+ + CO2 Element oxidized ____________________ Element reduced ___________________ 6) Determine the balanced molecular, ionic and net ionic equations for the following single displacement (replacement) reaction. (9) (ME) Al(s) + HCl(aq) ® (IE) (NIE)
1. Identify the anode, the cathode, the reduced species and the oxidized species for the following electrochemical cells. Write the half reactions for the anode and cathode, the overall reaction. Calculate the total cell potential. a) Fe (8)| Fe (aq) (0.2 M) || Ni” (aq) (0.1 M) | Ni(s) b) Zn (s) | Zn? (aq) (1.0 x 10' M)||Cl(aq)(0.3 M) CI, (g) (0.100 bar) Pt (S) c) Pb (s) Pb2(aq) (1.0 x 10ʻM) || Cu (aq) (1.0 x 10M) Cu...
3. Balance the following reactions and identify the species that have been oxidized and the species that have been reduced: Clz (g) + l'(aq) → 12 (s) + Cl(aq): - Al (s) + O2(g) → Al2O3 (s): -- 3/3 Ca (s) + H20 (1) ► H2 (9) + Ca (OH)2 (s): --- WO2 (s) + Hz (g) → W (s) + H2O (): -
Balance the equation and identify the species being oxidized and reduced. ___ Na (s) + __-H20 (1) ►_NaOH (aq) + _H2 (g)
Part B: Basic Conditions Using the half-reaction method, balance the following redox reactions under basic conditions and identify which of the reactants is being reduced and which is being oxidized. 7. SO32- + Cu(OH)2 → S022- + Cu(OH) a. Oxidized: b. Reduced: c. Balanced Equation: 8. O2 + Mn(OH)2 → MnO2 a. Oxidized: b. Reduced: c. Balanced Equation: 9. NO;' + H2 → NO a. Oxidized: b. Reduced: c. Balanced Equation:
For each reaction below, balance the following reactions and indicate the species that has been oxidized and the species that has been reduced: Copy and paste the table below, to complete the chart. For each reaction below, balance the following reactions and indicate the species that has been oxidized and the species that has been reduced: Copy and paste the table below, to complete the chart. Reaction Species Oxidized Species Reduced Cl2 (g) + (aq) → 12 (s) + Cl(aq)...