Identify if the following reactions are redox reaction or not. If they are redox reactions. specify...
Redox Equations Which of the following reactions are redox reactions? Identify the substance oxidized, the substance reduced, the oxidizing agent, the reducing agent. 1.2 Mg(s) + O2(g) → 2 MgO (s) 2. H SO. (aq) + Al(OH) (aq) → Al(SO.) (aq) + H,O (1) 3. 2 Na (s) + H2O (1) ► 2 NaOH(aq) + H2(g) 4. Cao (s) + CO2(g) → Caco, (s) 5. AgNO, (aq) + NaCl (aq) ► AgCl(s) + NaNO, (aq) Identify the substance oxidized, the...
Identify whether the reaction is a redox reaction. If it is, determine which species is oxidized and which is reduced. 2Fe^3+(aq) + 3S^2- (aq) rightarrow Fe_2S_3(s) 2FeCl_3(aq) + 3Co(s) rightarrow 2Fe(s) + 3CoCl_2(aq) 2NH_4Cl(aq) + F_2(g) rightarrow 2NH_4F(aq) + Cl_2(aq) H^+(aq) + OH^-(aq) rightarrow H_2O(I) 2HNO_3(aq) + Zn(s) rightarrow Zn(NO3)2(aq) + H_2(g) 2H_2O(I) + 2K(s) rightarrow 2KOH(aq) + H_2(g) 2.
15) Draw the shapes of the following orbitals; (a) s orbital(b) 2p, (c) 2p d) 2p 16) Identify each of the following reactions as being a neutralization, precipitation, or Redox reaction. (a) Fe203 (s) + 3CO (g) → 2Fe (s) + 3CO2 (g) (b) Na:S04 (aq) + Hig(NOJ2(aq) → HgSO4 (s) + 2NaNO3 (aa) (c) CsOH (aq) + HCio. (aq) → Cs. (aq) + 2H20 (I) + CIO.(aq) (d) Mg(NO3)2 (g) + Na:S (aq) → MgS (s) + 2NaNO3 (aq)...
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:
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)...
1. (a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) NO3- (aq) + N2O (g) (ii) (acid solution) Fe042- (aq) + Fe3+ (aq) (iii) (base solution) Fe203 () → Fe(OH)2 (S) (iv) (base solution) Cu20 (s) + Cu(OH)2 (S) (b) Which of the above equations are oxidation half-reactions? (c) Give the formulas of the reactants that become oxidized in the course of the reaction.
4. (6 pts.) Oxidation-Reduction Reactions: write out two ways you can identify the species that has been oxidized in a redox reaction: b. Identify the element reduced and the element oxidized in the following oxidation- reduction reactions. Fe(s) + CuCl2(aq) FeCl2(aq) + Cu(s) Element Oxidized: Element Reduced: C(s) + O2(g) → C02(g) Element Oxidized: Element Reduced:
1. Determine if each of the following reactions is a redox reaction, or is not a redox reaction. a. C4H8 (g) + O2 + H20 (g) + CO2 (g) b. HCl (aq) + NaOH (aq) → H20 (1) + NaCl (aq) c. Fe2O3 + H2 → Fe + H2O d. Cu (s) + HNO3 (aq) → Cu(NO3)2 (aq) + NO2 (g) + H20 (1) e. CzHe(g) + 5 O2 (g) → 3 CO2 (g) + 4 H20 (g)
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)...
For each of the following balanced redox reactions, identify which elements get oxidized and reduced. Also, ldentify the oxidant and the reductant. 1) 2Cr20 (aq)+3CH,OH(aq) 16H (aq) 3HCO,H(aq)+4Cr(aq)+ 11H20 (1) 2) 2NO -(aq) + H2S(g) + 2H+(aq) →2NO2(g) + S(g) +2H2O (l)