Ozone is a powerful oxidizing agent. Using ozone as the oxidant, write equations to represent oxidation of 

(a) Br^–(aq) to BrO^–(aq) (hypobromite); 

(b) NO(g) to NO₂(g); 

(c) Fe²⁺(aq) to Fe³⁺(aq) in acidic solution;

(d) Ag(s) to AgO(s); 

(e) [Fe(CN)₆]^4– to [Fe(CN)₆]^3– in basic solution. The half-equations for the reduction of O₃ in acidic and basic solutions are given in Table D.4 of Appendix D.

Table D.4

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TABLE D.4 Standard Electrode (Reduction) Potentials at 25 °Ca Reduction Half-Reaction F2(g) + 2 e 2 F (aq) OF2(g) + 2 H¹ (aq) + 4e¯ O3(g) + 2 H¹(aq) + 2 e H2O(1) + 2F (aq) O₂(g) + H₂O(1) S₂O²(aq) +2e= 2 SO4²-(aq) Ag²¹(aq) + 2e¯ — Ag†(aq) Co³ (aq) +e Co²+ (aq) H,O2(aq) + 2H*(aq)+2e <2 H,O(1) Ce3+ (aq) Ce4+ (aq) + e MnO4 (aq) + 4H+ (aq) + 3 e MnO₂(s) + 2 H₂0 (1) PbO₂(s) + SO₂²¯(aq) + 4 H*(aq) + 2 e¯ — PbSO4(s) + 2 H₂O(1) Mn³+ (aq) + e Mn²+ (aq) Au³+(aq) + 3e Au(s) MnO4 (aq) + 8 H(aq) + 5 e Mn²+ (aq) + 4 H₂O(1) 2 BrO3 (aq) + 12 H(aq) + 10 e = Br₂(1) + 6 H₂O(1) PbO₂(s) + 4H+ (aq) + 2e Pb²+(aq) + 2 H₂O(1) Cl¯(aq) + 2 H₂O(1) CIO3 (aq) + 6 H¹(aq) + 6 e¯ ⇒ Au¹(aq) Au³+(aq) + 2 e Cell Notation F|F₂ | Pt F, H* | OF₂ | Pt H+, H₂O|03, O₂ | Pt SO4²-, S₂08² | Pt Ag+, Ag²+ | Pt Co²+, Co²+ | Pt H₂O₂, H+ | Pt Ce³+, Ce+|Pt MnO₂ | MnO4, H+ | Pt PbSO4, PbO₂ | SO4²-, H+ | Pt Mn²+, Mn³+ | Pt Au³+ | Au Mn²+, MnO4 | Pt BrO3, H | Br₂ | Pt Pb²+, H | PbO₂ | Pt CI, CIO3, H+ | Pt Au*, Au³+|Pt Standard Reduction Potential, V +2.866 +2.1 +2.075 +2.01 +1.98 +1.92 +1.763 +1.72 +1.70 +1.69 +1.54 +1.52 +1.51 +1.478 +1.455 +1.450 +1.36