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

TABLE D.4 Standard Electrode (Reduction) Potentials at 25 Ca Reduction Half-Reaction F2(g) + 2 e 2 F (aq) OF2(g) + 2 H (aq) + 4e O3(g) + 2 H(aq) + 2 e H2O(1) + 2F (aq) O(g) + HO(1) SO(aq) +2e= 2 SO4-(aq) Ag(aq) + 2e Ag(aq) Co (aq) +e Co+ (aq) H,O2(aq) + 2H*(aq)+2e