(a) Use the data in Appendix 2B to decide which of ozone and fluorine is the stronger oxidizing agent in water.

(b) Does your answer depend on whether the reaction is carried out in acidic or basic solution?

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2B STANDARD POTENTIALS AT 25 °C Potentials in Electrochemical Order Reduction half-reaction Strongly oxidizing H₂XeO6 + 2 H+ + 2 e → XeO3 + 3 H₂O F₂2 e 2 F™ 03 + 2 H+ + 2 e → O₂ + H₂O S₂O8² +2e →2 SO4²- Ag+ + e → Agt Cơ từ cot H₂O₂+ 2 H+ + 2e →2 H₂O Aue Au Pb+ + 2 e Pb²+ → 2 HClO + 2 H+ +2e →Ch₂ + 2 H₂O Ce++eCe³+ 2 HBrO + 2 H+ + 2 e MnO4 + 8 H+ + 5e Mn³+ + e→→Mn²+ Au³+ + 3 e Au Cl₂ +2 e 2 Cl Cr₂O7² + 14 H+ + 6 e 03 + H₂O + 2 e O₂ + 4 H+ + 4e MnO₂ + 4H+ + 2e clo + 2H+ + 2e Pt²+ + 2 e →→ Pt Br₂ + 2 e2 Br¯ Pu²+ + e→Pu³+ 3+ → Br2 + 2 H₂O →Mn²+ + 4 H₂0 2 Cr³+ + 7 H₂O 02 + 2 OH™ 2 H₂O →Mn²+ + 2 H₂O →ClO3 + H₂O NO3 + 4 H+ + 3 e→NO + 2 H₂O 2+ 2 Hg²+ + 2e → Hg₂²+ clo + H₂O +2e →Cl + 2 OH™ Hg²+ + 2 e → Hg Eº/V +3.0 +2.87 +2.07 +2.05 +1.98 +1.81 +1.78 +1.69 +1.67 +1.63 +1.61 +1.60 +1.51 +1.51 +1.40 +1.36 +1.33 +1.24 +1.23 +1.23 +1.23 +1.20 +1.09 +0.97 +0.96 +0.92 +0.89 +0.85 Reduction half-reaction NO3 + H₂O + 2e →NO₂+ 2 OH™ Ti¹+ + e → Ti³+ 2 H + 2e → H₂ Fe³+ + 3 e Fe O₂ + H₂O + 2 e → HO₂ + OH™ Pb²+ + 2e →→ Pb In+ + e → In Sn²+ + 2 e Sn Ag + I Ni Agi + e → Ni²+ + 2 e V³+ + e → V²+ Co²+ +2 e In³+ + 3 e Tl+ + e → TI Co In PbSO4 + 2 e Ti³+ + e → Ti²+ In²+ + e → In+ Cd²+ + 2e → Cd Cr³+ +eCr²+ Fe²+ + 2e → Fe In +2 e S+ 2e → S²- Pb + SO4²- + In Gae Ga O₂ + e → 0₂ U4+ + e → Se+ 2 e Cr³+ +eIn2+ Se²- + 3e → Cr Eº/V +0.01 0.00 0, by definition -0.04 -0.08 -0.13 -0.14 -0.14 -0.15 -0.23 -0.26 -0.28 -0.34 -0.34 -0.36 -0.37 -0.40 -0.40 -0.41 -0.44 -0.44 -0.48 -0.49 -0.53 -0.56 -0.61 -0.67 -0.74