Bromine is obtained from brine wells. The process involves treating water containing bromide ion with Cl₂ and extracting the Br₂ from the solution using an organic solvent. Write a balanced equation for the reaction of Cl₂ and Br⁻. What are the oxidizing and reducing agents in this reaction? Using the table of standard reduction potentials (Appendix M), verify that this is a product-favored reaction at equilibrium.

Data given in Appendix M

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Standard Reduction Potentials in Aqueous Solution TABLE 21 at 25 °C Acidic Solution F₂(g) + 2 e 2 F-(aq) Co² (aq) + e- →→Co²+ (aq) Pb²+ (aq) + 2 e - Pb²+ (aq) H,Oz(aq) + 2 H+(aq) + 2 e — 2 H,O NiO₂ (s) + 4 H+ (aq) + 2 e Ni²+ (aq) + 2 H₂O PbO₂ (s) + SO4² (aq) + 4 H*(aq) + 2 e PbSO4(s) + 2 H₂O - Au (aq) + e→→→→ Au(s) Ce (aq) + e. - 2 HCIO(aq) + 2 H+ (aq) + 2 e Ce³+ (aq) NaBiO;(s) + 6 H*(aq) + 2 e → MnO₂ (aq) + 8 H+ (aq) + 5 e Au (aq) + 3 e →→ Au(s) CIO₂ (aq) + 6 H+(aq) + 5 e- → + Cl₂(g) + 3 H₂O BrO₂ (aq) + 6 H+ (aq) + 6 e Br(aq) + 3 H₂0 → 2 Cl-(aq) Cl₂(g) + 2 e Cr₂O7²-(aq) + 14 H+ (aq) + 6 e → N₂H5+ (aq) + 3 H+ (aq) + 2 e2 NH₂ + (aq) MnO₂ (s) + 4 H+ (aq) + 2 e-- → Mn²+ (aq) + 2 H₂O → ► Cl₂(g) + 2 H₂O → Br₂(e) + 2 e→→ 2 Br (aq) - AuCl(aq) + 3 e - O₂(g) + 4 H+ (aq) + 4 e → 2 H₂O - Pt2+(aq) + 2 e→→→→ Pt(s) 10₁ (aq) + 6 H (aq) + 5 e- CIO, (aq) + 2 H+ (aq) + 2 e - Bi³+(aq) + Na (aq) + 3 H₂O Mn²+ (aq) + 4 H₂O 2 Cr³+ (aq) + 7 H₂O •Ỉ I,(aq) + 3 H,O CIO₂ (aq) + H₂O Au(s) + 4 CI-(aq) Standard Reduction Potential E° (volts) 2.87 1.82 1.8 1.77 1.7 1.685 1.68 1.63 1.61 -1.6 1.51 1.50 1.47 1.44 1.36 1.33 1.24 1.23 1.229 1.2 1.195 1.19 1.08 1.00