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9. Assign oxidation number to each element, then classify each of the following unbalanced half-reactions as either an oxidation or a reduction: a. NO, (aq) → NO(g) b. Zn(s) → Zn²(aq) c. Ti (aq) →TiO;(s)

9. Assign oxidation number to each element, then classify each of the following unbalanced half-reactions as either an oxidation or a reduction: a. NO, (aq) → NO(g) b. Zn(s) → Zn²(aq) c. Ti (aq) →TiO;(s)

Chemistry
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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9. Assign oxidation number to each element, then classify each of the following unbalanced half-reactions as either an oxidation or a reduction: a. NO, (aq) → NO(g) b. Zn(s) → Zn²(aq) c. Ti (aq) → TiO₂ (s) d. Sn(aq) → Sn²*(aq) 10. Balance the half-reactions in the previous problem, assuming they occur in acidic solution 11. Balance the half-reactions in the previous problem, assuming they occur in basic solution
Transcribed Image Text:9. Assign oxidation number to each element, then classify each of the following unbalanced half-reactions as either an oxidation or a reduction: a. NO, (aq) → NO(g) b. Zn(s) → Zn²(aq) c. Ti (aq) → TiO₂ (s) d. Sn(aq) → Sn²*(aq) 10. Balance the half-reactions in the previous problem, assuming they occur in acidic solution 11. Balance the half-reactions in the previous problem, assuming they occur in basic solution
D. Standard Electrode Potentials at 25 °C E'(V) 2.87 2.08 1.98 1.82 1.78 1.69 Half-Reaction F₂(g) +2 e 2 F (aq) O(g) + 2 H(aq) + 2 e O₂(g) + H₂(1) Ag² (aq) +eAg (aq) Co³(aq) + e Có (a) HyOz{ag) + 2 H (aq) + 2e 2 H, PbO₂ (s) + 4 H*(aq) + SO, aq) + 2 e PbSO4(s) + 2 H₂O() MnO₂ (aq) + 4 H (aq) + 3 e 2 HCIO(aq) + 2 H(aq) + 2 e MnO₂ (aq) + 8 H'(aq) + 5 e Au (aq) + 3 e Au(s) 2 BrO₂ (aq) + 12 H(aq) + 10 e Br₂(0)+ 6 H₂O() 1.48 PbO₂ (s) + 4 H(aq) + 2 e 1.46 1.36 Pb²+ (aq) + 2 H₂O(0) Cl₂(g) +2 e 2 Cl(aq) MnO₂(s) + 2 H₂O(l) 1.68 ·Cl₂(g) + 2 H₂O(l) 1.61 Mn2(aq) + 4H₂O() 1.51 1.50 Half-Reaction Cr₂O, (aq) + 14 H(aq) + 6 e 2 Cr³(aq) + 7 H₂O(n) O₂(g) + 4 H (aq) + 4 e 2 H₂O(1) MnO₂(s) + 4 H(aq) + 2 e 10₂ (aq) + 6 H(aq) + 5 e 2 Br (ag) Br₂(0)+2 e AuCl(aq) + 3 e Au(s) + 4 Cl(aq) VO₂ (aq) + 2 H(aq) + e HNO₂(aq) + H(aq) + e NO₂ (aq) + 4 H(aq) + 3 e CIO₂(g) + e →CIO₂ (aq) 2 Hg²+ (aq) + 2 e 2 Hg₂² (aq) Ag" (aq) + e- Ag(s) Hg(aq) + 2 e 2 Hg() - - Mn²(aq) + 2 H₂O(l) • } b(aq) + 3H2O( VO² (aq) + H₂O() NO(g) + 2 H₂O(0) NO(g) + 2 H₂O(1) E° (V) 1.33 1.23 1.21 1.20 1.09 1.00 1.00 0.98 0.96 0.95 0.92 0.80 0.80
Transcribed Image Text:D. Standard Electrode Potentials at 25 °C E'(V) 2.87 2.08 1.98 1.82 1.78 1.69 Half-Reaction F₂(g) +2 e 2 F (aq) O(g) + 2 H(aq) + 2 e O₂(g) + H₂(1) Ag² (aq) +eAg (aq) Co³(aq) + e Có (a) HyOz{ag) + 2 H (aq) + 2e 2 H, PbO₂ (s) + 4 H*(aq) + SO, aq) + 2 e PbSO4(s) + 2 H₂O() MnO₂ (aq) + 4 H (aq) + 3 e 2 HCIO(aq) + 2 H(aq) + 2 e MnO₂ (aq) + 8 H'(aq) + 5 e Au (aq) + 3 e Au(s) 2 BrO₂ (aq) + 12 H(aq) + 10 e Br₂(0)+ 6 H₂O() 1.48 PbO₂ (s) + 4 H(aq) + 2 e 1.46 1.36 Pb²+ (aq) + 2 H₂O(0) Cl₂(g) +2 e 2 Cl(aq) MnO₂(s) + 2 H₂O(l) 1.68 ·Cl₂(g) + 2 H₂O(l) 1.61 Mn2(aq) + 4H₂O() 1.51 1.50 Half-Reaction Cr₂O, (aq) + 14 H(aq) + 6 e 2 Cr³(aq) + 7 H₂O(n) O₂(g) + 4 H (aq) + 4 e 2 H₂O(1) MnO₂(s) + 4 H(aq) + 2 e 10₂ (aq) + 6 H(aq) + 5 e 2 Br (ag) Br₂(0)+2 e AuCl(aq) + 3 e Au(s) + 4 Cl(aq) VO₂ (aq) + 2 H(aq) + e HNO₂(aq) + H(aq) + e NO₂ (aq) + 4 H(aq) + 3 e CIO₂(g) + e →CIO₂ (aq) 2 Hg²+ (aq) + 2 e 2 Hg₂² (aq) Ag" (aq) + e- Ag(s) Hg(aq) + 2 e 2 Hg() - - Mn²(aq) + 2 H₂O(l) • } b(aq) + 3H2O( VO² (aq) + H₂O() NO(g) + 2 H₂O(0) NO(g) + 2 H₂O(1) E° (V) 1.33 1.23 1.21 1.20 1.09 1.00 1.00 0.98 0.96 0.95 0.92 0.80 0.80
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