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Electrochemistry Lesson 5 Balancing Half Reactions

Electrochemistry Lesson 5 Balancing Half Reactions. Core Concepts What is reduced and oxidized? What gains or loses electrons? What are the oxidizing and reducing agents? 2H + + As 2 O 3 + 2NO 3 - + 2H 2 O  2H 3 AsO 4 + N 2 O 3. Core Concepts

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Electrochemistry Lesson 5 Balancing Half Reactions

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  1. Electrochemistry Lesson 5 Balancing Half Reactions

  2. Core Concepts What is reduced and oxidized? What gains or loses electrons? What are the oxidizing and reducing agents? 2H+ + As2O3 + 2NO3- + 2H2O  2H3AsO4 + N2O3

  3. Core Concepts What is reduced and oxidized? What gains or loses electrons? What are the oxidizing and reducing agents? 2H+ + As2O3 + 2NO3- + 2H2O  2H3AsO4 + N2O3 You must use oxidation #'s

  4. Core Concepts What is reduced and oxidized? What gains or loses electrons? What are the oxidizing and reducing agents? +3 +5 +5 +3 2H+ + As2O3 + 2NO3- + 2H2O  2H3AsO4 + N2O3

  5. Core Concepts What is reduced and oxidized? What gains or loses electrons? What are the oxidizing and reducing agents? +3 +5 +5 +3 2H+ + As2O3 + 2NO3- + 2H2O  2H3AsO4 + N2O3 oxidized reduced

  6. Core Concepts What is reduced and oxidized? What gains or loses electrons? What are the oxidizing and reducing agents? +3 +5 +5 +3 2H+ + As2O3 + 2NO3- + 2H2O  2H3AsO4 + N2O3 oxidized reduced loses e's gains e's

  7. Core Concepts What is reduced and oxidized? What gains or loses electrons? What are the oxidizing and reducing agents? +3 +5 +5 +3 2H+ + As2O3 + 2NO3- + 2H2O  2H3AsO4 + N2O3 oxidized reduced loses e's gains e's red agent ox agent

  8. PdCl2 reacts with Mn but not Br-. Write the spontaneous reaction.

  9. PdCl2 reacts with Mn but not Br-. Write the spontaneous reaction.

  10. PdCl2 reacts with Mn but not Br-. Write the spontaneous reaction. Pd2+ + Mn(s) Pd(s) + Mn2+

  11. PdCl2 reacts with Mn but not Br-. Write the spontaneous reaction. Pd2+ + Mn(s) Pd(s) + Mn2+ Rank the oxidizing agents in decreasing strength.

  12. PdCl2 reacts with Mn but not Br-. Write the spontaneous reaction. Pd2+ + Mn(s) Pd(s) + Mn2+ Rank the oxidizing agents in decreasing strength. Pd2+

  13. PdCl2 reacts with Mn but not Br-. Write the spontaneous reaction. Pd2+ + Mn(s) Pd(s) + Mn2+ Rank the oxidizing agents in decreasing strength. Br- Pd2+ Mn

  14. PdCl2 reacts with Mn but not Br-. Write the spontaneous reaction. Pd2+ + Mn(s) Pd(s) + Mn2+ Rank the oxidizing agents in decreasing strength. Br2 Br- Pd2+ Mn

  15. PdCl2 reacts with Mn but not Br-. Write the spontaneous reaction. Pd2+ + Mn(s) Pd(s) + Mn2+ Rank the oxidizing agents in decreasing strength. Br2 Br- Pd2+ Mn2+ Mn

  16. PdCl2 reacts with Mn but not Br-. Write the spontaneous reaction. Pd2+ + Mn(s) Pd(s) + Mn2+ Rank the oxidizing agents in decreasing strength. Br2 Br- Pd2+ Pd Mn2+ Mn

  17. PdCl2 reacts with Mn but not Br-. Write the spontaneous reaction. Pd2+ + Mn(s) Pd(s) + Mn2+ Rank the oxidizing agents in decreasing strength. Br2 Br- Pd2+ Pd Mn2+ Mn Br2 Pd2+ Mn2+

  18. PdCl2 reacts with Mn but not Br-. Write the spontaneous reaction. Pd2+ + Mn(s) Pd(s) + Mn2+ Rank the reducing agents in decreasing strength. Br2 Br- Pd2+ Pd Mn2+ Mn

  19. PdCl2 reacts with Mn but not Br-. Write the spontaneous reaction. Pd2+ + Mn(s) Pd(s) + Mn2+ Rank the reducing agents in decreasing strength. Br2 Br- Pd2+ Pd Mn2+ Mn Mn Pd Br-

  20. Balancing Redox Half Reactions in Acid Solution

  21. Balancing Redox Half Reactions in Acid Solution Cr2O72-→ Cr3+

  22. Balancing Redox Half Reactions in Acid Solution Cr2O72-→ Cr3+ 1. Balance the central atom

  23. Balancing Redox Half Reactions in Acid Solution Cr2O72-→ Cr3+ 1. Balance the central atom

  24. Balancing Redox Half Reactions in Acid Solution Cr2O72-→ 2Cr3+ 1. Balance the central atom

  25. Balancing Redox Half Reactions in Acid Solution Cr2O72-→ 2Cr3+ 1. Balance the central atom 2. Balance O by adding H2O

  26. Balancing Redox Half Reactions in Acid Solution Cr2O72-→ 2Cr3+ + 7H2O 1. Balance the central atom 2. Balance O by adding H2O

  27. Balancing Redox Half Reactions in Acid Solution Cr2O72-→ 2Cr3+ + 7H2O 1.Balance the central atom 2.Balance O by adding H2O 3.Balance H by adding H+

  28. Balancing Redox Half Reactions in Acid Solution Cr2O72- + 14H+→ 2Cr3+ + 7H2O 1.Balance the central atom 2.Balance O by adding H2O 3.Balance H by adding H+

  29. Balancing Redox Half Reactions in Acid Solution Cr2O72- + 14H+→ 2Cr3+ + 7H2O 1.Balance the central atom 2.Balance O by adding H2O 3.Balance H by adding H+ 4. Balance the charge by adding electrons

  30. Balancing Redox Half Reactions in Acid Solution +12 Cr2O72-+ 14H+→ 2Cr3+ + 7H2O 1.Balance the central atom 2.Balance O by adding H2O 3.Balance H by adding H+ 4. Balance the charge by adding electrons

  31. Balancing Redox Half Reactions in Acid Solution +12 +6 Cr2O72-+ 14H+→ 2Cr3+ + 7H2O 1.Balance the central atom 2.Balance O by adding H2O 3.Balance H by adding H+ 4. Balance the charge by adding electrons

  32. Balancing Redox Half Reactions in Acid Solution most positive side +12 +6 6e- + Cr2O72- + 14H+→ 2Cr3+ + 7H2O 1.Balance the central atom 2.Balance O by adding H2O 3.Balance H by adding H+ 4. Balance the charge by adding electrons

  33. Balancing Redox Half Reactions in Acid Solution most positive side +12 +6 6e- + Cr2O72- + 14H+→ 2Cr3+ + 7H2O 1.Balance the central atom 2.Balance O by adding H2O 3.Balance H by adding H+ 4. Balance the charge by adding electrons 5. Check charge

  34. Balancing Redox Half Reactions in Acid Solution most positive side +6 +6 6e- + Cr2O72- + 14H+→ 2Cr3+ + 7H2O 1.Balance the central atom 2.Balance O by adding H2O 3.Balance H by adding H+ 4. Balance the charge by adding electrons 5. Check charge

  35. Balancing Redox Half Reactions in Acid Solution

  36. Balancing Redox Half Reactions in Acid Solution HV2O53-→ H2VO3+

  37. Balancing Redox Half Reactions in Acid Solution HV2O53-→ H2VO3+ 1. Balance the central atom

  38. Balancing Redox Half Reactions in Acid Solution HV2O53-→ 2H2VO3+ 1. Balance the central atom

  39. Balancing Redox Half Reactions in Acid Solution HV2O53-→ 2H2VO3+ 1. Balance the central atom 2. Balance O by adding H2O

  40. Balancing Redox Half Reactions in Acid Solution H2O + HV2O53-→ 2H2VO3+ 1. Balance the central atom 2. Balance O by adding H2O

  41. Balancing Redox Half Reactions in Acid Solution H2O + HV2O53-→ 2H2VO3+ 1.Balance the central atom 2.Balance O by adding H2O 3.Balance H by adding H+

  42. Balancing Redox Half Reactions in Acid Solution H2O + HV2O53- + H+→ 2H2VO3+ 1.Balance the central atom 2.Balance O by adding H2O 3.Balance H by adding H+

  43. Balancing Redox Half Reactions in Acid Solution H2O + HV2O53- + H+ → 2H2VO3+ 1.Balance the central atom 2.Balance O by adding H2O 3.Balance H by adding H+ 4. Balance the charge by adding electrons

  44. Balancing Redox Half Reactions in Acid Solution -2 H2O + HV2O53- + H+ → 2H2VO3+ 1.Balance the central atom 2.Balance O by adding H2O 3.Balance H by adding H+ 4. Balance the charge by adding electrons

  45. Balancing Redox Half Reactions in Acid Solution -2 +2 H2O + HV2O53- + H+ → 2H2VO3+ 1.Balance the central atom 2.Balance O by adding H2O 3.Balance H by adding H+ 4. Balance the charge by adding electrons

  46. Balancing Redox Half Reactions in Acid Solution most positive side -2 +2 H2O + HV2O53- + H+ → 2H2VO3+ 1.Balance the central atom 2.Balance O by adding H2O 3.Balance H by adding H+ 4. Balance the charge by adding electrons

  47. Balancing Redox Half Reactions in Acid Solution -2 +2 H2O + HV2O53- + H+ → 2H2VO3+ + 4e- 1.Balance the central atom 2.Balance O by adding H2O 3.Balance H by adding H+ 4. Balance the charge by adding electrons

  48. Balancing Redox Half Reactions in Acid Solution -2 +2 H2O + HV2O53- + H+ → 2H2VO3+ + 4e- 1.Balance the central atom 2.Balance O by adding H2O 3.Balance H by adding H+ 4. Balance the charge by adding electrons 5. Check charge

  49. Balancing Redox Half Reactions in Acid Solution -2 -2 H2O + HV2O53- + H+ → 2H2VO3+ + 4e- 1.Balance the central atom 2.Balance O by adding H2O 3.Balance H by adding H+ 4. Balance the charge by adding electrons 5. Check charge

  50. Balancing Redox Half Reactions in Acid Solution HBr2O72- → H2BrO2-

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