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Balancing Redox Reactions

Balancing Redox Reactions. AlI 3. I 2 (s) + Al (s) . 3. 2. 2. +7. +3. +2. +4. MnO 4 - + C 2 O 4 2-  Mn 2+ + CO 2. MnO 4 - + C 2 O 4 2-  Mn 2+ + CO 2. 2. 2 O 2. 4 H 2 O. HELP. 4 OH -. MnO 4 -.  Mn 2+. MnO 4 -.  Mn 2+. MnO 4 - + C 2 O 4 2-  Mn 2+ + CO 2.

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Balancing Redox Reactions

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  1. Balancing Redox Reactions AlI3 I2 (s) + Al (s)  3 2 2 +7 +3 +2 +4 MnO4- + C2O42- Mn2+ + CO2 MnO4- + C2O42- Mn2+ + CO2 2 2 O2 4 H2O HELP 4 OH-

  2. MnO4-  Mn2+ MnO4-  Mn2+ MnO4- + C2O42- Mn2+ + CO2 1. Break it into two half-reactions MnO4-  Mn2+  CO2 C2O42- 2. Balance redox active species 3. Balance oxygen using H2O + H2O 4

  3. MnO4-  Mn2+ MnO4- MnO4-  Mn2+  Mn2+ + H2O + H2O 4 4 8 H+ + +7 +2 4. Balance hydrogen using H+ 8 H+ + 5. Balance charge using e- 5 e- + This is a balanced half-reaction electrons are a ________ reactant MnO4- is _______ electrons gaining MnO4- is being _______ reduced Where do the e- come from?

  4. C2O42-  CO2 C2O42- C2O42- C2O42- C2O42-  CO2  CO2  CO2  CO2 2 2 2 2. Balance redox active species 2 3. Balance oxygen using H2O 4. Balance hydrogen using H+ 5. Balance charge using e- + e- 2

  5. +3 +4 C2O42-  CO2 2 + e- 2 This is a balanced half-reaction electrons are a ________ product C2O42- is _______ electrons losing C2O42- is being _______ oxidized Now combine the two half-reactions

  6. ( ) ( ) + e- 2 C2O42-  CO2 2 MnO4-  Mn2+ + H2O 4 8 H+ + 2 5 e- + 5  16H+ + 8H2O + 10CO2 + 2MnO4- + 5C2O42- 2Mn2+ stoichiometry additional product, H2O additional reactant, acid

  7. Ag+ (aq)  Ag (s) + C6H12O7 (aq) + C6H12O6 (aq)  Ag+ Ag (s) C6H12O6  C6H12O7

  8. Ag+ + C6H12O6 Ag (s) + C6H12O7  Ag+ + e- Ag (s) balance mass balance oxygen H2O balance hydrogen H+ balance charge e-

  9. H2O + C6H12O6  C6H12O7 + H+ 2 + e- 2 balance mass balance oxygen H2O balance hydrogen H+ balance charge e-

  10. ( ) + H+ 2 H2O + C6H12O6  C6H12O7 + H+ 2 + e- 2  2 Ag+ + e- Ag (s) H2O + C6H12O6 + 2Ag+  C6H12O7 + 2Ag (s) Ag+ reduced Ag+ oxidizing agent C6H12O6 oxidized C6H12O6 reducing agent C C + 3+

  11. ( ) 2 H2O 2 2 OH- OH- +2 + H2O H2O H2O + C6H12O6  C6H12O7 + H+ 2 + e- 2  2 Ag+ + e- Ag (s) H2O + C6H12O6 + 2Ag+  C6H12O7 + H+ 2 + 2Ag (s) 2 OH- 2 OH- This reaction takes place in a basic solution OH- 1 +H2O+ C6H12O6 +2Ag+  C6H12O7 +2Ag (s) + C6H12O6 +2Ag+  C6H12O7 +2Ag (s)

  12. CNO-  MnO2 CN-  MnO4- CNO-  MnO2 CN-  MnO4-  CNO- (aq) + MnO2 (s) CN-(aq) + MnO4- (aq) separate half-reactions CNO-  MnO2 CN-  MnO4- balance mass balance oxygen H2O+ + H2O 2

  13. CNO-  MnO2 H2O+ CN-  MnO4- + H2O 2 ( ) CNO- H2O+ CN-  + H+ 2 ( ) 4  MnO2 MnO4- + H+ + H2O 2 CNO-  MnO2 H2O+ CN-  MnO4- + H2O 2 balance hydrogen + H+ 2 + H+ 4 balance charge 3 + e- 2 2 3 e-+  3 CN- +2 MnO4- + 2 H+ 3 CNO- + 2 MnO2 + H2O

  14. 3 CN- +2 MnO4- + 2 H+ 3 CNO- + 2 MnO2 + H2O OH- 2 OH- 2 add OH- make the solutions basic 3 CN- + 2 MnO4- +H2O  3 CNO- + 2 MnO2 + 2 OH-

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