CHEM105 1nd Edition Lecture 10 Outline of Last Lecture • Solubility rules• precipitation reactions Outline of Current Lecture • Cont. Oxidation-Reduction Reactions: Electron Transfer • Cosidering Electron Transfer in Redox Reactions • Balancing Redox Reactions Using Half-Reactions Current Lecture• Na(s) +Cl2(g) ------> NaCl(s)Na os Oxidized (0 , +1) Reducing agent: NaCl is reduced ( 0 , -1) Oxidizing agent: Cl2-Redox reactions must be balanced for number of electrons transferred as well as the number and types of atoms.• Cu(s) + Ag+(aq) ------> Cu2+(aq) + Ag(s)Cu(s) + 2AgNO3(aq) -----> Cu(NO3)2(aq) + 2Ag(s)• C12H22O11(s) + KClO3(l) -----> CO2(g) + H2O(g) + KCl(s)C12H22O11(s) + 8KClO3(l) -----> 12CO2(g) +11H2O(g) +8KCl(s) C is Oxidized Cl is reduced • 14KMnO4(s) + 4C3H8O3(l) ------> 7Mn2O3(s) + 5CO2(g) + 16H2O(g) + K2CO3(s)C is Oxidized Mn is reduced • Fe2O3(s) + Al(s) ------> Al2O3(s) + Fe(l) Fe2O3(s) + 2Al(s) ------> Al2O3(s) + 2Fe(l) - The method of half reactions • H2SO4(aq) + CH2O(aq) -----> H2S(aq) +CO2(g) +H2O(l)In acidic solution H+(aq) amd H2O(l) to balance H and OOxidation half reaction:CH2O(aq) +H2O(l) -------> CO2(g) + 4H+(aq) +4e-Reduction Half reaction: H2SO4(aq) +8H(aq) +8e- ----> H2S(aq) +
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