Which of the following statements about this ReDox reaction are correct?

1). For the following redox reaction, Identify half reactions, reduced element, oxidized element,......?

• oxidizing agent, and reducing agent. MnO4– (aq) + H2C2O4(aq) → Mn2+ (aq) + CO2(g) #2). Determine the cell notation for the redox reaction given below. 3Cl2(g) + 2 Fe(s) → 6 Cl– (aq) + 2 Fe3+(aq) #3). Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) 3Cl2(g) + 2 Fe(s) → 6 Cl– (aq) + 2 Fe3+(aq) Cl2(g) + 2 e– → 2 Cl– (aq) E° = +1.36 V Fe3+(aq) + 3 e– → Fe(s) E° = -0.04 V

• Answer:

  1). For the following redox reaction, Identify half reactions, reduced element, oxidized element, oxidizing agent, and reducing agent. MnO4– (aq) + H2C2O4(aq) → Mn2+ (aq) + CO2(g) +7 -2 ----------- +1 +3 -2 ---------- +2 ----------- +4 -2 MnO4-(aq) + 5e- ---------------> Mn2+(aq) [ Reduction reaction; oxidizing agent and Mn is the reduced element ] H2C2O4(aq) -------------> CO2(g) + e- [ Oxidation reaction; reducing agent and C is the oxidized element ] #2). Determine the cell notation for the redox reaction given below. 3Cl2(g) + 2 Fe(s) → 6 Cl– (aq) + 2 Fe3+(aq) -- 0 ----------- 0 ----------- -1 ------------- +3 2Fe(s) | 2Fe3+(s) || 3Cl2(g) | 6Cl-(aq) #3). Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) 3Cl2(g) + 2 Fe(s) → 6 Cl– (aq) + 2 Fe3+(aq) Cl2(g) + 2 e– → 2 Cl– (aq) E° = +1.36 V [ E*red = +1.36 V ] Fe3+(aq) + 3 e– → Fe(s) E° = -0.04 V [ E*ox = -E*red = +0.04 V ] E*cell = Eox + Ered = +1.36 + 0.04 = 1.40 V Bill