Consider the following unbalanced redox reaction: a) Balance the reaction in acidic solution using smallest whole-number coefficients. A. Balance the reaction in acidic solution using smallest whole-number coefficients. Identify the anode and cathode half-reactions, and the oxidizing and reducing agents.
B. Using data found on the Useful Information page, calculate AGo for this reaction at 25cC. anode and cathode half-reactions, and the oxidizing and reducing agents.
C. Determine E cell for this reaction at 25°C.
Useful Information
Standard Reduction Potentials at 25 C E° (V)
H3As04 2H + 2 eHAsO2 2 H20 0.560
HAsO2+3 H+ + 3e-As (s) + 2 H2O 0.240
H2MoOa + 2H+ + 2e-→ MoD2 + 2 H2O 0.646
Mo02 + 4 H+ + e--* Mo3+ + 2 H20 0.008
Ag+ (aq) + e -→ Ag (s) 0.799
Fe3+ (aq) + e -→ Fe2+ (aq) 0.77
Fe2* (aq) 2Fe (s) 0.440
Al3 (a3Al (s) -1.676
Nİ2+ (aq) + 2e--+ Ni (s) 0.280
Selected Aqueous Equilibrium Constants at 25°C
Ka (HCN) -49-10-10
Ky (Ag(CN)2-)= 1.0 × 1021
Ksp FeAsO457x 10-21
Kal (H3As04) -5.6x 10-3
Ka2 (H3As04 10x 10-7
Ka3 (H3AsO4 3.0 x 10-12
Selected Thermodynamic Data at 25°C S
Delta H°f(kJ/mol) S°(J/mol K)
Zn (s) 0 4163
Zn2+ (aq) -153.9 -112.1
H2 (g) 0 130.7
H+ (aq) 0 0