Calculate the equilibrium constant, K, for the reaction shown at 25 °C. Fe*(aq) + B(s) + 6H,O(1) - Fe(s) + H,BO, (s) + 3 H,O*(aq) The balanced reduction half-reactions for the equation and their respective standard reductio Fe3+(aq) + 3 e¯ → Fe(s) E° = -0.04 V H,BO, (s) + 3 H,0*(aq) + 3 e- B(s) + 6 H,O(1) E° = -0.8698 V

Half-reaction E° (V) Cr3+ (aq) + 3e- → Cr (s) -0.74 Fe2+ (aq) + 2e- → Fe (s) -0.440 Fe3+ (aq) + e- → Fe2+ (s) +0.771 Sn4+ (aq) + 2e- → Sn2+ (aq) +0.154 The standard cell potential (E°cell) for the voltaic cell based on the reaction below is ________ V.Sn2+ (aq) + 2Fe3+ (aq) → 2Fe2+ (aq) + Sn4+ (aq)   a). +1.21 b). +0.617 c). -0.46 d). +1.39 e). +0.46

7. Please answer the following questions. (a) Given the following reduction potentials Cd (OH)2 (s) + 2e → Cd (s) + 2 OH (aq) Eºred = -0.76 V NIO(OH) (s) + H₂O (1) + e → Ni(OH)2 (aq) + OH (aq) Eºred = +0.49 V Calculate the standard emf of the nickel-cadmium (nicad) rechargeable battery. *hint: the reaction for the discharge of nicad battery is: Cd (s) + 2 NIO(OH) (s) + 2 H₂O (1)→ 2Ni(OH)2 (aq) + Cd(OH)2 (s) (b) A typical nicad voltaic cell generates an emf of +1.30 V. Why is there a difference between this value and the one you calculated in part (b)? (c) Calculate the equilibrium constant for the overall nicad reaction based on this typical emf value.

Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AG for the following redox reaction. Round your answer to 2 significant digits. 2Cr(OH)3 (s) +100H¯ (aq) +3Zn²+ (aq) → 2CrO²¯ (aq) +8H₂O (1) + 3 Zn (s) 0 x10 X