Consider the reaction of iodine with manganese dioxide. 3I₂(s) + 2MnO₂(s) + 8OH^-(aq) 6I^-(aq) + 2MnO₄^-(aq) + 4H₂O(l)
The equilibrium constant for the overall reaction is 8.3 × 10^-7. What is E°_cell for the reaction at 25°C? (R = 8.314 J/K • mol, F = 96,500 C • mol^-1)

Question

Consider the reaction of iodine with manganese dioxide. 3I₂(s) + 2MnO₂(s) + 8OH^-(aq)

Consider the reaction of iodine with manganese dioxide. 3I<sub>2</sub>(s) + 2MnO<sub>2</sub>(s) + 8OH<sup>-</sup>(aq) 6I<sup>-</sup>(aq) + 2MnO<sub>4</sub><sup>-</sup>(aq) + 4H<sub>2</sub>O(l) The equilibrium constant for the overall reaction is 8.3 × 10<sup>-7</sup>. What is E°<sub>cell</sub> for the reaction at 25°C? (R = 8.314 J/K • mol, F = 96,500 C • mol<sup>-1</sup>) A) -0.36 V B) -0.18 V C) -0.12 V D) -0.060 V E) +0.12 V

6I^-(aq) + 2MnO₄^-(aq) + 4H₂O(l)
The equilibrium constant for the overall reaction is 8.3 × 10^-7. What is E°_cell for the reaction at 25°C? (R = 8.314 J/K • mol, F = 96,500 C • mol^-1)

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The Answer of Consider the reaction of iodine with manganese dioxide. 3I₂(s) + 2MnO₂(s) + 8OH^-(aq) 6I^-(aq) + 2MnO₄^-(aq) + 4H₂O(l) The equilibrium constant for the overall reaction is 8.3 × 10^-7. What is E°_cell for the reaction at 25°C? (R = 8.314 J/K • mol, F = 96,500 C • mol^-1)

Consider the Reaction of Iodine with Manganese Dioxide