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.) 2F₂(g) + Mn(s) → 4 F⁻(aq) + Mn²⁺(aq)
F₂(g) + e⁻ → 2 F⁻(aq) E° = +2.87 V
Mn²⁺(aq) + 2 e⁻ → Mn(s) E° = -1.18 V

Question

Quizplus · Accepted Answer

First, we need to identify the oxidation and reduction half-reactions: Oxidation: F₂(g) + e⁻ → 2 F⁻(aq) E° = +2.87 V Reduction: Mn²⁺(aq) + 2 e⁻ → Mn(s) E° = -1.18 V We need to reverse the oxidation half-reaction to match the reactants in the reduction half-reaction: 2 F⁻(aq) → F₂(g) + e⁻ E° = -2.87 V Now, we can add the two half-reactions together to get the overall reaction: 2 F₂(g) + Mn(s) → 4 F⁻(aq) + Mn²⁺(aq) We add the standard reduction potential and the standard oxidation potential to obtain the standard cell potential: E°cell = E°reduction + E°oxidation E°cell = -1.18 V + (-2.87 V) E°cell = -4.05 V The answer is B) 4.050 V because the standard cell potential is negative, indicating a non-spontaneous reaction.

Use the Standard Half-Cell Potentials Listed Below to Calculate the Standard