Determine E°_cell for the reaction: Cl₂(g) + 2 F^-(aq) → 2 Cl^-(aq) + F₂(g) .The half reactions are:
F₂(g) + 2 e^- → 2 F^-(aq) E° = +2.866 V
Cl₂(g) + 2 e^- → 2 Cl^-(aq) E° = 1.358 V

Question

Determine E°_cell for the reaction: Cl₂(g)+ 2 F^-(aq)→ 2 Cl^-(aq)+ F₂(g).The half reactions are: F₂(g)+ 2 e^- → 2 F^-(aq)E° = +2.866 V Cl₂(g)+ 2 e^- → 2 Cl^-(aq)E° = 1.358 V

Quizplus · Accepted Answer

The standard cell potential (E°cell) is calculated by subtracting the reduction potential of the anode from the reduction potential of the cathode. Here, F2 is reduced and Cl2 is oxidized. E°cell = E°(F2) - E°(Cl2) = 2.866 V - 1.358 V = 1.508 V. Since the reaction is reversed, the sign changes, resulting in -1.508 V.

Determine E°cell for the Reaction: Cl2(g)+ 2 F-(aq)→ 2 Cl-(aq)

Determine E°_cell for the Reaction: Cl₂(g)+ 2 F^-(aq)→ 2 Cl^-(aq)