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

Question

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

Quizplus · Accepted Answer

To find E°cell, subtract the reduction potential of the anode (Cl₂) from the reduction potential of the cathode (F₂): E°cell = E°(cathode) - E°(anode) = 2.866 V - 1.358 V = 1.508 V. However, the reaction is reversed, so the sign changes, resulting in -1.508 V.

Determine E°cell for the Reaction: Cl2 + 2 F- →

Determine E°cell for the Reaction: Cl₂ + 2 F- →