Determine E°_cell for the reaction: I₂(s) + Cu(s) → 2 I^-(aq) + Cu²⁺(aq) .The half reactions are:
I₂(s) + 2 e^- → 2 I^-(aq) E° = +0.535 V
Cu²⁺(aq) + 2 e^- → Cu(s) E° = 0.340 V

Question

Determine E°_cell for the reaction: I₂(s)+ Cu(s)→ 2 I^-(aq)+ Cu²⁺(aq).The half reactions are: I₂(s)+ 2 e^- → 2 I^-(aq)E° = +0.535 V Cu²⁺(aq)+ 2 e^- → Cu(s)E° = 0.340 V

Quizplus · Accepted Answer

The standard cell potential, E°cell, is calculated by subtracting the standard reduction potential of the anode (the oxidation half-reaction) from the standard reduction potential of the cathode (the reduction half-reaction). In this case, the I2(s) is being reduced and Cu is being oxidized, so E°cell = E°cathode - E°anode = 0.535 V - 0.340 V = 0.195 V.

Determine E°cell for the Reaction: I2(s)+ Cu(s)→ 2 I-(aq)+ Cu2+(aq)

Determine E°_cell for the Reaction: I₂(s)+ Cu(s)→ 2 I^-(aq)+ Cu²⁺(aq)