Using the following standard reduction potentials, Fe³⁺(aq) + e^- →Fe²⁺(aq) E° = +0.77 V
Cu²⁺(aq) + 2 e^- →Cu(s) E° = +0.34 V
Calculate the standard cell potential for the galvanic cell reaction given below,and determine whether or not this reaction is spontaneous under standard conditions.
Cu²⁺(aq) + 2 Fe²⁺(aq) → 2 Fe³⁺(aq) + Cu(s)

Question

Quizplus · Accepted Answer

To calculate the standard cell potential, we need to subtract the reduction potential of the anode (Fe²⁺) from the reduction potential of the cathode (Cu²⁺). E°cell = E°cathode - E°anode E°cell = (0.34 V) - (0.77 V) = -0.43 V Since the calculated cell potential is negative, the reaction is nonspontaneous under standard conditions.

Using the Following Standard Reduction Potentials, Fe3+(aq)+ E- →Fe2+(aq)E° =

Using the Following Standard Reduction Potentials, Fe³⁺(aq)+ E^- →Fe²⁺(aq)E° =