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We’re being asked to determine the standard cell potential (E°cell) of the reaction occurring in an electrochemical cell. To calculate for the standard cell potential, use the following equation:
When a balanced reaction is given, identify the anode and the cathode half-reactions by determining the changes in oxidation states of each species based on the given reaction:
Use the standard half-cell potentials listed below to calculate the standard cell potential, E°cell, for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.)
3 Br2(l) + 2 Fe(s) → 6Br1-(aq) + 2Fe2+(aq)
Br2(l) + 2 e- → 2 Br1-(aq) E° = +1.09 V
Fe2+(aq) + 2 e- → Fe(s) E° = -0.45 V
B) -0.64 V
C) -1.54 V
D) +1.54 V
E) the standard cell potential is 0.0v
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Based on our data, we think this problem is relevant for Professor Marzal's class at UCF.