Question

A voltaic cell houses the reaction between aqueous iodine and cobalt metal: I₂(aq) + Co(s) → Co²⁺(aq) + 2I⁻(aq) E°cell = 2.63 V. Calculate E°iodine, given that E°cobalt = -1.16 V

Answer 1

The standard electrode potential for iodine in a voltaic cell with a cell potential of 2.63 V and a known cobalt potential of -1.16 V is calculated to be 1.47 V.

Step-by-step explanation:

The student has asked to calculate the standard electrode potential for iodine, E°iodine, in the voltaic cell reaction between aqueous iodine and cobalt metal which has a cell potential (E°cell) of 2.63 V and given that the standard electrode potential for cobalt (E°cobalt) is -1.16 V. The relationship between the cell potential and the electrode potentials of the two half-cells is given by the equation E°cell = E°cathode - E°anode. To find E°iodine, which acts as the cathode in this reaction, we rearrange the equation to E°cathode = E°cell + E°anode. Plugging in the values, we get E°iodine = 2.63 V + (-1.16 V) = 1.47 V. This positive value indicates that the iodine/cobalt reaction is spontaneous under standard conditions.