Final answer:
To determine oxidation and reduction half-reactions and whether a reaction is spontaneous, one must know the oxidation states of reactants and products,
Step-by-step explanation:
The initial reaction provided seems to contain a typo with the ion 'CO₂⁺⁺' and 'Co₃₂⁻' which are not common ions. Assuming that it might be 'Co²⁺' for cobalt(II) and 'Co³⁺' for cobalt(III), let's correct it to:
Fe³⁺(aq) + Co²⁺(aq) → Fe²⁺(aq) + Co³⁺(aq)
The oxidation and reduction half-reactions will be identified based on the change in oxidation states of iron and cobalt. The standard cell potential (E°) is calculated using the standard reduction potentials from a reference table (which we assume to be provided).
Oxidation half-reaction:
Fe²⁺(aq) → Fe³⁺(aq) + e⁻
Reduction half-reaction:
Co³⁺(aq) + e⁻ → Co²⁺(aq)
To calculate the E° cell, we would use the standard electrode potentials for Fe³⁺/Fe²⁺ and Co³⁺/Co²⁺ couples from a reference table, adding them if the tabulated values are for the reduction half-reactions or subtracting if one is reversed (oxidation).
A positive value of E° cell would indicate that the reaction is spontaneous under standard conditions.