Liquid bromine is added to an aqueous solution of potassium iodide. The following reaction takes place.

Br₂(l) + 2I^–(aq) 2Br ^–(aq) + I₂(aq) E^θcell = +0.53 V

a. Write two half-equations for this reaction.

b. Draw a labelled diagram to show two linked half-cells that could be used to measure the standard cell potential for this reaction.

c. The standard cell potential for this reaction is +0.53 V. Does the position of equilibrium favour the reactants or the products? Explain your answer.

d. The standard electrode potentials for a number of half-equations are shown below:

Fe³⁺(aq) + e^– → Fe²⁺(aq)        E^θ= +0.77 V

I₂(aq) + 2e^– → 2I–(aq)            E^θ = +0.54 V

Ni²⁺(aq) + 2e^– → Ni(s)            E^θ= –0.25 V

Pb⁴⁺(aq) + 2e^– → Pb²⁺(aq)    E^θ= +1.69 V

Which atom or ion in this list will reduce iodine to iodide ions? Explain your answer.