a. Define the term standard electrode potential.

b. Draw a labelled diagram to show how the standard electrode potential of a half-cell containing chlorine gas and chloride ions can be measured.

c. Write a half-equation for this half-cell.

d. The standard electrode potential of a Cl₂/Cl^– half-cell is +1.36 V. This Cl₂/Cl^– half-cell was connected to a standard half-cell containing solid iodine in equilibrium with iodide ions. The standard electrode potential of an I₂/I^– half-cell is +0.54 V.

i. Calculate the standard cell voltage for this cell.

ii. Write the balanced ionic equation for the overall cell reaction.