Problem: The standard emf for the cell using the overall cell reaction below is +2.20 V:The emf generated by the cell when[Al3+] = 4.5 x 10-3 M and [I-] = 0.15 M is _____ V.

We're being asked to calculate the emf generated by the cell when [Al³⁺] = 4.5×10^‒3 M and [I^‒] = 0.15 M.

We're going to calculate for E_cell using the following steps:

Step 1: Write the two half-reactions and determine the anode and cathode.
Step 2: Write the overall reaction and determine the number of electrons transferred (n).
Step 3: Calculate E_cell using the Nernst equation.

$\boxed{{\mathbf{E}}_{\mathbf{cell}}\mathbf{=}\mathbf{E}{\mathbf{°}}_{\mathbf{cell}}\mathbf{-}\mathbf{\left(}\frac{\mathbf{0}\mathbf{.}\mathbf{05916}\mathbf{ }\mathbf{V}}{\mathbf{n}}\mathbf{\right)}\mathbf{ }\mathbf{log}\mathbf{ }\mathbf{Q}}$

Step 1: Write the two half-reactions and determine the anode and cathode.