Define what is meant by standard cell potential.
Draw a fully labelled diagram of the experimental arrangement you would use to measure the standard electrode potential of the $\text{Pb}^{2+}$(aq)/Pb(s) electrode. Include the required chemicals.
The $E^\circ$ for a $\text{Pb}^{2+}$(aq)/Pb(s) electrode is $-0.13\,\text{V}$. Suggest how the $E$ for this electrode would change relative to its $E^\circ$ value if the concentration of $\text{Pb}^{2+}$(aq) ions is lowered. Show your choice by putting a tick (✓) in the correct box in the table. Explain your answer.
Calculate the mass of Pb converted to $\text{PbSO}_4$ when a current of $0.40\,\text{A}$ is supplied by the cell for $80\,\text{minutes}$.
Complete the half-equation for the reaction happening at the positive electrode. $\text{PbO}_2$(s) + \text{SO}_4^{2-}$(aq) + \ldots + \ldots \rightarrow \text{PbSO}_4$(s) + \ldots$
The diagrams show how the voltage across two different cells changes with time while each cell is used to supply an electric current. Suggest a reason why the voltage of the lead-acid cell changes after several hours, and why the voltage of the fuel cell stays constant.