State the electrode material used in each half-cell. • $\text{Sn}^{4+}/\text{Sn}^{2+}$ half-cell • $\text{Al}^{3+}/\text{Al}$ half-cell
Use the Nernst equation to work out the electrode potential, $E$, of the $\text{Sn}^{4+}/\text{Sn}^{2+}$ half-cell under these conditions.
Calculate the $E_{\text{cell}}$ under these conditions.
Write an equation for the overall cell reaction that takes place.
Aluminium is made industrially by electrolysis of a melt that contains large amounts of $\text{Al}^{3+}$ ions. Calculate the mass of aluminium obtained when a current of $300\,000\,\text{A}$ flows for $24$ hours. Give your answer to three significant figures.
Explain why chromium metal cannot be obtained by electrolysis of dilute aqueous chromium(II) sulfate. Your response should include data from the Data Booklet.