Describe the standard conditions applied to the $\text{Sn}^{4+}/\text{Sn}^{2+}$ half-cell.
Complete the diagram below to show experimentally how $E^\circ(\text{Sn}^{4+}/\text{Sn}^{2+})$ may be measured. Your diagram must be fully labelled so that every apparatus item and substance is identified.
Equal volumes of $1.0\,\text{mol dm}^{-3}\,\text{Sn}^{2+}(aq)$ and $1.0\,\text{mol dm}^{-3}\,\text{Cl}^-(aq)$ are mixed. Use relevant $E^\circ$ values to explain whether a reaction takes place between these ions.
Equal volumes of $1.0\,\text{mol dm}^{-3}$ of $\text{Sn}^{2+}(aq)$ and acidified $1.0\,\text{mol dm}^{-3}\,\text{VO}_2^+(aq)$ are mixed. Write an equation for the reaction occurring in the final mixture.
A solution of $\text{SnCl}_2(aq)$ is electrolysed for a measured period using a steady current. A mass of $2.95\,\text{g}$ of tin metal forms at the cathode. $\text{Al}_2\text{O}_3(l)$ is electrolysed for the same period with the same current. Calculate the mass of aluminium metal formed at the cathode. Give your answer to three significant figures. Show your working.