State the standard conditions applied to the $\text{Sn}^{4+}/\text{Sn}^{2+}$ half-cell.
Finish the diagram below to show the experimental measurement of $E^\circ(\text{Sn}^{4+}/\text{Sn}^{2+})$. Make sure every piece of apparatus and every substance is fully labelled.
Mix equal volumes of $1.0\ \text{mol dm}^{-3}\ \text{Sn}^{2+}(aq)$ and $1.0\ \text{mol dm}^{-3}\ \text{Cl}^-(aq)$. Use appropriate $E^\circ$ values to explain whether these two ions react.
Mix equal volumes of $1.0\ \text{mol dm}^{-3}$ of $\text{Sn}^{2+}(aq)$ and acidified $1.0\ \text{mol dm}^{-3}\ \text{VO}^{2+}(aq)$. Write an equation for the reaction occurring in the mixture.
A solution of $\text{SnCl}_2(aq)$ is electrolysed for a set time using a constant current. This produces $2.95\ \text{g}$ of tin metal 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.