Identify the substances produced at the anode and at the cathode in the electrolysis of aqueous sodium sulfate, $\text{Na}_2\text{SO}_4\text{(aq)}$.
In the electrolysis of molten sodium chloride, chlorine is formed at the anode and sodium is formed at the cathode. A sample of molten sodium chloride is electrolysed for $1.50$ hours with a current of $4.50\,\text{A}$. Calculate the volume of chlorine and the mass of sodium formed at room conditions.
The equation for the standard electrode potential, $E^{\circ}$, for the reduction of $\text{MnO}_4^{-}\text{(aq)}$ to $\text{Mn}^{2+}\text{(aq)}$ in acid solution is $\text{MnO}_4^{-}\text{(aq)} + 8\text{H}^+\text{(aq)} + 5e^- \rightleftharpoons \text{Mn}^{2+}\text{(aq)} + 4\text{H}_2\text{O(l)}$ with $E^{\circ} = +1.52\,\text{V}$. Draw the apparatus diagram that would be used to measure the $E^{\circ}$ value of this half-cell. Your diagram should be fully labelled to show all apparatus, substances and conditions.
Use the Data Booklet to identify a substance that could oxidise $\text{Mn}^{2+}$ ions to $\text{MnO}_4^{-}$ ions under standard conditions. Write an equation for the reaction.