State the substances released at the anode and at the cathode in the electrolysis of saturated $\text{KCl}(aq)$.
During the electrolysis of dilute sulfuric acid, oxygen is produced at the anode. Dilute sulfuric acid is electrolysed for $15.0$ minutes with a current of $0.750\,\text{A}$. Calculate the volume of oxygen produced under room conditions.
State the $E^\circ$ values for chlorine, bromine and iodine when each is acting as an oxidising agent.
Decide which of chlorine, bromine and iodine will react with a solution of $\text{Sn}^{2+}(aq)$ under standard conditions. Justify your answer. Include a relevant equation in your response.
Excess chlorine is added to a solution of acidified $\text{Mn}^{2+}(aq)$ under standard conditions. Give the formula of the manganese-containing product formed in this reaction.
An electrochemical cell may be formed by linking an $\text{Fe}^{3+}/\text{Fe}^{2+}$ half-cell with an $\text{S}_2\text{O}_8^{2-}/\text{SO}_4^{2-}$ half-cell under standard conditions. Calculate the standard cell potential of this electrochemical cell.
State the material that should be used for the electrode in each half-cell: in the $\text{Fe}^{3+}/\text{Fe}^{2+}$ half-cell; in the $\text{S}_2\text{O}_8^{2-}/\text{SO}_4^{2-}$ half-cell.
Describe one change to each half-cell that would raise the cell potential. The temperature must stay at $298\,\text{K}$.