Construct and annotate the electrolytic cell for the electrolysis of concentrated potassium iodide.

Identify the half-equations occurring at the cathode and anode electrodes and the equation for the overall cell reaction.

Construct and annotate the electrolytic cell for the electrolysis of concentrated potassium iodide.

State a suitable material that can be used for each electrode.

Construct and annotate the electrolytic cell for the electrolysis of concentrated potassium iodide.

Identify the direction of the movement of electrons and ion flow.

Construct and annotate the electrolytic cell for the electrolysis of concentrated potassium iodide.

State what would be observed at each electrode.

A current of $2.35 \mathrm{A}$ is passed through an electrolytic cell for the electrolysis of water, using a dilute sulphuric acid solution, for a duration of $5.00 \mathrm{h}$.

Construct and annotate a suitable electrolytic cell for this experiment.

A current of $2.35 \mathrm{A}$ is passed through an electrolytic cell for the electrolysis of water, using a dilute sulfuric acid solution, for a duration of $5.00 \mathrm{h}$.

Identify the half-equations occurring at the cathode and anode electrodes and the equation for the overall cell reaction.

A current of $2.35 \mathrm{A}$ is passed through an electrolytic cell for the electrolysis of water, using a dilute sulphuric acid solution, for a duration of $5.00 \mathrm{h}$.

Identify the direction of the movement of electrons and ion flow.

A current of $2.35 \mathrm{A}$ is passed through an electrolytic cell for the electrolysis of water, using a dilute sulphuric acid solution, for a duration of $5.00 \mathrm{h}$.

Determine the volume, in ${\mathrm{cm}}^3$, of the two gases generated in the process at SATP conditions.

Electroplating is an important application of electrolytic cells with commercial implications. Copper may be plated using an electrolytic cell with an aqueous acidified copper(II) sulfate electrolyte. For the copper plating of tin to make jewellery, state the half-equation at each electrode.

Assume the tin electrode is inert. Suggest two observations that you would be able to make as the electroplating progresses.