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.

Construct and annotate an example of a voltaic cell consisting of a $\mathrm{Ni}\left(\mathrm{s}\right)\mid {\mathrm{Ni}}^{2+}\left(\mathrm{aq}\right)$ half-cell and a $\mathrm{Cu}\left(\mathrm{s}\right)\mid {\mathrm{Cu}}^{2+}\left(\mathrm{aq}\right)$ half-cell.

Deduce the equation for the spontaneous reaction occurring in this cell.

A voltaic cell consisting of a $\mathrm{Ni}\left(\mathrm{s}\right)\mid {\mathrm{Ni}}^{2+}\left(\mathrm{aq}\right)$ half-cell and a $\mathrm{Cu}\left(\mathrm{s}\right)\mid {\mathrm{Cu}}^{2+}\left(\mathrm{aq}\right)$ half-cell.

State the cell diagram convention for the cell.

Construct and annotate an example of a voltaic cell consisting of a $\mathrm{Ag}\left(\mathrm{s}\right)\mid {\mathrm{Ag}}^{+}\left(\mathrm{aq}\right)$ half-cell and a $\mathrm{Co}\left(\mathrm{s}\right)\mid {\mathrm{Co}}^{2+}\left(\mathrm{aq}\right)$ half-cell.

Deduce the equation for the spontaneous reaction occurring in this cell.

A voltaic cell consisting of a $\mathrm{Ag}\left(\mathrm{s}\right)\mid {\mathrm{Ag}}^{+}\left(\mathrm{aq}\right)$ half-cell and a $\mathrm{Co}\left(\mathrm{s}\right)\mid {\mathrm{Co}}^{2+}\left(\mathrm{aq}\right)$ half-cell.

State the cell diagram convention for the cell.

A voltaic cell is consists of a $\mathrm{Ag}\left(\mathrm{s}\right)\mid {\mathrm{Ag}}^{+}\left(\mathrm{aq}\right)$ half-cell and a $\mathrm{Co}\left(\mathrm{s}\right)\mid {\mathrm{Co}}^{2+}\left(\mathrm{aq}\right)$ half-cell.

Given: ${\mathrm{Co}}^{2+}\left(\mathrm{aq}\right)+2{\mathrm{e}}^{-}\rightleftharpoons \mathrm{Co}\left(\mathrm{s}\right){\mathrm{E}}^{\ominus }=-0.28\mathrm{V}$, ${\mathrm{Ag}}^{+}\left(\mathrm{aq}\right)/\mathrm{Ag}\left(\mathrm{s}\right) = 0.80 \mathrm{V}$

Calculate the standard potential, in $\mathrm{V}$, for this cell.

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.