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.

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.

$$\begin{gathered} {\mathrm{Co}}^{2+}\left(\mathrm{aq}\right)+2{\mathrm{e}}^{-}\to \mathrm{Co}\left(\mathrm{s}\right){\mathrm{E}}^{\ominus }=-0.28\mathrm{V} \\ {\mathrm{Ag}}^{+}\left(\mathrm{aq}\right) + {\mathrm{e}}^{-} \to \mathrm{Ag}\left(\mathrm{s}\right){\mathrm{E}}^{\ominus }= 0.80 \mathrm{V} \end{gathered}$$

Identify the direction of the movement of electrons and ion flow, both in solution and in the salt bridge.

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.

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.

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

Determine ${\mathrm{\Delta G}}^{\ominus }$ , the standard change in Gibbs free energy, in J, for the electrochemical reaction.

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.