The same quantity of electricity was passed through separate molten samples of sodium bromide, $\mathrm{NaBr}$, and magnesium chloride, ${\mathrm{MgCl}}_2$. Which statement is true about the amounts, in mol, that are formed?

What is the mass, in g, of copper produced at the cathode when a current of $1.00 \mathrm{A}$ is passed through a solution of aqueous copper(II) sulphate for $60$ minutes?

$\left(1\mathrm{F}=96500 {\mathrm{C} \mathrm{mol}}^{-1}\right)$

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

Identify the half-equations occurring at the cathode and anode electrodes.

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.