Sergey Bylikin, Gary Horner and, Brian Murphy Solutions for Chapter: Redox Processes (AHL), Exercise 2: Question

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.

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

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.

A voltaic cell is consists 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.

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

Given: ${\mathrm{Ni}}^{2+}\left(\mathrm{aq}\right)+2{\mathrm{e}}^{-}\rightleftharpoons \mathrm{Ni}\left(\mathrm{s}\right){\mathrm{E}}^{\ominus }=-0.23\mathrm{V}$, ${\mathrm{Cu}}^{2+}\left(\mathrm{aq}\right)/\mathrm{Cu}\left(\mathrm{s}\right) = 0.34 \mathrm{V}$

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

A voltaic cell is consists 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.

Given: ${\mathrm{Ni}}^{2+}\left(\mathrm{aq}\right)+2{\mathrm{e}}^{-}\rightleftharpoons \mathrm{Ni}\left(\mathrm{s}\right){\mathrm{E}}^{\ominus }=-0.23\mathrm{V}$, ${\mathrm{Cu}}^{2+}\left(\mathrm{aq}\right)/\mathrm{Cu}\left(\mathrm{s}\right) = 0.34 \mathrm{V}$

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