Question

a) Draw Labelled diagram of Standard Hydrogen Electrode (SHE). Write its half-cell reaction of ${\text{E}}^0$ value.
b) Calculate $\mathrm{\Delta }r{G}^0$ for the following reaction:
$F{e^{+2}}_{\left(aq\right)}+A{g}^{+}\to F{e^{+3}}_{(aq)}+A{g}_{\left(s\right)}$, (Given$E_{\left(cell\right)}^0=+0.03V,F=96500C$)

Answer 1

Hint: The Standard Hydrogen Electrode, is a redox electrode which is the basic of the thermodynamic scale of oxidation-reduction potential. It is basically used as a reference electrode on half-cell potential reactions. The value of the standard electrode potential is zero, which forms the basis to calculate cell potentials using different electrodes or different concentrations.

Complete answer:
The Standard Hydrogen Electrode also known as SHE. The potential of SHE is always 0 at 298K, this is the reason it is used as a reference electrode.
The redox half-cell reaction of the SHE is:
$2{H^{+}}_{\left(aq\right)}+2e^{-}\to {H_2}_{\left(g\right)}$$E^0$
Hydrogen Standard electrode potential ($E^0$) is declared as zero at any temperature.

Addition Information:
The absolute electrode potential of SHE is measured to be 4.44+-0.02V at room temperature. But for a basic comparison with all other electrode reactions, Hydrogen standard electrode potential ($E^0$) is declared to be zero volts at any temperature.
The reasons for choice for platinum for the hydrogen electrode is:
-Inertness of platinum
-The capability of platinum to catalyze the reaction of proton reduction
-Use a surface material that absorbs hydrogen well at its interface. This increases the reaction kinetics

Note:
The value of standard electrode potential is always zero. During the reaction, hydrogen gas is passed through and into the solution and the reaction that takes place is: $2{H^{+}}_{\left(aq\right)}+2e^{-}\to {H_2}_{\left(g\right)}$
b) Calculate $\mathrm{\Delta }r{G}^0$ for the following reaction:
$F{e^{+2}}_{\left(aq\right)}+A{g}^{+}\to F{e^{+3}}_{(aq)}+A{g}_{\left(s\right)}$, (Given$E_{(cell)}^0=+0.03V,F=96500C$)