Chemistry - Electrochemistry Question with Solution | TestHub

The standard reduction potential of the copper electrode is $E^{\circ }({\mathrm{Cu}}^{+2}\mid \mathrm{Cu})=+0.34\mathrm{V}$.

The standard reduction potential of the standard hydrogen electrode (SHE) is $E^{\circ }({\mathrm{H}}^{+}\mid {\mathrm{H}}_2)=0.00\mathrm{V}$.

Since the standard reduction potential of copper is greater than that of hydrogen, copper has a higher tendency to get reduced. Therefore, in the galvanic cell, the copper electrode acts as the cathode (where reduction occurs) and the standard hydrogen electrode acts as the anode (where oxidation occurs).

At anode (oxidation):
${\mathrm{H}}_{2(\mathrm{g})}⟶2{\mathrm{H}}_{(\mathrm{aq})}^{+}+2{\mathrm{e}}^{-}$

At cathode (reduction):
${\mathrm{Cu}}_{(\mathrm{aq})}^{+2}+2{\mathrm{e}}^{-}⟶{\mathrm{Cu}}_{(\mathrm{s})}$

Adding the two half-cell reactions gives the net cell reaction:
${\mathrm{H}}_{2(\mathrm{g})}+{\mathrm{Cu}}_{(\mathrm{aq})}^{+2}⟶2{\mathrm{H}}_{(\mathrm{aq})}^{+}+{\mathrm{Cu}}_{(\mathrm{s})}$

Answer: ${\mathrm{H}}_{2(\mathrm{g})}+{\mathrm{Cu}}_{(\mathrm{aq})}^{+2}⟶2{\mathrm{H}}_{(\mathrm{aq})}^{+}+{\mathrm{Cu}}_{(\mathrm{s})}$