In the given reaction,

Copper metal, Cu(s) is oxidised to ${\mathrm{Cu}}^{2+}$ (aq), while ${\mathrm{Ag}}^{+}$(aq) is reduced to silver metal, Ag (s), then the equilibrium greatly lies in favour of

• A

  ${\mathrm{Ag}}^{+}\left(\mathrm{s}\right)\text{ and }{\mathrm{Cu}}^{2+}\left(\mathrm{aq}\right)$

• B

  ${\mathrm{Ag}}^{+}\left(\mathrm{aq}\right)\text{ and }{\mathrm{Cu}}^{2+}\left(\mathrm{s}\right)$

• C

  $\mathrm{Ag}\left(\mathrm{s}\right)\text{ and }{\mathrm{Cu}}^{2+}\left(\mathrm{aq}\right)$

• D

  ${\mathrm{Cu}}^{2+}\left(\mathrm{aq}\right)\text{ and }\mathrm{Ag}\left(\mathrm{s}\right)$