\(\mathrm{E}_{\text {cell }}^0\) of the reaction \(\mathrm{Mg}_{(\mathrm{s})}+2 \mathrm{Ag}^{+}(0.0001 \mathrm{M}) \rightleftharpoons \mathrm{Mg}^{2+}(0.01 \mathrm{M})+2 \mathrm{Ag}_{(\mathrm{s})}\) is \(3.17 \mathrm{~V}\). The \(\mathrm{E}_{\text {cell }}\) of the reaction and its cell notation respectively are :

1. A \(2.993 \mathrm{~V}, \mathrm{Ag}\left|\mathrm{Ag}^{+}(0.0001 \mathrm{M}) \| \mathrm{Mg}^2+(0.01 \mathrm{M})\right| \mathrm{Mg}\)
2. B \(\text { 3.993 V, } \mathrm{Mg}\left|\mathrm{Mg}^{2+}(0.0001 \mathrm{M}) \| \mathrm{Ag}^{+}(0.01 \mathrm{M})\right| \mathrm{Ag}\)
3. C \(2.993 \mathrm{~V}, \mathrm{Mg}\left|\mathrm{Mg}^{2+}(0.01 \mathrm{M}) \| \mathrm{Ag}^{+}(0.0001 \mathrm{M})\right| \mathrm{Ag}\)
4. D \(\text { 3.993 V, Ag| } \mathrm{Ag}^{+}(0.01 \mathrm{M}) \| \mathrm{Mg}^{2+}(0.0001 \mathrm{M}) \mid \mathrm{Mg}\)