In an electrochemical cell, the following reaction takes place: 2 Ag^+( aq )+ Mg ( s ) → 2 Ag ( s )+ Mg^2+( aq ); E_cell^°=2 · 96 V As the reaction…

In an electrochemical cell, the following reaction takes place : \[\begin{aligned} & 2 \mathrm{Ag}^{+}(\mathrm{aq})+\mathrm{Mg}(\mathrm{~s}) \rightarrow 2 \mathrm{Ag}(\mathrm{~s})+\mathrm{Mg}^{2+}(\mathrm{aq}) \\ & \mathrm{E}_{\text {cell }}^{\circ}=2 \cdot 96 \mathrm{~V} \end{aligned} \] As the reaction progresses, what will happen to the overall voltage of the cell ?