A student constructs two separate concentration cells at \(298\text{ K}\). Cell 1 consists of two \(\text{Ag(s)}\) electrodes immersed in separate beakers containing \(\text{AgNO}_3(aq)\). Cell 2 consists of two \(\text{Cu(s)}\) electrodes immersed in separate beakers containing \(\text{CuSO}_4(aq)\). In both setups, the half-cells are connected by a salt bridge and an external wire, and the reaction quotient is defined as \(Q = \dfrac{[\text{cation}]_{\text{anode}}}{[\text{cation}]_{\text{cathode}}}\). The graph shows the measured cell potential, \(E_{\text{cell}}\), as a function of \(\log Q\) as each cell discharges toward equilibrium.

Which of the following correctly identifies the curve corresponding to Cell 1 (\(\text{Ag/Ag}^+\)) and provides the correct explanation for why both curves intersect the horizontal axis at \(\log Q = 0\)?