A student constructs a galvanic concentration cell at \(298\text{ K}\) by placing a strip of solid silver, \(\text{Ag(s)}\), into each of two beakers. Beaker 1 contains \(100\text{ mL}\) of \(0.010\text{ M}\ \text{AgNO}_3\text{(aq)}\), and Beaker 2 contains \(100\text{ mL}\) of \(1.0\text{ M}\ \text{AgNO}_3\text{(aq)}\). The two half-cells are connected by a salt bridge, and a wire connects the two silver electrodes through a voltmeter. Based on the Nernst equation at \(298\text{ K}\), \(E_{\text{cell}} = E^\circ_{\text{cell}} - \dfrac{0.0592\text{ V}}{n}\log Q\), what is the initial cell potential, \(E_{\text{cell}}\)?