A student constructs a galvanic cell at \(298\text{ K}\) using the reaction represented below:

\[ \text{Ni(s)} + 2\,\text{Ag}^+\text{(aq)} \rightarrow \text{Ni}^{2+}\text{(aq)} + 2\,\text{Ag(s)} \quad E^\circ_{\text{cell}} = +1.06\text{ V} \]

The cell is initially operated under standard conditions with \([\text{Ni}^{2+}] = 1.0\text{ M}\) and \([\text{Ag}^+] = 1.0\text{ M}\). The student then dilutes the solution in the anode compartment by adding distilled water until \([\text{Ni}^{2+}] = 0.010\text{ M}\), while maintaining \([\text{Ag}^+] = 1.0\text{ M}\) at \(298\text{ K}\). Which of the following best predicts how the cell potential, \(E_{\text{cell}}\), changes, and provides the correct justification?