A galvanic cell is constructed at \(298\text{ K}\) using a zinc electrode immersed in a \(1.0\text{ M }\text{Zn(NO}_3)_2(aq)\) solution and a copper electrode immersed in a \(1.0\text{ M }\text{Cu(NO}_3)_2(aq)\) solution. The overall cell reaction is represented below.

\[\text{Zn}(s) + \text{Cu}^{2+}(aq) \rightarrow \text{Zn}^{2+}(aq) + \text{Cu}(s) \quad E^\circ_{\text{cell}} = +1.10\text{ V}\]

A student adds \(100\text{ mL}\) of distilled water to the cathode compartment while keeping the anode compartment unchanged. Which of the following best predicts and explains the effect of this change on the cell potential, \(E_{\text{cell}}\)?