A student constructs a galvanic cell under standard conditions. One beaker contains a \(\text{Zn(s)}\) electrode immersed in \(1.0\text{ M }\text{Zn(NO}_3)_2\text{(aq)}\), and the second beaker contains a \(\text{Cu(s)}\) electrode immersed in \(1.0\text{ M }\text{Cu(NO}_3)_2\text{(aq)}\). The two half-cells are connected by an external wire with a voltmeter and a salt bridge filled with \(\text{KNO}_3\text{(aq)}\). The balanced equation for the spontaneous reaction is
\[\text{Zn}(s) + \text{Cu}^{2+}(aq) \rightarrow \text{Zn}^{2+}(aq) + \text{Cu}(s)\]
Which of the following correctly identifies the direction of \(\text{NO}_3^-\text{(aq)}\) ion migration from the salt bridge and provides the correct justification?