A student constructs an electrolytic cell to plate pure copper onto an electrode. The cell contains an aqueous solution of \(\text{CuSO}_4\) and is operated at a constant current of \(9.65\text{ A}\) for \(10.0\text{ minutes}\). The reduction half-reaction at the cathode is

\[\text{Cu}^{2+}\text{(aq)} + 2\,e^- \rightarrow \text{Cu(s)}\]

Assuming \(100\%\) current efficiency, what mass of \(\text{Cu(s)}\) is deposited onto the cathode?