A metal object is electroplated with nickel in an electrolytic cell containing an aqueous solution of \(\text{NiSO}_4\). A constant current of \(9.65\text{ A}\) is passed through the cell to deposit \(21.1\text{ g}\) of \(\text{Ni(s)}\) onto the object. Assuming that the reduction of \(\text{Ni}^{2+}\) is the only reaction occurring at the cathode and proceeds with \(100\%\) current efficiency, which of the following is closest to the time required to complete the electroplating process? (The molar mass of \(\text{Ni}\) is \(58.7\text{ g/mol}\), and Faraday's constant is \(96{,}500\text{ C/mol } e^-\).)