An electrolytic cell is operated at a constant current of \(1.93\text{ A}\) to electrolyze water. The oxidation half-reaction occurring at the anode is shown below.

\[ 2\text{H}_2\text{O}(l) \rightarrow \text{O}_2(g) + 4\text{H}^+(aq) + 4e^- \]

Assuming the oxygen gas behaves ideally, how many minutes of electrolysis are required to produce \(67.2\text{ mL}\) of \(\text{O}_2(g)\) at standard temperature and pressure (STP)? (Assume that \(1\text{ mol}\) of gas occupies \(22.4\text{ L}\) at STP and \(1\text{ F} = 96{,}500\text{ C/mol } e^-\).)