A sample of \(4.86\text{ g}\) of \(\text{Mg(s)}\) is placed in a rigid sealed container containing \(4.80\text{ g}\) of \(\text{O}_2\text{(g)}\). The mixture is ignited and the reaction proceeds to completion according to the equation below.

\[ 2\,\text{Mg(s)} + \text{O}_2\text{(g)} \rightarrow 2\,\text{MgO(s)} \]

Given that the molar masses of \(\text{Mg}\), \(\text{O}_2\), and \(\text{MgO}\) are \(24.3\text{ g/mol}\), \(32.0\text{ g/mol}\), and \(40.3\text{ g/mol}\), respectively, what is the maximum mass of \(\text{MgO(s)}\) that can be produced?