A student reacts a sample of pure aluminum metal with an excess of hydrochloric acid according to the following balanced chemical equation:

\[ 2\,\text{Al}(s) + 6\,\text{HCl}(aq) \rightarrow 2\,\text{AlCl}_3(aq) + 3\,\text{H}_2(g) \]

The generated \(\text{H}_2(g)\) is collected over water at \(27^\circ\text{C}\) (\(300\text{ K}\)). The experimental data obtained by the student are recorded in the table below.

Quantity	Measured Value
Mass of \(\text{Al}(s)\) reacted	\(0.0540\text{ g}\)
Total barometric pressure	\(780\text{ torr}\)
Temperature of gas and water	\(27^\circ\text{C}\) (\(300\text{ K}\))
Volume of wet \(\text{H}_2(g)\) collected	\(59.1\text{ mL}\)
Vapor pressure of water at \(27^\circ\text{C}\)	\(20\text{ torr}\)

Given that the molar mass of \(\text{Al}\) is \(27.0\text{ g/mol}\) and \(R = 0.0821\text{ L}\cdot\text{atm}/(\text{mol}\cdot\text{K})\), what is the percent yield of \(\text{H}_2(g)\) for the reaction?