A student conducts a calorimetry experiment to investigate thermal equilibrium. Three separate \(50.0\text{ g}\) metal samples—aluminum (\(\text{Al}\)), iron (\(\text{Fe}\)), and lead (\(\text{Pb}\))—are heated to \(100.0^\circ\text{C}\) in a boiling-water bath. Each hot metal sample is then transferred into a separate well-insulated calorimeter containing \(100.0\text{ g}\) of distilled water at \(20.0^\circ\text{C}\).

Metal	Specific Heat Capacity \(\left(\text{J}/(\text{g}\cdot^\circ\text{C})\right)\)
\(\text{Al(s)}\)	\(0.90\)
\(\text{Fe(s)}\)	\(0.45\)
\(\text{Pb(s)}\)	\(0.13\)

Assuming negligible heat loss to the surroundings and calorimeters, which of the following correctly ranks the final equilibrium temperatures, \(T_f\), of the water samples from greatest to least?