A student heats a \(100.0\text{ g}\) sample of a metal with a specific heat capacity of \(0.418\text{ J}/(\text{g}\cdot^\circ\text{C})\) in a boiling water bath until it reaches a uniform temperature of \(100.0^\circ\text{C}\). The metal is quickly transferred to an insulated calorimeter containing \(90.0\text{ g}\) of distilled water (specific heat capacity \(4.18\text{ J}/(\text{g}\cdot^\circ\text{C})\)) at \(20.0^\circ\text{C}\). Assuming no heat is lost to the calorimeter or the surroundings, what is the final temperature of the system at thermal equilibrium?