A \(70.0\text{ g}\) sample of solid aluminum (specific heat capacity \(0.90\text{ J}/(\text{g}\cdot^\circ\text{C})\)) is heated to \(100.0^\circ\text{C}\) in a hot water bath and then quickly transferred into an insulated coffee-cup calorimeter containing \(60.0\text{ g}\) of distilled water (specific heat capacity \(4.2\text{ J}/(\text{g}\cdot^\circ\text{C})\)) initially at \(20.0^\circ\text{C}\). Assuming no heat is lost to the calorimeter cup or the surroundings, what is the final temperature of the mixture at thermal equilibrium?