Digital ACT Science Practice Question #1825

Why did the aluminum sample produce a significantly higher final equilibrium temperature than lead despite having identical mass? Experiment Context (Calorimetric Determination of Specific Heat): A 100.0 g cylinder of various metals heated to 100.0°C was transferred into an insulated calorimeter containing 100.0 g of water at 20.0°C (c_water = 4.184 J/g*°C). Final equilibrium temperatures were recorded: Table 24: - Lead: Final Equilibrium Temp = 22.4°C; Metal Specific Heat = 0.13 J/g*°C - Copper: Final Equilibrium Temp = 27.1°C; Metal Specific Heat = 0.39 J/g*°C - Iron: Final Equilibrium Temp = 28.2°C; Metal Specific Heat = 0.45 J/g*°C - Aluminum: Final Equilibrium Temp = 36.4°C; Metal Specific Heat = 0.90 J/g*°C