AP Chemistry
6.4 Heat Capacity and Calorimetry
6.3 Heat Transfer and Thermal Equilibrium
A student places a sample of an unknown metal with a mass of \(100.0\text{ g}\) and an initial temperature of \(80.0^\circ\text{C}\) into an insulated cup containing \(50.0\text{ g}\) of water at an initial temperature of \(20.0^\circ\text{C}\). The specific heat capacity of the metal is \(0.42\text{ J/(g}\cdot^\circ\text{C)}\), and the specific heat capacity of water is \(4.2\text{ J/(g}\cdot^\circ\text{C)}\). Assuming no heat is lost to the surroundings or the cup, what is the final thermal equilibrium temperature of the system?
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