AP Chemistry
6.4 Heat Capacity and Calorimetry
A student performs a coffee-cup calorimetry experiment to determine the specific heat capacity of an unknown metal. A sample of the metal is heated in a water bath and quickly transferred into an insulated cup containing water. The collected data are shown in the table below.
Assuming that no heat is lost to the calorimeter or the surroundings, what is the specific heat capacity of the unknown metal? (The specific heat capacity of water is \(4.18\text{ J}/(\text{g}\cdot^\circ\text{C})\).)
| Measurement | Value |
|---|---|
| Mass of unknown metal sample | \(50.0\text{ g}\) |
| Initial temperature of metal | \(98.0^\circ\text{C}\) |
| Mass of water in calorimeter | \(100.0\text{ g}\) |
| Initial temperature of water | \(20.0^\circ\text{C}\) |
| Final temperature of mixture | \(22.0^\circ\text{C}\) |
Assuming that no heat is lost to the calorimeter or the surroundings, what is the specific heat capacity of the unknown metal? (The specific heat capacity of water is \(4.18\text{ J}/(\text{g}\cdot^\circ\text{C})\).)
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