AP Chemistry
6.5 Energy of Phase Changes
6.4 Heat Capacity and Calorimetry
A student warms an \(18.0\text{ g}\) frozen water sample from \(-10.0^\circ\text{C}\) until it becomes liquid water at \(25.0^\circ\text{C}\). The ice melts at \(0.0^\circ\text{C}\), and heat exchange with the surroundings is negligible.
Approximately how much total heat must be absorbed by the sample?
| Property | Value |
|---|---|
| Specific heat capacity of ice | \(2.0\text{ J/(g}\cdot^\circ\text{C)}\) |
| Specific heat capacity of liquid water | \(4.0\text{ J/(g}\cdot^\circ\text{C)}\) |
| Enthalpy of fusion of \(\text{H}_2\text{O}\) | \(6.0\text{ kJ/mol}\) |
| Molar mass of \(\text{H}_2\text{O}\) | \(18.0\text{ g/mol}\) |
Approximately how much total heat must be absorbed by the sample?
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