AP Chemistry
6.5 Energy of Phase Changes
6.4 Heat Capacity and Calorimetry
6.3 Heat Transfer and Thermal Equilibrium
A student prepares three separate mixtures in identical, insulated calorimeters as shown in the table below. In each trial, a solid ice cube at \(0.0^\circ\text{C}\) is added to liquid water, and each system is allowed to reach thermal equilibrium. Assume negligible heat exchange with the calorimeter and the surroundings.
(\(\Delta H_{\text{fus}}\) of ice \(= 336\text{ J/g}\); specific heat capacity of liquid water \(= 4.2\text{ J}/(\text{g}\cdot^\circ\text{C})\))
Which of the following correctly ranks the beakers from highest to lowest final temperature of the mixture at thermal equilibrium?
| Beaker | Mass of Ice at \(0.0^\circ\text{C}\) | Mass of Liquid Water | Initial Temperature of Liquid Water |
|---|---|---|---|
| X | \(10.0\text{ g}\) | \(70.0\text{ g}\) | \(24.0^\circ\text{C}\) |
| Y | \(10.0\text{ g}\) | \(15.0\text{ g}\) | \(60.0^\circ\text{C}\) |
| Z | \(10.0\text{ g}\) | \(20.0\text{ g}\) | \(25.0^\circ\text{C}\) |
(\(\Delta H_{\text{fus}}\) of ice \(= 336\text{ J/g}\); specific heat capacity of liquid water \(= 4.2\text{ J}/(\text{g}\cdot^\circ\text{C})\))
Which of the following correctly ranks the beakers from highest to lowest final temperature of the mixture at thermal equilibrium?
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