---
title: "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.  | 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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url: "https://nerd-notes.com/ubq/123878/"
date_modified: "2026-09-28T12:30:44+00:00"
---

# 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.

| 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?

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.

| 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?

- **A.** \(\text{Beaker Y} > \text{Beaker X} > \text{Beaker Z}\)
- **B.** \(\text{Beaker Y} > \text{Beaker Z} > \text{Beaker X}\)
- **C.** \(\text{Beaker X} > \text{Beaker Y} > \text{Beaker Z}\)
- **D.** \(\text{Beaker X} > \text{Beaker Z} > \text{Beaker Y}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/123878/*