---
title: "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.  | 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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date_modified: "2026-08-19T12:39:52+00:00"
---

# 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.

| 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?

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.

| 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?

- **A.** \(7.8\text{ kJ}\)
- **B.** \(8.2\text{ kJ}\)
- **C.** \(8.5\text{ kJ}\)
- **D.** \(8.9\text{ kJ}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119336/*