---
title: "| Thermodynamic Property | Value | | :— | :— | | Specific heat capacity of ice, \\(c_{\\text{ice}}\\) | \\(2.1\\text{ J}/(\\text{g}\\cdot^\\circ\\text{C})\\) | | Specific heat capacity of water, \\(c_{\\text{water}}\\) | \\(4.2\\text{ J}/(\\text{g}\\cdot^\\circ\\text{C})\\) | | Specific heat capacity of steam, \\(c_{\\text{steam}}\\) | \\(2.0\\text{ J}/(\\text{g}\\cdot^\\circ\\text{C})\\) | | Enthalpy of fusion, \\(\\Delta H_{\\text{fus}}\\) | \\(330\\text{ J/g}\\) | | Enthalpy of vaporization, \\(\\Delta H_{\\text{vap}}\\) | \\(2260\\text{ J/g}\\) |  A student heats a \\(10.0\\text{ g}\\) sample of solid water (\\(\\text{H}_2\\text{O}\\)) initially at \\(-10.0\\text{ }^\\circ\\text{C}\\) until it is completely converted to steam at \\(110.0\\text{ }^\\circ\\text{C}\\) at a constant pressure of \\(1.0\\text{ atm}\\). Based on the thermodynamic data in the table above, what is the total quantity of thermal energy absorbed by the sample?"
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url: "https://nerd-notes.com/ubq/119758/"
date_modified: "2026-08-21T08:12:14+00:00"
---

# | Thermodynamic Property | Value |
| :— | :— |
| Specific heat capacity of ice, \(c_{\text{ice}}\) | \(2.1\text{ J}/(\text{g}\cdot^\circ\text{C})\) |
| Specific heat capacity of water, \(c_{\text{water}}\) | \(4.2\text{ J}/(\text{g}\cdot^\circ\text{C})\) |
| Specific heat capacity of steam, \(c_{\text{steam}}\) | \(2.0\text{ J}/(\text{g}\cdot^\circ\text{C})\) |
| Enthalpy of fusion, \(\Delta H_{\text{fus}}\) | \(330\text{ J/g}\) |
| Enthalpy of vaporization, \(\Delta H_{\text{vap}}\) | \(2260\text{ J/g}\) |

A student heats a \(10.0\text{ g}\) sample of solid water (\(\text{H}_2\text{O}\)) initially at \(-10.0\text{ }^\circ\text{C}\) until it is completely converted to steam at \(110.0\text{ }^\circ\text{C}\) at a constant pressure of \(1.0\text{ atm}\). Based on the thermodynamic data in the table above, what is the total quantity of thermal energy absorbed by the sample?

| Thermodynamic Property | Value |
| :--- | :--- |
| Specific heat capacity of ice, \(c_{\text{ice}}\) | \(2.1\text{ J}/(\text{g}\cdot^\circ\text{C})\) |
| Specific heat capacity of water, \(c_{\text{water}}\) | \(4.2\text{ J}/(\text{g}\cdot^\circ\text{C})\) |
| Specific heat capacity of steam, \(c_{\text{steam}}\) | \(2.0\text{ J}/(\text{g}\cdot^\circ\text{C})\) |
| Enthalpy of fusion, \(\Delta H_{\text{fus}}\) | \(330\text{ J/g}\) |
| Enthalpy of vaporization, \(\Delta H_{\text{vap}}\) | \(2260\text{ J/g}\) |

A student heats a \(10.0\text{ g}\) sample of solid water (\(\text{H}_2\text{O}\)) initially at \(-10.0\text{ }^\circ\text{C}\) until it is completely converted to steam at \(110.0\text{ }^\circ\text{C}\) at a constant pressure of \(1.0\text{ atm}\). Based on the thermodynamic data in the table above, what is the total quantity of thermal energy absorbed by the sample?

- **A.** \(4.6\text{ kJ}\)
- **B.** \(7.9\text{ kJ}\)
- **C.** \(25.9\text{ kJ}\)
- **D.** \(30.5\text{ kJ}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119758/*