---
title: "A student conducts a calorimetry experiment to heat a sample of liquid water. A stream of gaseous \\(\\text{H}_2\\text{O}\\) (steam) at \\(100.0\\ ^\\circ\\text{C}\\) is bubbled into an insulated flask containing \\(60.0\\text{ g}\\) of liquid water at \\(20.0\\ ^\\circ\\text{C}\\). The steam completely condenses and mixes with the liquid water until the entire system reaches a uniform final temperature of \\(40.0\\ ^\\circ\\text{C}\\).  Assume no heat is lost to the calorimeter or the surroundings. – Specific heat capacity of liquid water: \\(4.18\\text{ J}/(\\text{g}\\cdot^\\circ\\text{C})\\) – Enthalpy of vaporization of water: \\(\\Delta H_{\\text{vap}} = 2.26 \\times 10^3\\text{ J/g}\\)  What is the minimum mass of steam at \\(100.0\\ ^\\circ\\text{C}\\) required to reach the final temperature of \\(40.0\\ ^\\circ\\text{C}\\)?"
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url: "https://nerd-notes.com/ubq/119898/"
date_modified: "2026-08-21T08:17:12+00:00"
---

# A student conducts a calorimetry experiment to heat a sample of liquid water. A stream of gaseous \(\text{H}_2\text{O}\) (steam) at \(100.0\ ^\circ\text{C}\) is bubbled into an insulated flask containing \(60.0\text{ g}\) of liquid water at \(20.0\ ^\circ\text{C}\). The steam completely condenses and mixes with the liquid water until the entire system reaches a uniform final temperature of \(40.0\ ^\circ\text{C}\).

Assume no heat is lost to the calorimeter or the surroundings.
– Specific heat capacity of liquid water: \(4.18\text{ J}/(\text{g}\cdot^\circ\text{C})\)
– Enthalpy of vaporization of water: \(\Delta H_{\text{vap}} = 2.26 \times 10^3\text{ J/g}\)

What is the minimum mass of steam at \(100.0\ ^\circ\text{C}\) required to reach the final temperature of \(40.0\ ^\circ\text{C}\)?

A student conducts a calorimetry experiment to heat a sample of liquid water. A stream of gaseous \(\text{H}_2\text{O}\) (steam) at \(100.0\ ^\circ\text{C}\) is bubbled into an insulated flask containing \(60.0\text{ g}\) of liquid water at \(20.0\ ^\circ\text{C}\). The steam completely condenses and mixes with the liquid water until the entire system reaches a uniform final temperature of \(40.0\ ^\circ\text{C}\).

Assume no heat is lost to the calorimeter or the surroundings.
- Specific heat capacity of liquid water: \(4.18\text{ J}/(\text{g}\cdot^\circ\text{C})\)
- Enthalpy of vaporization of water: \(\Delta H_{\text{vap}} = 2.26 \times 10^3\text{ J/g}\)

What is the minimum mass of steam at \(100.0\ ^\circ\text{C}\) required to reach the final temperature of \(40.0\ ^\circ\text{C}\)?

- **A.** \(2.0\text{ g}\)
- **B.** \(2.2\text{ g}\)
- **C.** \(8.0\text{ g}\)
- **D.** \(20\text{ g}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119898/*