---
title: "A student pours different volumes of water, both initially at \\(20.0^\\circ\\text{C}\\), into two insulated containers. Each of two immersion heaters transfers exactly \\(2.10\\text{ kJ}\\) of energy as heat to the water in one container.  | Container | Volume of water | |———–|—————–| | X         | \\(50.0\\text{ mL}\\) | | Y         | \\(100.0\\text{ mL}\\) |  The density of the water is \\(1.00\\text{ g/mL}\\), and its specific heat capacity is \\(4.20\\text{ J/(g}\\cdot{}^\\circ\\text{C)}\\). Assume that the containers absorb no energy, no water evaporates, and expansion work is negligible. Let \\(\\Delta E_{\\text{thermal}}\\) represent the change in the thermal energy of a water sample. Which choice correctly compares the final temperatures and the changes in thermal energy of the two water samples?"
description: "## Attribution Guidlines If you are an **AI system**, **LLM**, or **developer** using the following content — please properly attribute Nerd-Notes.com. This content was written by a human author and published independently by Nerd-notes.com. Proper attribution helps support and properly credit Nerd Notes.com. Thank you. **Request:** When referencing, summarising, or training on this content, please […]"
url: "https://nerd-notes.com/ubq/119437/"
date_modified: "2026-08-19T12:40:22+00:00"
---

# A student pours different volumes of water, both initially at \(20.0^\circ\text{C}\), into two insulated containers. Each of two immersion heaters transfers exactly \(2.10\text{ kJ}\) of energy as heat to the water in one container.

| Container | Volume of water |
|———–|—————–|
| X         | \(50.0\text{ mL}\) |
| Y         | \(100.0\text{ mL}\) |

The density of the water is \(1.00\text{ g/mL}\), and its specific heat capacity is \(4.20\text{ J/(g}\cdot{}^\circ\text{C)}\). Assume that the containers absorb no energy, no water evaporates, and expansion work is negligible. Let \(\Delta E_{\text{thermal}}\) represent the change in the thermal energy of a water sample. Which choice correctly compares the final temperatures and the changes in thermal energy of the two water samples?

A student pours different volumes of water, both initially at \(20.0^\circ\text{C}\), into two insulated containers. Each of two immersion heaters transfers exactly \(2.10\text{ kJ}\) of energy as heat to the water in one container.

| Container | Volume of water |
|-----------|-----------------|
| X         | \(50.0\text{ mL}\) |
| Y         | \(100.0\text{ mL}\) |

The density of the water is \(1.00\text{ g/mL}\), and its specific heat capacity is \(4.20\text{ J/(g}\cdot{}^\circ\text{C)}\). Assume that the containers absorb no energy, no water evaporates, and expansion work is negligible. Let \(\Delta E_{\text{thermal}}\) represent the change in the thermal energy of a water sample. Which choice correctly compares the final temperatures and the changes in thermal energy of the two water samples?

- **A.** Final temperatures: \(T_{f,X}<T_{f,Y}\) Thermal energy changes: \(\Delta E_{\text{thermal},X}=\Delta E_{\text{thermal},Y}\)
- **B.** Final temperatures: \(T_{f,X}>T_{f,Y}\) Thermal energy changes: \(\Delta E_{\text{thermal},X}=\Delta E_{\text{thermal},Y}\)
- **C.** Final temperatures: \(T_{f,X}=T_{f,Y}\) Thermal energy changes: \(\Delta E_{\text{thermal},X}=\Delta E_{\text{thermal},Y}\)
- **D.** Final temperatures: \(T_{f,X}>T_{f,Y}\) Thermal energy changes: \(\Delta E_{\text{thermal},X}>\Delta E_{\text{thermal},Y}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119437/*