---
title: "A student conducts two separate calorimetry trials to investigate the enthalpy of neutralization for the reaction represented by the equation below:  \\[ \\text{HCl(aq)} + \\text{NaOH(aq)} \\rightarrow \\text{NaCl(aq)} + \\text{H}_2\\text{O(l)} \\quad \\Delta H^\\circ_{\\text{rxn}} = -56\\text{ kJ/mol}_{\\text{rxn}} \\]  In each trial, the indicated solutions, initially at \\(22.0\\ ^\\circ\\text{C}\\), are mixed in an insulated calorimeter of negligible heat capacity. Assume that all solutions have a density of \\(1.00\\text{ g/mL}\\) and a specific heat capacity of \\(4.18\\text{ J/(g}\\cdot^\\circ\\text{C)}\\).  | Trial | Volume and concentration of \\(\\text{HCl(aq)}\\) | Volume and concentration of \\(\\text{NaOH(aq)}\\) | Total volume | |—|—|—|—| | 1 | \\(50.0\\text{ mL}\\) of \\(1.0\\text{ M}\\) | \\(50.0\\text{ mL}\\) of \\(1.0\\text{ M}\\) | \\(100.0\\text{ mL}\\) | | 2 | \\(50.0\\text{ mL}\\) of \\(1.0\\text{ M}\\) | \\(50.0\\text{ mL}\\) of \\(2.0\\text{ M}\\) | \\(100.0\\text{ mL}\\) |  Which of the following correctly predicts and explains the relationship between the temperature change in Trial 2, \\(\\Delta T_2\\), and the temperature change in Trial 1, \\(\\Delta T_1\\)?"
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/123799/"
date_modified: "2026-09-28T12:30:21+00:00"
---

# A student conducts two separate calorimetry trials to investigate the enthalpy of neutralization for the reaction represented by the equation below:

\[ \text{HCl(aq)} + \text{NaOH(aq)} \rightarrow \text{NaCl(aq)} + \text{H}_2\text{O(l)} \quad \Delta H^\circ_{\text{rxn}} = -56\text{ kJ/mol}_{\text{rxn}} \]

In each trial, the indicated solutions, initially at \(22.0\ ^\circ\text{C}\), are mixed in an insulated calorimeter of negligible heat capacity. Assume that all solutions have a density of \(1.00\text{ g/mL}\) and a specific heat capacity of \(4.18\text{ J/(g}\cdot^\circ\text{C)}\).

| Trial | Volume and concentration of \(\text{HCl(aq)}\) | Volume and concentration of \(\text{NaOH(aq)}\) | Total volume |
|—|—|—|—|
| 1 | \(50.0\text{ mL}\) of \(1.0\text{ M}\) | \(50.0\text{ mL}\) of \(1.0\text{ M}\) | \(100.0\text{ mL}\) |
| 2 | \(50.0\text{ mL}\) of \(1.0\text{ M}\) | \(50.0\text{ mL}\) of \(2.0\text{ M}\) | \(100.0\text{ mL}\) |

Which of the following correctly predicts and explains the relationship between the temperature change in Trial 2, \(\Delta T_2\), and the temperature change in Trial 1, \(\Delta T_1\)?

A student conducts two separate calorimetry trials to investigate the enthalpy of neutralization for the reaction represented by the equation below:

\[ \text{HCl(aq)} + \text{NaOH(aq)} \rightarrow \text{NaCl(aq)} + \text{H}_2\text{O(l)} \quad \Delta H^\circ_{\text{rxn}} = -56\text{ kJ/mol}_{\text{rxn}} \]

In each trial, the indicated solutions, initially at \(22.0\ ^\circ\text{C}\), are mixed in an insulated calorimeter of negligible heat capacity. Assume that all solutions have a density of \(1.00\text{ g/mL}\) and a specific heat capacity of \(4.18\text{ J/(g}\cdot^\circ\text{C)}\).

| Trial | Volume and concentration of \(\text{HCl(aq)}\) | Volume and concentration of \(\text{NaOH(aq)}\) | Total volume |
|---|---|---|---|
| 1 | \(50.0\text{ mL}\) of \(1.0\text{ M}\) | \(50.0\text{ mL}\) of \(1.0\text{ M}\) | \(100.0\text{ mL}\) |
| 2 | \(50.0\text{ mL}\) of \(1.0\text{ M}\) | \(50.0\text{ mL}\) of \(2.0\text{ M}\) | \(100.0\text{ mL}\) |

Which of the following correctly predicts and explains the relationship between the temperature change in Trial 2, \(\Delta T_2\), and the temperature change in Trial 1, \(\Delta T_1\)?

- **A.** \(\Delta T_2\) will be greater than \(\Delta T_1\) because the greater total initial moles of solute present in Trial 2 increase the frequency of collisions between particles, releasing more thermal energy.
- **B.** \(\Delta T_2\) will be greater than \(\Delta T_1\) because the higher concentration of \(\text{NaOH(aq)}\) provides twice as many moles of \(\text{OH}^-\) ions to react.
- **C.** \(\Delta T_2\) will be approximately equal to \(\Delta T_1\) because the molar heat capacity of the mixture doubles when the concentration of \(\text{NaOH(aq)}\) is doubled.
- **D.** \(\Delta T_2\) will be approximately equal to \(\Delta T_1\) because \(\text{HCl}\) is the limiting reactant in both trials, resulting in the same number of moles of reaction occurring in the same total solution mass.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/123799/*