---
title: "A student dissolves a sample of solid calcium chloride, \\(\\text{CaCl}_2\\text{(s)}\\), in water contained in an insulated calorimeter. The student observes that the temperature of the water increases from \\(22.0^\\circ\\text{C}\\) to \\(31.0^\\circ\\text{C}\\). Which of the following claims and justifications correctly identifies the thermochemical nature of the dissolution process?"
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url: "https://nerd-notes.com/ubq/119194/"
date_modified: "2026-08-19T12:39:19+00:00"
---

# A student dissolves a sample of solid calcium chloride, \(\text{CaCl}_2\text{(s)}\), in water contained in an insulated calorimeter. The student observes that the temperature of the water increases from \(22.0^\circ\text{C}\) to \(31.0^\circ\text{C}\). Which of the following claims and justifications correctly identifies the thermochemical nature of the dissolution process?

A student dissolves a sample of solid calcium chloride, \(\text{CaCl}_2\text{(s)}\), in water contained in an insulated calorimeter. The student observes that the temperature of the water increases from \(22.0^\circ\text{C}\) to \(31.0^\circ\text{C}\). Which of the following claims and justifications correctly identifies the thermochemical nature of the dissolution process?

- **A.** The process is exothermic because thermal energy flows from the dissolving \(\text{CaCl}_2\) (system) to the water (surroundings).
- **B.** The process is exothermic because thermal energy flows from the water (surroundings) to the dissolving \(\text{CaCl}_2\) (system).
- **C.** The process is endothermic because thermal energy flows from the water (surroundings) to the dissolving \(\text{CaCl}_2\) (system).
- **D.** The process is endothermic because thermal energy flows from the dissolving \(\text{CaCl}_2\) (system) to the water (surroundings).

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119194/*