---
title: "A \\(70.0\\text{ g}\\) sample of solid aluminum (specific heat capacity \\(0.90\\text{ J}/(\\text{g}\\cdot^\\circ\\text{C})\\)) is heated to \\(100.0^\\circ\\text{C}\\) in a hot water bath and then quickly transferred into an insulated coffee-cup calorimeter containing \\(60.0\\text{ g}\\) of distilled water (specific heat capacity \\(4.2\\text{ J}/(\\text{g}\\cdot^\\circ\\text{C})\\)) initially at \\(20.0^\\circ\\text{C}\\). Assuming no heat is lost to the calorimeter cup or the surroundings, what is the final temperature of the mixture at thermal equilibrium?"
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url: "https://nerd-notes.com/ubq/121477/"
date_modified: "2026-08-23T05:04:47+00:00"
---

# A \(70.0\text{ g}\) sample of solid aluminum (specific heat capacity \(0.90\text{ J}/(\text{g}\cdot^\circ\text{C})\)) is heated to \(100.0^\circ\text{C}\) in a hot water bath and then quickly transferred into an insulated coffee-cup calorimeter containing \(60.0\text{ g}\) of distilled water (specific heat capacity \(4.2\text{ J}/(\text{g}\cdot^\circ\text{C})\)) initially at \(20.0^\circ\text{C}\). Assuming no heat is lost to the calorimeter cup or the surroundings, what is the final temperature of the mixture at thermal equilibrium?

A \(70.0\text{ g}\) sample of solid aluminum (specific heat capacity \(0.90\text{ J}/(\text{g}\cdot^\circ\text{C})\)) is heated to \(100.0^\circ\text{C}\) in a hot water bath and then quickly transferred into an insulated coffee-cup calorimeter containing \(60.0\text{ g}\) of distilled water (specific heat capacity \(4.2\text{ J}/(\text{g}\cdot^\circ\text{C})\)) initially at \(20.0^\circ\text{C}\). Assuming no heat is lost to the calorimeter cup or the surroundings, what is the final temperature of the mixture at thermal equilibrium?

- **A.** \(16.0^\circ\text{C}\)
- **B.** \(36.0^\circ\text{C}\)
- **C.** \(60.0^\circ\text{C}\)
- **D.** \(84.0^\circ\text{C}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/121477/*