---
title: "A sample of pure \\(\\text{CaCO}_3\\text{(s)}\\) (molar mass \\(100.\\text{ g/mol}\\)) with a mass of \\(1.00\\text{ g}\\) reacts completely with excess \\(\\text{HCl(aq)}\\) according to the balanced equation below.  \\[ \\text{CaCO}_3\\text{(s)} + 2\\,\\text{HCl(aq)} \\rightarrow \\text{CaCl}_2\\text{(aq)} + \\text{H}_2\\text{O(l)} + \\text{CO}_2\\text{(g)} \\]  Assuming the reaction goes to completion and the gas behaves ideally, what volume of \\(\\text{CO}_2\\text{(g)}\\) is produced at \\(0^\\circ\\text{C}\\) and \\(1.00\\text{ atm}\\)?"
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url: "https://nerd-notes.com/ubq/119653/"
date_modified: "2026-08-21T08:11:57+00:00"
---

# A sample of pure \(\text{CaCO}_3\text{(s)}\) (molar mass \(100.\text{ g/mol}\)) with a mass of \(1.00\text{ g}\) reacts completely with excess \(\text{HCl(aq)}\) according to the balanced equation below.

\[ \text{CaCO}_3\text{(s)} + 2\,\text{HCl(aq)} \rightarrow \text{CaCl}_2\text{(aq)} + \text{H}_2\text{O(l)} + \text{CO}_2\text{(g)} \]

Assuming the reaction goes to completion and the gas behaves ideally, what volume of \(\text{CO}_2\text{(g)}\) is produced at \(0^\circ\text{C}\) and \(1.00\text{ atm}\)?

A sample of pure \(\text{CaCO}_3\text{(s)}\) (molar mass \(100.\text{ g/mol}\)) with a mass of \(1.00\text{ g}\) reacts completely with excess \(\text{HCl(aq)}\) according to the balanced equation below.

\[ \text{CaCO}_3\text{(s)} + 2\,\text{HCl(aq)} \rightarrow \text{CaCl}_2\text{(aq)} + \text{H}_2\text{O(l)} + \text{CO}_2\text{(g)} \]

Assuming the reaction goes to completion and the gas behaves ideally, what volume of \(\text{CO}_2\text{(g)}\) is produced at \(0^\circ\text{C}\) and \(1.00\text{ atm}\)?

- **A.** \(0.224\text{ L}\)
- **B.** \(0.448\text{ L}\)
- **C.** \(2.24\text{ L}\)
- **D.** \(4.48\text{ L}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119653/*