AP Chemistry
4.5 Stoichiometry
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 \(1.00\text{ atm}\)?
\[ \text{CaCO}_3\text{(s)} + 2\,\text{HCl(aq)} \rightarrow \text{CaCl}_2\text{(aq)} + \text{H}_2\text{O(l)} + \text{CO}_2\text{(g)} \]
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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