AP Chemistry
4.5 Stoichiometry
A student heats a pure limestone sample in a model kiln. The CaCO decomposition occurs according to the equation
\(\text{CaCO}_3\text{(s)} \rightarrow \text{CaO(s)} + \text{CO}_2\text{(g)}\)
The student completely decomposes \(25.0\text{ g}\) of \(\text{CaCO}_3\). The molar mass of \(\text{CaCO}_3\) is \(100.\text{ g/mol}\), and one mole of gas occupies \(22.4\text{ L}\) at standard temperature and pressure. What volume of \(\text{CO}_2\text{(g)}\) is produced at standard temperature and pressure?
\(\text{CaCO}_3\text{(s)} \rightarrow \text{CaO(s)} + \text{CO}_2\text{(g)}\)
The student completely decomposes \(25.0\text{ g}\) of \(\text{CaCO}_3\). The molar mass of \(\text{CaCO}_3\) is \(100.\text{ g/mol}\), and one mole of gas occupies \(22.4\text{ L}\) at standard temperature and pressure. What volume of \(\text{CO}_2\text{(g)}\) is produced at standard temperature and pressure?
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