AP Chemistry
4.5 Stoichiometry
A sample of methane gas, \(\text{CH}_4\text{(g)}\), undergoes complete combustion in the presence of excess oxygen gas, \(\text{O}_2\text{(g)}\), according to the balanced chemical equation below.
\[ \text{CH}_4\text{(g)} + 2\,\text{O}_2\text{(g)} \rightarrow \text{CO}_2\text{(g)} + 2\,\text{H}_2\text{O(g)} \]
If \(16.0\text{ g}\) of \(\text{CH}_4\text{(g)}\) is completely consumed, what is the theoretical yield of \(\text{H}_2\text{O(g)}\)?
\[ \text{CH}_4\text{(g)} + 2\,\text{O}_2\text{(g)} \rightarrow \text{CO}_2\text{(g)} + 2\,\text{H}_2\text{O(g)} \]
If \(16.0\text{ g}\) of \(\text{CH}_4\text{(g)}\) is completely consumed, what is the theoretical yield of \(\text{H}_2\text{O(g)}\)?
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