AP Chemistry
6.6 Introduction to Enthalpy of Reaction
The complete combustion of methane is represented by the thermochemical equation below.
\[ \text{CH}_4\text{(g)} + 2\,\text{O}_2\text{(g)} \rightarrow \text{CO}_2\text{(g)} + 2\,\text{H}_2\text{O(l)} \quad \Delta H^\circ_{\text{rxn}} = -890\text{ kJ/mol}_{\text{rxn}} \]
What is the total enthalpy change when \(2.50\text{ mol}\) of \(\text{CH}_4\text{(g)}\) reacts completely with excess oxygen gas?
\[ \text{CH}_4\text{(g)} + 2\,\text{O}_2\text{(g)} \rightarrow \text{CO}_2\text{(g)} + 2\,\text{H}_2\text{O(l)} \quad \Delta H^\circ_{\text{rxn}} = -890\text{ kJ/mol}_{\text{rxn}} \]
What is the total enthalpy change when \(2.50\text{ mol}\) of \(\text{CH}_4\text{(g)}\) reacts completely with excess oxygen gas?
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