AP Chemistry
6.7 Bond Enthalpies
6.2 Energy Diagrams
6.1 Endothermic and Exothermic Processes
The production of hydrogen gas from natural gas is carried out through the steam-methane reforming process according to the following balanced equation:
\[ \text{CH}_4\text{(g)} + \text{H}_2\text{O(g)} \rightarrow \text{CO(g)} + 3\,\text{H}_2\text{(g)} \]
The average bond enthalpies for the bonds involved in the reaction are given in the table below.
Based on the bond enthalpy data, which of the following correctly classifies the enthalpy change of the reaction, \(\Delta H_{\text{rxn}}^\circ\), and compares the potential energy of the products to that of the reactants?
\[ \text{CH}_4\text{(g)} + \text{H}_2\text{O(g)} \rightarrow \text{CO(g)} + 3\,\text{H}_2\text{(g)} \]
The average bond enthalpies for the bonds involved in the reaction are given in the table below.
| Bond | Average bond enthalpy (\(\text{kJ/mol}\)) |
|---|---|
| \(\text{C}-\text{H}\) | \(410\) |
| \(\text{O}-\text{H}\) | \(460\) |
| \(\text{C}\equiv\text{O}\) | \(1070\) |
| \(\text{H}-\text{H}\) | \(435\) |
Based on the bond enthalpy data, which of the following correctly classifies the enthalpy change of the reaction, \(\Delta H_{\text{rxn}}^\circ\), and compares the potential energy of the products to that of the reactants?
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