AP Chemistry
6.7 Bond Enthalpies
A student investigates the hydrogenation of ethene to form ethane, represented by the balanced equation below:
\(\text{C}_2\text{H}_4\text{(g)} + \text{H}_2\text{(g)} \rightarrow \text{C}_2\text{H}_6\text{(g)}\)
Based on the average bond enthalpies given in the table, what is the estimated standard enthalpy change, \(\Delta H^\circ_{rxn}\), for the reaction?
\(\text{C}_2\text{H}_4\text{(g)} + \text{H}_2\text{(g)} \rightarrow \text{C}_2\text{H}_6\text{(g)}\)
| Bond | Average Bond Enthalpy (kJ/mol) |
|---|---|
| \(\text{C–C}\) | 348 |
| \(\text{C=C}\) | 614 |
| \(\text{C–H}\) | 413 |
| \(\text{H–H}\) | 436 |
Based on the average bond enthalpies given in the table, what is the estimated standard enthalpy change, \(\Delta H^\circ_{rxn}\), for the reaction?
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