The hydrogenation of ethene is represented by with an enthalpy change of per mole of…

CHEMISTRY · Subjective · A Level · Chemistry · Energetics · Energetics

Problem

The hydrogenation of ethene is represented by

\text{C}_2\text{H}_4(g)+\text{H}_2(g)\rightarrow\text{C}_2\text{H}_6(g)

with an enthalpy change of

\Delta H= -136\,\text{kJ}

per mole of reaction. Given the following average bond energies:

\text{H--H}: 436\,\text{kJ mol}^{-1}

\text{C--H}: 413\,\text{kJ mol}^{-1}

\text{C--C}: 348\,\text{kJ mol}^{-1}

Determine the average bond energy of the

\text{C} = \text{C}

(double) bond, in

\text{kJ mol}^{-1}