Estimation of change in enthalpy of a gas phase reaction using bond enthalpies
Use Hess' Law:  $\Delta$H = $\Sigma$ Enthalpy of Bonds Broken - $\Sigma$ Enthalpy of Bonds Formed

Reactants 


Bond enthalpy of C2H4 = 602 + (413 * 4) = 2254 kJ mol-1
Bond enthalpy of O2 = 3 * 498 = 1494 kJ mol-1
$\therefore$ $\Sigma$ Enthalpy of Bonds Broken= 2254 + 1494 = 3748 kJ mol-1


Products


Bond enthalpy of CO2 = (799 * 2) * 2 = 3196 kJ mol-1
Bond enthalpy of H2O = (463 * 2) * 2 = 1852 kJ mol-1
$\therefore \Sigma$ Enthalpy of Bonds Formed = 3196 + 1852 = 5048 kJ mol-1


Overall


$\Delta$H = 3748 - 5048 = -1300 kJ mol-1




After having a quick Google search for the enthalpy change of combustion for ethene, it came up as -1411 kJ mol-1. Our calculated answer isn't far off. I'm hoping we got the same answer.