Calculate the $\Delta H$ for the reaction: $C_2H_4(g) + H_2(g) \rightarrow C_2H_6(g)$, from the following data:



$\begin{array}{ll}

C_2H_4(g) + 3O_2(g) \rightarrow 2CO_2(g) + 2H_2O(l) & \Delta H = -1411\text{ kJ/mole} \\

C_2H_6(g) + 7/2O_2(g) \rightarrow 2CO_2(g) + 3H_2O(l) & \Delta H = -1560.\text{ kJ/mole} \\

H_2(g) + 1/2O_2(g) \rightarrow H_2O(l) & \Delta H = -285.8\text{ kJ/mole}

\end{array}$