\[ \text{C}_2 ext{H}_4\text{(g)} + \text{Cl}_2\text{(g)} \rightarrow \text{C}_2\text{H}_4\text{Cl}_2\text{(g)} \]

Bond	Average bond enthalpy (\(\text{kJ/mol}\))
\(\text{C}-\text{H}\)	\(410\)
\(\text{C}-\text{C}\)	\(350\)
\(\text{C}=\text{C}\)	\(610\)
\(\text{Cl}-\text{Cl}\)	\(240\)
\(\text{C}-\text{Cl}\)	\(330\)

A student investigates the addition reaction between ethene, \(\text{C}_2\text{H}_4\text{(g)}\), and chlorine gas, \(\text{Cl}_2\text{(g)}\), to produce 1,2-dichloroethane, \(\text{C}_2\text{H}_4\text{Cl}_2\text{(g)}\), as represented by the balanced equation above. Based on the average bond enthalpies given in the table, what is the estimated enthalpy change of the reaction, \(\Delta H^\circ_{\text{rxn}}\)?