At 25 ^$\circ$ C, the Following Heats of Reaction Are Known

At 25 ^$\circ$ C, the following heats of reaction are known:
$\begin{array}{ll}2 \mathrm{ClF}(\mathrm{~g}) +\mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{Cl}_{2} \mathrm{O}(\mathrm{~g}) +\mathrm{F}_{2} \mathrm{O}(\mathrm{~g}) & \Delta \mathrm{H}_{\mathrm{rxn}}^{\circ}=167.4 \mathrm{~kJ} / \mathrm{mol} \\2 \mathrm{ClF}_{3}(\mathrm{~g}) +2 \mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{Cl}_{2} \mathrm{O}(\mathrm{~g}) +3 \mathrm{~F}_{2} \mathrm{O}(\mathrm{~g}) & \Delta \mathrm{H}_{\mathrm{rxn}}^{\circ}=341.4 \mathrm{~kJ} / \mathrm{mol} \\2 \mathrm{~F}_{2}(\mathrm{~g}) +\mathrm{O}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{~F}_{2} \mathrm{O}(\mathrm{~g}) & \Delta \mathrm{H}_{\mathrm{rxn}}^{\circ}=-43.4 \mathrm{~kJ} / \mathrm{mol}\end{array}$
At the same temperature, use the above data to calculate the heat released (kJ) when 3.40 moles of ClF(g) reacts with excess F₂: ClF(g) + F₂(g) $\rarr$ ClF₃(g)

A) 109 kJ
B) 233 kJ
C) 370. kJ
D) 465 kJ
E) 1,580 kJ