Given the following equations and ${\mathrm{\Delta H}}^{\circ }$ values, determine the enthalpy of reaction at 298 K for the reaction:
${\mathrm{C}}_2{\mathrm{H}}_4\left(g\right)+6{\mathrm{F}}_2\left(\mathrm{g}\right)⟶2{\mathrm{CF}}_4\left(\mathrm{g}\right)+4\mathrm{HF}\left(g\right)$
$\begin{array}{lc}{\mathrm{H}}_2\left(g\right)+{\mathrm{F}}_2\left(g\right)⟶2\mathrm{HF}\left(g\right);& \mathrm{\Delta }{H}_1^{\circ }=-537\mathrm{kJ}\\ \mathrm{C}\left(s\right)+2{\mathrm{F}}_2\left(g\right)⟶{\mathrm{CF}}_4\left(g\right);& \mathrm{\Delta }{H}_2^{\circ }=-680\mathrm{kJ}\\ 2\mathrm{C}\left(s\right)+2{\mathrm{H}}_2\left(g\right)⟶{\mathrm{C}}_2{\mathrm{H}}_4\left(g\right);& \mathrm{\Delta }{H}_3^{\circ }=52\mathrm{kJ}\end{array}$