Calculate the enthalpy change $(H)$ when a $2\mathrm{.}841g$ sample of benzene, $C_6{H}_6(l)(78\mathrm{.}11\frac{g}{m}ol),$ is burned in excess oxygen to form $C{O}_2(g)$ and $H_{2}O(I)$ in a reaction at constant pressure and $298\mathrm{.}15K.$ Use the following information.

$H_{f}C{O}_2(g)=-393\mathrm{.}51kJ$

$H_f{H}_{2}O(l)=-285\mathrm{.}83kJ$

$H_f{O}_2=0kJ$

$H_f{C}_6{H}_6(l)=49\mathrm{.}03kJ$

A$.+118\mathrm{.}8kJ$

B$.+59\mathrm{.}42kJ$

C$.-118\mathrm{.}8kJ$

D$.+55\mathrm{.}13kJ$

E$.-55\mathrm{.}13kJ$